All Related Questions of General Chemistry

Q: Although your textbook lists the rules for converting an ordinary number to

Although your textbook lists the rules for converting an ordinary number to scientific notation, oftentimes students remember such rules better if they put them into their own words. Pretend you are h...

Q: True or false? If a theory is disproven, then all

True or false? If a theory is disproven, then all of the observations that support that theory are also disproven. Explain.

Q: Write each of the following numbers in standard scientific notation.

Write each of the following numbers in standard scientific notation. a. 97,820 b. 42.14 * 103 c. 0.08214 * 10-3 d. 0.0003914 e. 927.1 f. 4.781 * 102 * 10-3

Q: Discuss several political, social, or personal considerations that might affect

Discuss several political, social, or personal considerations that might affect a scientist’s evaluation of a theory. Give examples of how such external forces have influenced scientists in the past....

Q: Although reviewing your lecture notes and reading your textbook are important,

Although reviewing your lecture notes and reading your textbook are important, why does the study of chemistry depend so much on problem solving? Can you learn to solve problems yourself just by looki...

Q: Why is the ability to solve problems important in the study of

Why is the ability to solve problems important in the study of chemistry? Why is it that the method used to attack a problem is as important as the answer to the problem itself?

Q: Students approaching the study of chemistry must learn certain basic facts (

Students approaching the study of chemistry must learn certain basic facts (such as the names and symbols of the most common elements), but it is much more important that they learn to think criticall...

Q: The “Chemistry in Focus” segment Chemistry: An Important Component

The “Chemistry in Focus” segment Chemistry: An Important Component of Your Education discusses how studying chemistry can be beneficial not only in your chemistry courses but in your studies in genera...

Q: Write each of the following numbers in standard scientific notation.

Write each of the following numbers in standard scientific notation. a. 1/0.00032 b. 103/10-3 c. 103/103 d. 1/55,000 e. (105)(104)(10-4)/(10-2) f. 43.2/(4.32 * 10-5) g. (4.32 * 10-5)/432 h. 1/(...

Q: Write each of the following numbers as “ordinary” decimal numbers

Write each of the following numbers as “ordinary” decimal numbers. a. 6.244 * 103 b. 9.117 * 10-2 c. 8.299 * 101 d. 1.771 * 10-4 e. 5.451 * 102 f. 2.934 * 10-5

Q: You want to cook some raw noodles to make a pasta dish

You want to cook some raw noodles to make a pasta dish for supper. So, you turn on the gas stovetop (which uses a flame), place a large pot of water over the flame, wait for the water to boil, place t...

Q: This section presents several ways our day-to-day lives

This section presents several ways our day-to-day lives have been enriched by chemistry. List three materials or processes involving chemistry that you feel have contributed to such an enrichment, and...

Q: Classify each of the following as a physical or chemical change or

Classify each of the following as a physical or chemical change or property. a. Oven cleaners contain sodium hydroxide, which converts the grease/oil spatters inside the oven to water-soluble materia...

Q: Classify each of the following as a physical or chemical change or

Classify each of the following as a physical or chemical change or property. a. A fireplace poker glows red when you heat it in the fire. b. A marshmallow turns black when toasted too long in a camp...

Q: Consider three 10-g samples of water: one as ice

Consider three 10-g samples of water: one as ice, one as liquid, and one as vapor. How do the volumes of these three samples compare with one another? How is this difference in volume related to the p...

Q: Do the proton and the neutron have exactly the same mass?

Do the proton and the neutron have exactly the same mass? How do the masses of the proton and the neutron compare to the mass of the electron? Which particles make the greatest contribution to the mas...

Q: The symbols for most elements are based on the first few letters

The symbols for most elements are based on the first few letters of the respective element’s common English name. In some cases, however, the symbol seems to have nothing to do with the element’s comm...

Q: Several chemical elements have English names beginning with the letters B,

Several chemical elements have English names beginning with the letters B, N, P, or S. For each letter, list the English names for two elements whose names begin with that letter, and give the symbols...

Q: Correct each of the following misstatements from Dalton’s atomic theory.

Correct each of the following misstatements from Dalton’s atomic theory. a. Elements are made of tiny particles called molecules. b. All atoms of a given element are very similar. c. The atoms of a...

Q: A given compound always contains the same relative masses of its constituent

A given compound always contains the same relative masses of its constituent elements. How is this related to the relative numbers of each kind of atom present?

Q: In lab you report a measured volume of 158.6 mL

In lab you report a measured volume of 158.6 mL of water. Using significant figures as a measure of the error, what range of answers does your reported volume imply? Choose the best answer and justify...

Q: For the pin shown in Fig. 2.5, why

For the pin shown in Fig. 2.5, why is the third figure determined for the length of the pin uncertain? Considering that the third figure is uncertain, explain why the length of the pin is indicated as...

Q: Compare and contrast the ease with which molecules are able to move

Compare and contrast the ease with which molecules are able to move relative to each other in the three states of matter.

Q: Scientists J. J. Thomson and William Thomson (Lord Kelvin

Scientists J. J. Thomson and William Thomson (Lord Kelvin) made numerous contributions to our understanding of the atom’s structure. a. Which subatomic particle did J. J. Thomson discover, and what d...

Q: Dalton’s original atomic theory proposed that all atoms of a given element

Dalton’s original atomic theory proposed that all atoms of a given element are identical. Did this turn out to be true after further experimentation was carried out? Explain.

Q: Describe how the process of filtration could be used to separate a

Describe how the process of filtration could be used to separate a mixture into its components. Give an example.

Q: In a common laboratory experiment in general chemistry, students are asked

In a common laboratory experiment in general chemistry, students are asked to determine the relative amounts of benzoic acid and charcoal in a solid mixture. Benzoic acid is relatively soluble in hot...

Q: Of the following isotopes, which are isotopes of the same element

Of the following isotopes, which are isotopes of the same element?

Q: You are asked to determine the perimeter of the cover of your

You are asked to determine the perimeter of the cover of your textbook. You measure the length as 34.29 cm and the width as 26.72 cm. How many significant figures should you report for the perimeter?...

Q: Evaluate each of the following mathematical expressions, and express the answer

Evaluate each of the following mathematical expressions, and express the answer to the correct number of significant digits. a. 44.2124 + 0.81 + 7.335 b. 9.7789 + 3.3315 - 2.21 c. 0.8891 + 0.225 +...

Q: Evaluate each of the following mathematical expressions, and express the answer

Evaluate each of the following mathematical expressions, and express the answer to the correct number of significant digits. a. (4.771 + 2.3)/3.1 b. 5.02 * 102 + 4.1 * 102 c. 1.091 * 103 + 2.21 * 1...

Q: Classify each of the following as a physical or chemical change or

Classify each of the following as a physical or chemical change or property. a. Milk curdles if a few drops of lemon juice are added to it. b. Butter turns rancid if it is left exposed at room tempe...

Q: Without actually performing the calculations indicated, tell to how many significant

Without actually performing the calculations indicated, tell to how many significant digits the answer to the calculation should be expressed. b. (67.41 + 0.32 + 1.98)/(18.225) c. (2.001 * 10-3)(4.7...

Q: We use chemical reactions in our everyday lives, too, not

We use chemical reactions in our everyday lives, too, not just in the science laboratory. Give at least five examples of chemical transformations that you use in your daily activities. Indicate what t...

Q: Under ordinary conditions, only a few pure elements occur as liquids

Under ordinary conditions, only a few pure elements occur as liquids. Give an example of a metallic and a nonmetallic element that ordinarily occur as liquids.

Q: Evaluate each of the following and write the answer to the appropriate

Evaluate each of the following and write the answer to the appropriate number of significant figures. a. (2.0944 + 0.0003233 + 12.22)/(7.001) b. (1.42 * 102 + 1.021 * 103)/(3.1 * 10-1) c. (9.762 *...

Q: Oxygen forms molecules in which there are two oxygen atoms, O2

Oxygen forms molecules in which there are two oxygen atoms, O2. Phosphorus forms molecules in which there are four phosphorus atoms, P4. Does this mean that O2 and P4 are “compounds” because they cont...

Q: Perform each of the following conversions, being sure to set up

Perform each of the following conversions, being sure to set up the appropriate conversion factor in each case. a. 12.5 in. to centimeters b. 12.5 cm to inches c. 2513 ft to miles d. 4.53 ft to me...

Q: Perform each of the following conversions, being sure to set up

Perform each of the following conversions, being sure to set up the appropriate conversion factor in each case. a. 2.23 m to yards b. 46.2 yd to meters c. 292 cm to inches d. 881.2 in. to centimete...

Q: Perform each of the following conversions, being sure to set up

Perform each of the following conversions, being sure to set up the appropriate conversion factor in each case. a. 1.75 mi to kilometers b. 2.63 gal to quarts c. 4.675 calories to joules d. 756.2...

Q: Perform each of the following conversions, being sure to set up

Perform each of the following conversions, being sure to set up the appropriate conversion factor in each case. a. 254.3 g to kilograms b. 2.75 kg to grams c. 2.75 kg to pounds d. 2.75 kg to ounce...

Q: For the masses and volumes indicated, calculate the density in grams

For the masses and volumes indicated, calculate the density in grams per cubic centimeter. a. mass = 452.1 g; volume = 292 cm3 b. mass = 0.14 lb; volume = 125 mL c. mass = 1.01 kg; volume = 1000 cm...

Q: List the names, symbols, and atomic numbers of the top

List the names, symbols, and atomic numbers of the top four elements in Groups 1, 2, 6, and 7.

Q: Which subatomic particles contribute most to the atom’s mass? Which subatomic

Which subatomic particles contribute most to the atom’s mass? Which subatomic particles determine the atom’s chemical properties?

Q: Read the “Chemistry in Focus” segment A Mystifying Problem,

Read the “Chemistry in Focus” segment A Mystifying Problem, and discuss how David and Susan analyzed the situation, arriving at the theory that the lead glaze on the pottery was responsible for their...

Q: Is it possible for the same two elements to form more than

Is it possible for the same two elements to form more than one compound? Is this consistent with Dalton’s atomic theory? Give an example.

Q: Iron has a density of 7.87 g/cm3.

Iron has a density of 7.87 g/cm3. If 52.4 g of iron is added to 75.0 mL of water in a graduated cylinder, to what volume reading will the water level in the cylinder rise?

Q: You want to make a rectangular box that weighs 2.0

You want to make a rectangular box that weighs 2.0 pounds and floats on water. The width and height of the box are each 5.0 cm long. Choose the minimum length of the box that will keep it afloat on th...

Q: The principal goal of alchemists was to convert cheaper, more common

The principal goal of alchemists was to convert cheaper, more common metals into gold. Considering that gold had no particular practical uses (for example, it was too soft to be used for weapons), why...

Q: Express each of the following as an “ordinary” decimal number

Express each of the following as an “ordinary” decimal number. a. 3.011 * 1023 e. 4.32002 * 10-4 b. 5.091 * 109 f. 3.001 * 10-2 c. 7.2 * 102 g. 2.9901 * 10-7 d. 1.234 * 105 h. 4.2 * 10-1

Q: Make the following conversions. a. 1.25 in

Make the following conversions. a. 1.25 in. to feet and to centimeters b. 2.12 qt to gallons and to liters c. 2640 ft to miles and to kilometers d. 1.254 kg lead to its volume in cubic centimeters...

Q: A metal ion with a 2+ charge contains 34 neutrons and

A metal ion with a 2+ charge contains 34 neutrons and 27 electrons. Identify the metal ion and determine its mass number.

Q: Which of the following statements is (are) true?

Which of the following statements is (are) true? a. A 1.00-liter bottle contains more soda than a 1.00-quart bottle. b. A man who is 1.52 m tall is taller than a woman who is 5 ft 3 in. tall. c. A...

Q: Express each of the following numbers in scientific (exponential) notation

Express each of the following numbers in scientific (exponential) notation. a. 529 b. 240,000,000 c. 301,000,000,000,000,000 d. 78,444 e. 0.0003442 f. 0.000000000902 g. 0.043 h. 0.0821

Q: Express each of the following as an “ordinary” decimal number

Express each of the following as an “ordinary” decimal number. a. 2.98 * 10-5 b. 4.358 * 109 c. 1.9928 * 10-6 d. 6.02 * 10-3 e. 1.01 * 10-1 f. 7.87 * 10-3 g. 9.87 * 107 h. 3.7899 * 102 i. 1.0...

Q: Rewrite each of the following as an “ordinary” decimal number

Rewrite each of the following as an “ordinary” decimal number. a. 2.789 * 103 b. 2.789 * 10-3 c. 9.3 * 107 d. 4.289 * 101 e. 9.999 * 104 f. 9.999 * 10-5

Q: Write each of the following numbers in standard scientific notation.

Write each of the following numbers in standard scientific notation. a. 102.3 * 10-5 b. 32.03 * 10-3 c. 59933 * 102 d. 599.33 * 104 e. 5993.3 * 103 f. 2054 * 10-1 g. 32,000,000 * 10-6 h. 59.93...

Q: Evaluate each of the following, and write the answer to the

Evaluate each of the following, and write the answer to the appropriate number of significant figures. a. 149.2 + 0.034 + 2000.34 b. 1.0322 * 103 + 4.34 * 103 c. 4.03 * 10-2 - 2.044 * 10-3 d. 2.09...

Q: Evaluate each of the following, and write the answer to the

Evaluate each of the following, and write the answer to the appropriate number of significant figures. a. (0.0432)(2.909)(4.43 * 108) b. (0.8922)/[(0.00932)(4.03 * 102)] c. (3.923 * 102)(2.94)(4.09...

Q: Evaluate each of the following, and write the answer to the

Evaluate each of the following, and write the answer to the appropriate number of significant figures. a. (2.9932 * 104)[2.4443 * 102 + 1.0032 * 101] b. [2.34 * 102 + 2.443 * 10-1]/(0.0323) c. (4.3...

Q: Perform each of the following conversions, being sure to set up

Perform each of the following conversions, being sure to set up clearly the appropriate conversion factor in each case. a. 8.43 cm to millimeters b. 2.41 * 102 cm to meters c. 294.5 nm to centimete...

Q: For the masses and volumes indicated, calculate the density in grams

For the masses and volumes indicated, calculate the density in grams per cubic centimeter. a. mass = 234 g; volume = 2.2 cm3 b. mass = 2.34 kg; volume = 2.2 m3 c. mass = 1.2 lb; volume = 2.1 ft3 d....

Q: The “Chemistry in Focus” segment Critical Units! discusses the

The “Chemistry in Focus” segment Critical Units! discusses the importance of unit conversions. Read the segment and make the proper unit conversions to answer the following questions. a. The Mars Cli...

Q: Read the “Chemistry in Focus” segment Measurement: Past,

Read the “Chemistry in Focus” segment Measurement: Past, Present, and Future and answer the following questions. a. Give three examples of how developing sophisticated measuring devices is useful in...

Q: Express each of the following numbers in standard scientific notation.

Express each of the following numbers in standard scientific notation. a. 0.5012 b. 5,012,000 c. 0.000005012 d. 5.012 e. 5012 f. 0.005012

Q: What similarities are there between the solid and liquid states of matter

What similarities are there between the solid and liquid states of matter? What differences are there between these two states?

Q: Sketch a flowchart of the steps in the scientific method. Then

Sketch a flowchart of the steps in the scientific method. Then define each part of the method.

Q: A represents a quantitative observation.

A represents a quantitative observation.

Q: By how many places must the decimal point be moved, and

By how many places must the decimal point be moved, and in which direction, to convert each of the following to standard scientific notation? a. 5993 b. -72.14 c. 0.00008291 d. 62.357 e. 0.01014...

Q: For the measurement 0.003040 meters, indicate which (if

For the measurement 0.003040 meters, indicate which (if any) zeros are significant and which (if any) are not significant. Account for all five zeros in the measurement, and explain your reasoning.

Q: What is a compound? What are compounds composed of? What

What is a compound? What are compounds composed of? What is true about the composition of a compound, no matter where we happen to find the compound?

Q: On the planet Xgnu, the most common units of length are

On the planet Xgnu, the most common units of length are the blim (for long distances) and the kryll (for shorter distances). Because the Xgnuese have 14 fingers, perhaps it is not surprising that 1400...

Q: You pass a road sign saying “New York 110 km.”

You pass a road sign saying “New York 110 km.” If you drive at a constant speed of 100. km/h, how long should it take you to reach New York?

Q: Certain elements have special affinities for other elements. This causes them

Certain elements have special affinities for other elements. This causes them to bind together in special ways to form .

Q: Suppose your car is rated at 45 mi/gal for highway

Suppose your car is rated at 45 mi/gal for highway use and 38 mi/gal for city driving. If you wanted to write your friend in Spain about your car’s mileage, what ratings in kilometers per liter would...

Q: You are in Paris, and you want to buy some peaches

You are in Paris, and you want to buy some peaches for lunch. The sign in the fruit stand indicates that peaches are 2.76 euros per kilogram. Given that there are approximately 1.44 euros to the dolla...

Q: For a pharmacist dispensing pills or capsules, it is often easier

For a pharmacist dispensing pills or capsules, it is often easier to weigh the medication to be dispensed rather than to count the individual pills. If a single antibiotic capsule weighs 0.65 g, and a...

Q: On the planet Xgnu, the natives have 14 fingers. On

On the planet Xgnu, the natives have 14 fingers. On the official Xgnuese temperature scale (°X), the boiling point of water (under an atmospheric pressure similar to earth’s) is 140 °X, whereas water...

Q: For a material to float on the surface of water, the

For a material to float on the surface of water, the material must have a density less than that of water (1.0 g/mL) and must not react with the water or dissolve in it. A spherical ball has a radius...

Q: Elemental bromine is a dense, dark-red, pungent-

Elemental bromine is a dense, dark-red, pungent-smelling liquid. Are these characteristics of elemental bromine physical or chemical properties?

Q: A gas cylinder having a volume of 10.5 L contains

A gas cylinder having a volume of 10.5 L contains 36.8 g of gas. What is the density of the gas?

Q: Using Table 2.8, calculate the volume of 25.

Using Table 2.8, calculate the volume of 25.0 g of each of the following: a. hydrogen gas (at 1 atmosphere pressure) b. mercury c. lead d. water

Q: Ethanol and benzene dissolve in each other. When 100. mL

Ethanol and benzene dissolve in each other. When 100. mL of ethanol is dissolved in 1.00 L of benzene, what is the mass of the mixture? (See Table 2.8.)

Q: When 2891 is written in scientific notation, the exponent indicating the

When 2891 is written in scientific notation, the exponent indicating the power of 10 is .

Q: For each of the following numbers, if the number is rewritten

For each of the following numbers, if the number is rewritten in scientific notation, will the exponent of the power of 10 be positive, negative, or zero? a. 1/103 b. 0.00045 c. 52,550 d. 7.21 e....

Q: For each of the following numbers, if the number is rewritten

For each of the following numbers, if the number is rewritten in scientific notation, will the exponent of the power of 10 be positive, negative, or zero? a. 4,915,442 b. 1/1000 c. 0.001 d. 3.75

Q: For each of the following numbers, by how many places does

For each of the following numbers, by how many places does the decimal point have to be moved to express the number in standard scientific notation? In each case, is the exponent positive or negative?...

Q: For each of the following numbers, by how many places must

For each of the following numbers, by how many places must the decimal point be moved to express the number in standard scientific notation? In each case, will the exponent be positive, negative, or z...

Q: For each of the following numbers, by how many places must

For each of the following numbers, by how many places must the decimal point be moved to express the number in standard scientific notation? In each case, will the exponent be positive, negative, or z...

Q: can be broken down into the component elements by chemical changes

can be broken down into the component elements by chemical changes.

Q: Is the process represented below a physical or chemical change?

Is the process represented below a physical or chemical change?

Q: The composition of a given pure compound is always no matter what

The composition of a given pure compound is always no matter what the source of the compound.

Q: Which of the following are considered compounds (as opposed to elements

Which of the following are considered compounds (as opposed to elements)? a. He b. F2 c. HCl d. S8

Q: Write each of the following numbers in standard scientific notation. See

Write each of the following numbers in standard scientific notation. See the Appendix if you need help multiplying or dividing numbers with exponents. a. 1/102 b. 1/10-2 c. 55/103 d. (3.1 * 106)/1...

Q: The fundamental unit of length or distance in the metric system is

The fundamental unit of length or distance in the metric system is the .

Q: Draw a piece of lab glassware that can appropriately measure the volume

Draw a piece of lab glassware that can appropriately measure the volume of a liquid as 32.87 mL.

Q: Which distance is farther, 100 km or 50 mi?

Which distance is farther, 100 km or 50 mi?

Q: 1 L = dm3 = cm3 = mL

1 L = dm3 = cm3 = mL

Q: The volume 0.250 L could also be expressed as mL

The volume 0.250 L could also be expressed as mL.

Q: The distance 10.5 cm could also be expressed as m

The distance 10.5 cm could also be expressed as m.

Q: Would an automobile moving at a constant speed of 100 km/

Would an automobile moving at a constant speed of 100 km/h violate a 65-mph speed limit?

Q: Write each of the following numbers in standard scientific notation.

Write each of the following numbers in standard scientific notation. a. 1/1033 b. 1/105 c. 1/10-7 d. 1/0.0002 e. 1/3,093,000 f. 1/10-4 g. 1/109 h. 1/0.000015

Q: Which weighs more, 0.001 g of water or 1

Which weighs more, 0.001 g of water or 1 mg of water?

Q: Which weighs more, 4.25 g of gold or 425

Which weighs more, 4.25 g of gold or 425 mg of gold?

Q: The length 500 m can also be expressed as nm.

The length 500 m can also be expressed as nm.

Q: A perfect cube of unknown elemental composition has a length of 1

A perfect cube of unknown elemental composition has a length of 1.40 m on each side. The mass of the cube is 21.57 Mg (megagrams). Using this information and Table 2.8, determine the metal used to pre...

Q: You are working on a project where you need the volume of

You are working on a project where you need the volume of a box. You take the length, height, and width measurements and then multiply the values together to find the volume. You report the volume of...

Q: Indicate the number of significant figures in each of the following:

Indicate the number of significant figures in each of the following: a. This book contains over 500 pages. b. A mile is just over 5000 ft. c. A liter is equivalent to 1.059 qt. d. The population o...

Q: Round off each of the following numbers to three significant digits.

Round off each of the following numbers to three significant digits. a. 0.00042557 b. 4.0235 * 10-5 c. 5,991,556 d. 399.85 e. 0.0059998

Q: Round off each of the following numbers to the indicated number of

Round off each of the following numbers to the indicated number of significant digits. a. 0.75555 to four digits b. 292.5 to three digits c. 17.005 to four digits d. 432.965 to five digits

Q: If iron filings are placed with excess powdered sulfur in a beaker

If iron filings are placed with excess powdered sulfur in a beaker, the iron filings are still attracted by a magnet and could be separated from the sulfur with the magnet. Would this combination of i...

Q: If the combination of iron filings and sulfur in Question 25 is

If the combination of iron filings and sulfur in Question 25 is heated strongly, the iron reacts with the sulfur to form a solid that is no longer attracted by the magnet. Would this still represent a...

Q: (For Exercises 13–14) Magnesium metal is very malleable

(For Exercises 13–14) Magnesium metal is very malleable and is able to be pounded and stretched into long, thin, narrow “ribbons” that are often used in the introductory chemistry lab as a source of t...

Q: What does it mean to say that a solution is a homogeneous

What does it mean to say that a solution is a homogeneous mixture?

Q: Given that 1 L = 1000 cm3, determine what conversion factor

Given that 1 L = 1000 cm3, determine what conversion factor is appropriate to convert 350 cm3 to liters; to convert 0.200 L to cubic centimeters.

Q: A rectangular solid measures 1.0 m by 2.4

A rectangular solid measures 1.0 m by 2.4 mm by 3.9 dm. What is the volume in liters?

Q: Which of the following substances is(are) homogeneous mixture(

Which of the following substances is(are) homogeneous mixture(s)? a. chocolate chip cookie b. iodine crystals (I2) c. air (in this room) d. gasoline (for a car) e. sucrose, C12H22O11 (commonly fo...

Q: Perform each of the following conversions, being sure to set up

Perform each of the following conversions, being sure to set up clearly the appropriate conversion factor(s) in each case. a. 908 oz to kilograms b. 12.8 L to gallons c. 125 mL to quarts d. 2.89 g...

Q: The mean distance from the earth to the sun is 9.

The mean distance from the earth to the sun is 9.3 3 107 mi. What is this distance in kilometers? in centimeters?

Q: Given that one metric ton = 1000 kg, how many metric

Given that one metric ton = 1000 kg, how many metric tons are in 5.3 3 103 lb?

Q: Convert the following temperatures to kelvins. a. 0 °

Convert the following temperatures to kelvins. a. 0 °C b. 25 °C c. 37 °C d. 100 °C e. 2175 °C f. 212 °C

Q: Carry out the indicated temperature conversions. a. 175 °

Carry out the indicated temperature conversions. a. 175 °F to kelvins b. 255 K to Celsius degrees c. 245 °F to Celsius degrees d. 125 °C to Fahrenheit degrees

Q: Classify the following as mixtures or pure substances. a.

Classify the following as mixtures or pure substances. a. the vegetable soup you had for lunch b. the fertilizer your dad spreads on the front lawn in the spring c. the salt you sprinkle on your Fr...

Q: What are the fundamental units of mass, length, and temperature

What are the fundamental units of mass, length, and temperature in the metric system?

Q: A sample of a liquid solvent has a density of 0.

A sample of a liquid solvent has a density of 0.915 g/mL. What is the mass of 85.5 mL of the liquid?

Q: An organic solvent has a density of 1.31 g/

An organic solvent has a density of 1.31 g/mL. What volume is occupied by 50.0 g of the liquid?

Q: A solid metal sphere has a volume of 4.2 ft3

A solid metal sphere has a volume of 4.2 ft3. The mass of the sphere is 155 lb. Find the density of the metal sphere in grams per cubic centimeter.

Q: A sample containing 33.42 g of metal pellets is poured

A sample containing 33.42 g of metal pellets is poured into a graduated cylinder initially containing 12.7 mL of water, causing the water level in the cylinder to rise to 21.6 mL. Calculate the densit...

Q: Convert the following temperatures to Fahrenheit degrees. a. 25

Convert the following temperatures to Fahrenheit degrees. a. 25 °C b. 273 K d. 0 K c. 2196 °C e. 86 °C f. 2273 °C

Q: For each of the following descriptions, identify the power of 10

For each of the following descriptions, identify the power of 10 being indicated by the prefix in the measurement. a. The sign on the interstate highway says to tune my AM radio to 540 kilohertz for...

Q: Of the three states of matter, and are not very compressible

Of the three states of matter, and are not very compressible.

Q: Read the “Chemistry in Focus” segment Concrete—An Ancient

Read the “Chemistry in Focus” segment Concrete—An Ancient Material Made New and classify concrete as an element, a mixture, or a compound. Defend your answer.

Q: The “Chemistry in Focus” segment Measurement: Past, Present

The “Chemistry in Focus” segment Measurement: Past, Present, and Future states that hormones can be detected to a level of 1028 g/L. Convert this level to units of pounds per gallon.

Q: Complete the following table: /

Complete the following table:

Q: Give the metric prefix that corresponds to each of the following:

Give the metric prefix that corresponds to each of the following: a. 1000 b. 10-3 c. 10-9 d. 1,000,000 e. 10-1 f. 10-6

Q: For each of the mathematical expressions given: a. Tell

For each of the mathematical expressions given: a. Tell the correct number of significant figures for the answer. b. Evaluate the mathematical expression using correct significant figures in the res...

Q: The longest river in the world is the Nile River with a

The longest river in the world is the Nile River with a length of 4145 mi. How long is the Nile in cable lengths, meters, and nautical miles? Use these exact conversions to help solve the problem: 6...

Q: Secretariat is known as the horse with the fastest run in the

Secretariat is known as the horse with the fastest run in the Kentucky Derby. If Secretariat’s record 1.25-mi run lasted 1 minute 59.2 seconds, what was his average speed in m/s?

Q: A friend tells you that it is 69.1 °F

A friend tells you that it is 69.1 °F outside. What is this temperature in Celsius?

Q: The hottest temperature recorded in the United States is 134 °F

The hottest temperature recorded in the United States is 134 °F in Greenland Ranch, California. The melting point of phosphorus is 44 °C. At this temperature, would phosphorus be a liquid or a solid?...

Q: The density of osmium (the densest metal) is 22.

The density of osmium (the densest metal) is 22.57 g/cm3. What is the mass of a block of osmium with dimensions 1.84 cm * 3.61 cm * 2.10 cm?

Q: The radius of a neon atom is 69 pm, and its

The radius of a neon atom is 69 pm, and its mass is 3.35 3 10223 g. What is the density of the atom in grams per cubic centimeter (g/cm3)? Assume the atom is a sphere with volume=4/3πr3.

Q: Describe how the process of distillation could be used to separate a

Describe how the process of distillation could be used to separate a solution into its component substances. Give an example.

Q: During a filtration or distillation experiment, we separate a mixture into

During a filtration or distillation experiment, we separate a mixture into its individual components. Do the chemical identities of the components of the mixture change during such a process? Explain....

Q: If powdered elemental zinc and powdered elemental sulfur are poured into a

If powdered elemental zinc and powdered elemental sulfur are poured into a metal beaker and then heated strongly, a very vigorous chemical reaction takes place, and the zinc sulfide...

Q: Students often have trouble relating measurements in the metric system to the

Students often have trouble relating measurements in the metric system to the English system they have grown up with. Give the approximate English system equivalents for each of the following metric s...

Q: Classify each of the following as a(n) element,

Classify each of the following as a(n) element, compound, pure substance, homogeneous mixture, and/or heterogeneous mixture. More than one classification is possible, and not all of them may be used....

Q: If a piece of hard, white blackboard chalk is heated strongly

If a piece of hard, white blackboard chalk is heated strongly in a flame, the mass of the piece of chalk will decrease, and eventually the chalk will crumble into a fine white dust. Does this change s...

Q: has a definite volume but takes the shape of its container

has a definite volume but takes the shape of its container.

Q: During a very cold winter, the temperature may remain below freezing

During a very cold winter, the temperature may remain below freezing for extended periods. However, fallen snow can still disappear, even though it cannot melt. This is possible because a solid can va...

Q: Discuss the similarities and differences between a liquid and a gas.

Discuss the similarities and differences between a liquid and a gas.

Q: True or false? Salad dressing (such as oil and vinegar

True or false? Salad dressing (such as oil and vinegar dressing) separating into layers after standing is an example of a chemical change because the end result looks different from how it started. Ex...

Q: The fact that solutions of potassium chromate are bright yellow is an

The fact that solutions of potassium chromate are bright yellow is an example of a property.

Q: Solutions containing nickel(II) ion are usually bright green in

Solutions containing nickel(II) ion are usually bright green in color. When potassium hydroxide is added to such a nickel(II) solution, a pale-green fluffy solid forms and settles out of the solution....

Q: Solutions containing nickel(II) ion are usually bright green in

Solutions containing nickel(II) ion are usually bright green in color. When potassium hydroxide is added to such a nickel(II) solution, a pale-green fluffy solid forms and settles out of the solution....

Q: Classify the following mixtures as homogeneous or heterogeneous. a.

Classify the following mixtures as homogeneous or heterogeneous. a. potting soil b. white wine c. your sock drawer d. window glass e. granite

Q: Students often have trouble relating measurements in the metric system to the

Students often have trouble relating measurements in the metric system to the English system they have grown up with. Give the approximate English system equivalents for each of the following metric s...

Q: True or false? Mixtures always result in a chemical reaction because

True or false? Mixtures always result in a chemical reaction because they consist of two or more substances and thus combine to create a new product.

Q: Distillation and filtration are important methods for separating the components of mixtures

Distillation and filtration are important methods for separating the components of mixtures. Suppose we had a mixture of sand, salt, and water. Describe how filtration and distillation could be used s...

Q: Matter in the state has no shape and fills completely whatever container

Matter in the state has no shape and fills completely whatever container holds it.

Q: Which of the following describes a chemical property? a.

Which of the following describes a chemical property? a. The density of iron is 7.87 g/cm3. b. A platinum wire glows red when heated. c. An iron bar rusts. d. Aluminum is a silver-colored metal.

Q: Which of the following describes a physical change? a.

Which of the following describes a physical change? a. Paper is torn into several smaller pieces. b. Two clear solutions are mixed together to produce a yellow solid. c. A match burns in the air....

Q: A given compound always contains the same proportion (by mass)

A given compound always contains the same proportion (by mass) of the elements. This principle became known as .

Q: Several elements have chemical symbols beginning with the letter N. For

Several elements have chemical symbols beginning with the letter N. For each of the following chemical symbols, give the name of the corresponding element. a. Ne b. Ni c. N d. No e. Np f. Nb g....

Q: What is a compound?

What is a compound?

Q: Find the symbol in Column 2 for each name in Column 1

Find the symbol in Column 2 for each name in Column 1.

Q: Based on the following word descriptions, write the formula for each

Based on the following word descriptions, write the formula for each of the indicated substances. a. a compound whose molecules each contain six carbon atoms and six hydrogen atoms b. an aluminum co...

Q: Students often have trouble relating measurements in the metric system to the

Students often have trouble relating measurements in the metric system to the English system they have grown up with. Give the approximate English system equivalents for each of the following metric s...

Q: Based on the following word descriptions, write the formula for each

Based on the following word descriptions, write the formula for each of the indicated substances. a. a compound whose molecules contain twice as many oxygen atoms as carbon atoms b. a compound whose...

Q: True or false? Rutherford’s bombardment experiments with metal foil suggested that

True or false? Rutherford’s bombardment experiments with metal foil suggested that the a particles were being deflected by coming near a large, positively charged atomic nucleus.

Q: Where are neutrons found in an atom? Are neutrons positively charged

Where are neutrons found in an atom? Are neutrons positively charged, negatively charged, or electrically uncharged?

Q: What are the positively charged particles found in the nuclei of atoms

What are the positively charged particles found in the nuclei of atoms called?

Q: The proton and the (electron/neutron) have almost equal

The proton and the (electron/neutron) have almost equal masses. The proton and the (electron/neutron) have charges that are equal in magnitude but opposite in nature.

Q: An average atomic nucleus has a diameter of about m.

An average atomic nucleus has a diameter of about m.

Q: Which particles in an atom are most responsible for the chemical properties

Which particles in an atom are most responsible for the chemical properties of the atom? Where are these particles located in the atom?

Q: Explain what we mean when we say that a particular element consists

Explain what we mean when we say that a particular element consists of several isotopes.

Q: True or false? The mass number of a nucleus represents the

True or false? The mass number of a nucleus represents the number of protons in the nucleus.

Q: For an isolated atom, why do we expect the number of

For an isolated atom, why do we expect the number of electrons present in the atom to be the same as the number of protons in the nucleus of the atom?

Q: What is the chief factor that determines the physical state of a

What is the chief factor that determines the physical state of a sample of matter?

Q: Students often have trouble relating measurements in the metric system to the

Students often have trouble relating measurements in the metric system to the English system they have grown up with. Give the approximate English system equivalents for each of the following metric s...

Q: Why do we not necessarily expect the number of neutrons in the

Why do we not necessarily expect the number of neutrons in the nucleus of an atom to be the same as the number of protons?

Q: Which scientist discovered that the nuclei of most atoms contain neutrons as

Which scientist discovered that the nuclei of most atoms contain neutrons as well as protons?

Q: For each of the following elements, use the periodic table shown

For each of the following elements, use the periodic table shown in Fig. 4.9 to write the element’s atomic number, symbol, or name.

Q: Write the atomic symbol / for each of the isotopes described below

Write the atomic symbol / for each of the isotopes described below. a. the isotope of carbon with 7 neutrons b. the isotope of carbon with 6 neutrons c. Z = 6, number of neutrons = 8 d. atomic num...

Q: Write the atomic symbol for each of the isotopes described below.

Write the atomic symbol for each of the isotopes described below. a. Z = 26, A = 54 b. the isotope of iron with 30 neutrons c. number of protons = 26, number of neutrons = 31 d. the isotope of nit...

Q: How many protons and neutrons are contained in the nucleus of each

How many protons and neutrons are contained in the nucleus of each of the following atoms? Assuming each atom is uncharged, how many electrons are present?

Q: Read the “Chemistry in Focus” segment “Whair” Do

Read the “Chemistry in Focus” segment “Whair” Do You Live? How can isotopes be used to identify the general region of a person’s place of residence?

Q: Read the “Chemistry in Focus” segment Isotope Tales. Define

Read the “Chemistry in Focus” segment Isotope Tales. Define the term isotope, and explain how isotopes can be used to answer scientific and historical questions.

Q: Complete the following table. /

Complete the following table.

Q: True or false? The elements are arranged in the periodic table

True or false? The elements are arranged in the periodic table in order of increasing mass.

Q: The road sign I just passed says “New York City 100

The road sign I just passed says “New York City 100 km,” which is about mi.

Q: In which direction on the periodic table, horizontal or vertical,

In which direction on the periodic table, horizontal or vertical, are elements with similar chemical properties aligned? What are families of elements with similar chemical properties called?

Q: List the characteristic physical properties that distinguish the metallic elements from the

List the characteristic physical properties that distinguish the metallic elements from the nonmetallic elements.

Q: Where are the metallic elements found on the periodic table? Are

Where are the metallic elements found on the periodic table? Are there more metallic elements or nonmetallic elements?

Q: Most, but not all, metallic elements are solids under ordinary

Most, but not all, metallic elements are solids under ordinary laboratory conditions. Which metallic elements are not solids?

Q: List five nonmetallic elements that exist as gaseous substances under ordinary conditions

List five nonmetallic elements that exist as gaseous substances under ordinary conditions. Do any metallic elements ordinarily occur as gases?

Q: The elements that lie close to the “stair-step”

The elements that lie close to the “stair-step” line as shown below in blue are called .

Q: Write the number and name (if any) of the group

Write the number and name (if any) of the group (family) to which each of the following elements belongs. a. cesium b. Ra c. Rn d. chlorine e. strontium f. Xe g. Rb

Q: Without looking at your textbook or the periodic table, name three

Without looking at your textbook or the periodic table, name three elements in each of the following groups (families). a. halogens b. alkali metals c. alkaline earth metals d. noble/inert gases

Q: For each of the following elements, use the periodic table shown

For each of the following elements, use the periodic table shown in Fig. 4.9 to give the chemical symbol, atomic number, and group number and to specify whether each element is a metal, nonmetal, or m...

Q: The “Chemistry in Focus” segment Putting the Brakes on Arsenic

The “Chemistry in Focus” segment Putting the Brakes on Arsenic discusses the dangers of arsenic and a possible help against arsenic pollution. Is arsenic a metal, a nonmetal, or a metalloid? What othe...

Q: The GPS in my car indicates that I have 100. mi

The GPS in my car indicates that I have 100. mi left until I reach my destination. What is this distance in kilometers?

Q: Most substances are composed of rather than elemental substances.

Most substances are composed of rather than elemental substances.

Q: Are most of the chemical elements found in nature in the elemental

Are most of the chemical elements found in nature in the elemental form or combined in compounds? Why?

Q: The noble gas present in relatively large concentrations in the atmosphere is

The noble gas present in relatively large concentrations in the atmosphere is .

Q: Why are the elements of Group 8 referred to as the noble

Why are the elements of Group 8 referred to as the noble or inert gas elements?

Q: Molecules of nitrogen gas and oxygen gas are said to be ,

Molecules of nitrogen gas and oxygen gas are said to be , which means they consist of pairs of atoms.

Q: Give three examples of gaseous elements that exist as diatomic molecules.

Give three examples of gaseous elements that exist as diatomic molecules. Give three examples of gaseous elements that exist as monatomic species.

Q: A simple way to generate elemental hydrogen gas is to pass through

A simple way to generate elemental hydrogen gas is to pass through water.

Q: If sodium chloride (table salt) is melted and then subjected

If sodium chloride (table salt) is melted and then subjected to an electric current, elemental gas is produced, along wi...

Q: Most of the elements are solids at room temperature. Give three

Most of the elements are solids at room temperature. Give three examples of elements that are liquids at room temperature, and three examples of elements that are gases at room temperature.

Q: The two most common elemental forms of carbon are diamond and .

The two most common elemental forms of carbon are diamond and .

Q: The tablecloth on my dining room table is 2 m long,

The tablecloth on my dining room table is 2 m long, which is cm or about in.

Q: An isolated atom has a net charge of .

An isolated atom has a net charge of .

Q: Ions are produced when an atom gains or loses .

Ions are produced when an atom gains or loses .

Q: A simple ion with a 3+ charge (for example,

A simple ion with a 3+ charge (for example, Al+3) results when an atom (gains/loses) electrons.

Q: An ion that has two more electrons outside the nucleus than there

An ion that has two more electrons outside the nucleus than there are protons in the nucleus will have a charge of .

Q: Positive ions are called , whereas negative ions are called .

Positive ions are called , whereas negative ions are called .

Q: Simple negative ions formed from single atoms are given names that end

Simple negative ions formed from single atoms are given names that end in .

Q: Based on their location in the periodic table, give the symbols

Based on their location in the periodic table, give the symbols for three elements that would be expected to form positive ions in their reactions.

Q: True or false? N-3 and P-3 contain

True or false? N-3 and P-3 contain a different number of protons but the same number of electrons. Justify your answer.

Q: How many electrons are present in each of the following ions?

How many electrons are present in each of the following ions? a. Ba+2 b. P3- c. Mn2+ d. Mg2+ e. Cs+ f. Pb2-

Q: State the number of protons, electrons, and neutrons for /

State the number of protons, electrons, and neutrons for /

Q: Who is taller, a man who is 1.62 m

Who is taller, a man who is 1.62 m tall or a woman who is 5 ft 6 in. tall?

Q: For the following processes that show the formation of ions, use

For the following processes that show the formation of ions, use the periodic table to indicate the number of electrons and protons present in both the ion and the neutral atom from which the ion is m...

Q: For the following ions, indicate whether electrons must be gained or

For the following ions, indicate whether electrons must be gained or lost from the parent neutral atom, and how many electrons must be gained or lost. a. O2+ b. P3- c. Cr3+ d. Sn2+ e. Rb+ f. Pb2...

Q: For each of the following atomic numbers, use the periodic table

For each of the following atomic numbers, use the periodic table to write the formula (including the charge) for the simple ion that the element is most likely to form. a. 53 b. 38 c. 55 d. 88 e....

Q: On the basis of the element’s location in the periodic table,

On the basis of the element’s location in the periodic table, indicate what simple ion each of the following elements is most likely to form. a. P b. Ra c. At d. Rn e. Cs f. Se

Q: List some properties of a substance that would lead you to believe

List some properties of a substance that would lead you to believe it consists of ions. How do these properties differ from those of nonionic compounds?

Q: Why does a solution of sodium chloride in water conduct an electric

Why does a solution of sodium chloride in water conduct an electric current?

Q: Why does an ionic compound conduct an electric current when the compound

Why does an ionic compound conduct an electric current when the compound is melted but not when it is in the solid state?

Q: Why must the total number of positive charges in an ionic compound

Why must the total number of positive charges in an ionic compound equal the total number of negative charges?

Q: For each of the following positive ions, use the concept that

For each of the following positive ions, use the concept that a chemical compound must have a net charge of zero to predict the formula of the simple compounds that the positive ions would form with t...

Q: For each of the following negative ions, use the concept that

For each of the following negative ions, use the concept that a chemical compound must have a net charge of zero to predict the formula of the simple compounds that the negative ions would form with t...

Q: The fundamental SI unit of length is the meter. However,

The fundamental SI unit of length is the meter. However, we often deal with larger or smaller lengths or distances for which multiples or fractions of the fundamental unit are more useful. For each of...

Q: For each of the following elements, give the chemical symbol and

For each of the following elements, give the chemical symbol and atomic number. a. astatine b. xenon c. radium d. strontium e. lead f. selenium g. argon h. cesium

Q: Give the group number (if any) in the periodic table

Give the group number (if any) in the periodic table for the elements listed in Problem 85. If the group has a family name, give that name. From problem 85: For each of the following elements, give t...

Q: Which of the following statements is(are) true?

Which of the following statements is(are) true? a. Dalton was the first to theorize that atoms consist of smaller particles called electrons, protons, and neutrons. b. Dalton’s atomic theory didn’t...

Q: Which of the following is(are) true regarding 37Cl-

Which of the following is(are) true regarding 37Cl- and 40Ar? a. same group number on the periodic table b. same number of protons c. same number of neutrons d. same number of electrons

Q: Carbohydrates, a class of compounds containing the elements carbon, hydrogen

Carbohydrates, a class of compounds containing the elements carbon, hydrogen, and oxygen, were originally thought to contain one water molecule (H2O) for each carbon atom present. The carbohydrate glu...

Q: When iron rusts in moist air, the product is typically a

When iron rusts in moist air, the product is typically a mixture of two iron–oxygen compounds. In one compound, there is an equal number of iron and oxygen atoms. In the other compound, there are thre...

Q: How many protons and neutrons are contained in the nucleus of each

How many protons and neutrons are contained in the nucleus of each of the following atoms? For an atom of the element, how many electrons are present?

Q: Though the common isotope of aluminum has a mass number of 27

Though the common isotope of aluminum has a mass number of 27, isotopes of aluminum have been isolated (or prepared in nuclear reactors) with mass numbers of 24, 25, 26, 28, 29, and 30. How many neutr...

Q: How did Robert Boyle define an element?

How did Robert Boyle define an element?

Q: How many electrons are present in each of the following ions?

How many electrons are present in each of the following ions? a. Se2- b. Br- c. Cr3+ d. Rb+ e. Bi3+ f. Cu2+

Q: Which English unit of length or distance is most comparable in scale

Which English unit of length or distance is most comparable in scale to each of the following metric system units for making measurements? a. a centimeter b. a meter c. a kilometer

Q: Give the chemical symbol for each of the following elements.

Give the chemical symbol for each of the following elements. a. barium b. potassium c. cesium d. lead e. platinum f. gold

Q: Which of the following series of elements is not matched with the

Which of the following series of elements is not matched with the correct description? a. F, Cl, Br—halogens b. He, Ne, Ar—noble gases c. Mg, Ca, Sr—alkaline earth metals d. Fe, Co, Ni—transition...

Q: Give the chemical symbol for each of the following elements.

Give the chemical symbol for each of the following elements. a. silver b. aluminum c. cadmium d. antimony e. tin f. arsenic

Q: For each of the following chemical symbols, give the name of

For each of the following chemical symbols, give the name of the corresponding element. a. Te b. Pd c. Zn d. Si e. Cs f. Bi g. F h. Ti

Q: Write the simplest formula for each of the following substances, listing

Write the simplest formula for each of the following substances, listing the elements in the order given. a. a molecule containing one carbon atom and two oxygen atoms b. a compound containing one a...

Q: For each of the following atomic numbers, write the name and

For each of the following atomic numbers, write the name and chemical symbol of the corresponding element. (Refer to Figure 4.9.) a. 7 b. 10 c. 11 d. 28 e. 22 f. 18 g. 36 h. 54

Q: Write the atomic symbol /for each of the isotopes described below

Write the atomic symbol /for each of the isotopes described below. a. Z = 6, number of neutrons = 7 b. the isotope of carbon with a mass number of 13 c. Z = 6, A = 13 d. Z = 19, A = 44 e. the iso...

Q: How many protons and neutrons are contained in the nucleus of each

How many protons and neutrons are contained in the nucleus of each of the following atoms? In an atom of each element, how many electrons are present?

Q: Complete the following table. /

Complete the following table.

Q: For each of the following elements, use the table shown in

For each of the following elements, use the table shown in Fig. 4.9 to give the chemical symbol and atomic number and to specify whether the element is a metal or a nonmetal. Also give the named famil...

Q: The unit of volume in the metric system is the liter,

The unit of volume in the metric system is the liter, which consists of 1000 milliliters. How many liters or milliliters is each of the following common English system measurements approximately equiv...

Q: Read the “Chemistry in Focus” segment A Four-Wheel

Read the “Chemistry in Focus” segment A Four-Wheel-Drive Nanocar. It discusses carbon and copper atoms. Both atoms have stable isotopes. Example 4.2 had you consider the isotopes of carbon. Copper exi...

Q: Provide the name of the element that corresponds to each symbol given

Provide the name of the element that corresponds to each symbol given in the following table.

Q: Provide the symbols for the elements given in the following table.

Provide the symbols for the elements given in the following table.

Q: Complete the following table. /

Complete the following table.

Q: Complete the following table to predict whether the given atom will gain

Complete the following table to predict whether the given atom will gain or lose electrons in forming an ion.

Q: Using the periodic table, complete the following table. /

Using the periodic table, complete the following table.

Q: Complete the following table. / /

Complete the following table.

Q: Which of the following is(are) correct? a

Which of the following is(are) correct? a. 40Ca2+ contains 20 protons and 18 electrons. b. Rutherford created the cathode-ray tube and was the founder of the charge-to-mass ratio of an electron. c....

Q: Chemistry is an intimidating academic subject for many students. You are

Chemistry is an intimidating academic subject for many students. You are not alone if you are afraid of not doing well in this course! Why do you suppose the study of chemistry is so intimidating for...

Q: was the first scientist to recognize the importance of careful measurements

was the first scientist to recognize the importance of careful measurements.

Q: Which metric system unit is most appropriate for measuring the length of

Which metric system unit is most appropriate for measuring the length of an insect such as a beetle? a. meters b. millimeters c. megameters d. kilometers

Q: In addition to his important work on the properties of gases,

In addition to his important work on the properties of gases, what other valuable contributions did Robert Boyle make to the development of the study of chemistry?

Q: What are the three most abundant elements (by mass) in

What are the three most abundant elements (by mass) in the human body?

Q: What are the five most abundant elements (by mass) in

What are the five most abundant elements (by mass) in the earth’s crust, oceans, and atmosphere?

Q: Read the “Chemistry in Focus” segment Trace Elements: Small

Read the “Chemistry in Focus” segment Trace Elements: Small but Crucial, and answer the following questions. a. What is meant by the term trace element? b. Name two essential trace elements in the b...

Q: Give the symbols and names for the elements whose chemical symbols consist

Give the symbols and names for the elements whose chemical symbols consist of only one letter.

Q: Being a scientist is very much like being a detective. Detectives

Being a scientist is very much like being a detective. Detectives such as Sherlock Holmes or Miss Marple perform a very systematic analysis of a crime to solve it, much like a scientist does when addr...

Q: In science, what is the difference between a law and a

In science, what is the difference between a law and a theory? Provide examples of each.

Q: Observations may be either qualitative or quantitative. Quantitative observations are usually

Observations may be either qualitative or quantitative. Quantitative observations are usually referred to as measurements. List five examples of qualitative observations you might make around your hom...

Q: Use the periodic table shown in Fig. 4.9 to

Use the periodic table shown in Fig. 4.9 to find the symbol or name for each of the following elements

Q: Use the periodic table inside the front cover of this book to

Use the periodic table inside the front cover of this book to find the symbol or name for each of the following elements.

Q: When a measuring scale is used properly to the limit of precision

When a measuring scale is used properly to the limit of precision, the last significant digit recorded for the measurement is said to be uncertain. Explain.

Q: For each of the following chemical symbols, give the name of

For each of the following chemical symbols, give the name of the corresponding element. a. K b. Ge c. P d. C e. N f. Na g. Ne h. I

Q: What were the four fundamental substances postulated by the Greeks?

What were the four fundamental substances postulated by the Greeks?

Q: When a large or small number is written in standard scientific notation

When a large or small number is written in standard scientific notation, the number is expressed as the product of a number between 1 and 10, multiplied by the appropriate power of 10. For each of the...

Q: Classify the following as mixtures or pure substances. a.

Classify the following as mixtures or pure substances. a. a multivitamin tablet b. the blue liquid in your car’s windshield reservoir c. a ham and cheese omelet d. a diamond

Q: Classify the following mixtures as heterogeneous or homogeneous. a.

Classify the following mixtures as heterogeneous or homogeneous. a. soil b. mayonnaise c. Italian salad dressing d. the wood from which the desk you are studying on is made e. sand at the beach

Q: Why can the length of the pin shown in Fig. 2

Why can the length of the pin shown in Fig. 2.5 not be recorded as 2.850 cm?

Q: Indicate the number of significant figures in each of the following:

Indicate the number of significant figures in each of the following: a. 250. b. 250 c. 2.5 * 102 d. 250.0

Q: Indicate the number of significant figures implied in each of the following

Indicate the number of significant figures implied in each of the following statements: a. The population of the United States in 2016 was 324 million. b. One minute is equivalent to 60 seconds. c....

Q: When we round off a number, if the number to the

When we round off a number, if the number to the right of the digit to be rounded is greater than 5, then we should

Q: In a multiple-step calculation, is it better to round

In a multiple-step calculation, is it better to round off the numbers to the correct number of significant figures in each step of the calculation or to round off only the final answer? Explain.

Q: Round off each of the following numbers to three significant digits,

Round off each of the following numbers to three significant digits, and express the result in standard scientific notation. a. 254,931 b. 0.00025615 c. 47.85 * 103 d. 0.08214 * 105

Q: Round off each of the following numbers to two significant digits,

Round off each of the following numbers to two significant digits, and express the result in standard scientific notation. a. 1,566,311 b. 2.7651 * 10-3 c. 0.07759 d. 0.0011672

Q: Round off each of the following numbers to the indicated number of

Round off each of the following numbers to the indicated number of significant digits and write the answer in standard scientific notation. a. 4341 * 102 to three significant digits b. 93.441 * 103...

Q: When a large or small number is written in standard scientific notation

When a large or small number is written in standard scientific notation, the number is expressed as the product of a number between 1 and 10, multiplied by the appropriate power of 10. For each of the...

Q: Round off each of the following numbers to the indicated number of

Round off each of the following numbers to the indicated number of significant digits, and write the answer in standard scientific notation. a. 0.00034159 to two digits b. 103.351 * 102 to five digi...

Q: Consider the calculation indicated below: / Explain

Consider the calculation indicated below: Explain why the answer to this calculation should be reported to only two significant digits.

Q: The following water measurements are made: 18 mL of water measured

The following water measurements are made: 18 mL of water measured with a beaker, 128.7 mL of water measured with a graduated cylinder, and 23.45 mL of water measured with a buret. If all of these wat...

Q: When the calculation (2.31)(4.9795 *

When the calculation (2.31)(4.9795 * 103)/(1.9971 * 104) is performed, how many significant digits should be reported for the answer? You should not need to perform the calculation.

Q: Which of the following are true? a. P4 is

Which of the following are true? a. P4 is considered a compound. b. Metal rusting on a car is a chemical change. c. Dissolving sugar in water is a chemical change. d. Sodium chloride (NaCl) is a h...

Q: When the sum 4.9965 + 2.11 + 3

When the sum 4.9965 + 2.11 + 3.887 is calculated, to how many decimal places should the answer be reported? You should not need to perform the calculation.

Q: How many digits after the decimal point should be reported when the

How many digits after the decimal point should be reported when the calculation (10,434 -9.3344) is performed?

Q: The processes of melting and evaporation involve changes in the of a

The processes of melting and evaporation involve changes in the of a substance.

Q: A(n) always has the same composition.

A(n) always has the same composition.

Q: Without actually performing the calculations indicated, tell to how many significant

Without actually performing the calculations indicated, tell to how many significant digits the answer to the calculation should be expressed. a. (0.196)(0.08215)(295)/(1.1) b. (4.215 + 3.991 + 2.44...

Q: Will the power of 10 have a positive or a negative exponent

Will the power of 10 have a positive or a negative exponent when each of the following numbers is rewritten in standard scientific notation? a. 42,751 b. 1253 c. 0.002045 d. 0.1089

Q: Which of the following contains an element, a compound, and

Which of the following contains an element, a compound, and a mixture? a. copper, silicon dioxide (SiO2), copper(II) sulfate (CuSO4) b. hydrogen, carbon dioxide (CO2), water (H2O) c. chili, pizza,...

Q: How many significant digits should be used to report the answer to

How many significant digits should be used to report the answer to each of the following calculations? Do not perform the calculations. a. (2.7518 + 9.01 + 3.3349)/(2.1) b. (2.7751 * 1.95)/(.98) c....

Q: Which of the following best describes the air around you on a

Which of the following best describes the air around you on a typical day? (Assume the air is made up of ,80% nitrogen and ,20% oxygen. Ignore other gases such as water vapor and carbon dioxide.). a....

Q: A represents a ratio based on an equivalence statement between two measurements

A represents a ratio based on an equivalence statement between two measurements.

Q: How many significant figures are understood for the numbers in the following

How many significant figures are understood for the numbers in the following definition: 1 in. = 2.54 cm?

Q: Given that 1 mi = 1760 yd, determine what conversion factor

Given that 1 mi = 1760 yd, determine what conversion factor is appropriate to convert 1849 yd to miles; to convert 2.781 mi to yards.

Q: Given that 1 in. = 2.54 cm exactly,

Given that 1 in. = 2.54 cm exactly, indicate what conversion factor is appropriate to convert 3.25 in. to centimeters and to convert 46.12 cm to inches.

Q: For Exercises 57 and 58, apples cost $1.75

For Exercises 57 and 58, apples cost $1.75 per pound. What conversion factor is appropriate to express the cost of 5.3 lb of apples?

Q: For Exercises 57 and 58, apples cost $1.75

For Exercises 57 and 58, apples cost $1.75 per pound. What conversion factor could be used to determine how many pounds of apples could be bought for $25.00?

Q: Sketch the apparatus commonly used for simple distillation in the laboratory,

Sketch the apparatus commonly used for simple distillation in the laboratory, identifying each component.

Q: Will the power of 10 have a positive, negative, or

Will the power of 10 have a positive, negative, or zero exponent when each of the following numbers is rewritten in standard scientific notation? a. 0.08331 b. 2.8 c. 0.0491 d. 70,892,000

Q: The properties of a compound are often very different from the properties

The properties of a compound are often very different from the properties of the elements making up the compound. Water is an excellent example of this idea. Discuss.

Q: Which of the following best describes the substance XeF4? a

Which of the following best describes the substance XeF4? a. element b. compound c. heterogeneous mixture d. homogeneous mixture

Q: Which of the following statements is(are) true?

Which of the following statements is(are) true? a. A spoonful of sugar is a mixture. b. Only elements are pure substances. c. Air is a mixture of gases. d. Gasoline is a pure substance. e. Compou...

Q: 12.01 g of carbon contains 6.02 * 1023

12.01 g of carbon contains 6.02 * 1023 carbon atoms. What is the mass in grams of 1.89 * 1025 carbon atoms?

Q: Los Angeles and Honolulu are 2558 mi apart. What is this

Los Angeles and Honolulu are 2558 mi apart. What is this distance in kilometers?

Q: The United States has high-speed trains running between Boston and

The United States has high-speed trains running between Boston and New York capable of speeds up to 160 mi/h. Are these trains faster or slower than the fastest trains in the United Kingdom, which rea...

Q: The radius of an atom is on the order of 10210 m

The radius of an atom is on the order of 10210 m. What is this radius in centimeters? in inches? in nanometers?

Q: The temperature scale used in everyday life in most of the world

The temperature scale used in everyday life in most of the world except the United States is the scale.

Q: The point of water is at 32° on the Fahrenheit temperature

The point of water is at 32° on the Fahrenheit temperature scale.

Q: The normal boiling point of water is °F, or °

The normal boiling point of water is °F, or °C.

Q: What are the two characteristic properties of matter?

What are the two characteristic properties of matter?

Q: The freezing point of water is K.

The freezing point of water is K.

Q: On both the Celsius and Kelvin temperature scales, there are degrees

On both the Celsius and Kelvin temperature scales, there are degrees between the normal freezing and boiling points of water.

Q: On which temperature scale (°F, °C, or K

On which temperature scale (°F, °C, or K) does 1 degree represent the smallest change in temperature?

Q: Make the following temperature conversions: a. 44.2

Make the following temperature conversions: a. 44.2 °C to kelvins b. 891 K to °C c. 220 °C to kelvins d. 273.1 K to °C

Q: Carry out the indicated temperature conversions. a. 2153 °

Carry out the indicated temperature conversions. a. 2153 °F to kelvins b. 2153 °C to kelvins c. 555 °C to Fahrenheit degrees d. 224 °F to Celsius degrees

Q: Convert the following Fahrenheit temperatures to Celsius degrees. a.

Convert the following Fahrenheit temperatures to Celsius degrees. a. a chilly morning in early autumn, 45 °F b. a hot, dry day in the Arizona desert, 115 °F c. the temperature in winter when my car...

Q: Convert the following Celsius temperatures to Fahrenheit degrees. a.

Convert the following Celsius temperatures to Fahrenheit degrees. a. the boiling temperature of ethyl alcohol, 78.1 °C b. a hot day at the beach on a Greek isle, 40. °C c. the lowest possible tempe...

Q: The “Chemistry in Focus” segment Tiny Thermometers states that the

The “Chemistry in Focus” segment Tiny Thermometers states that the temperature range for the carbon nanotube gallium thermometers is 50 °C to 500 °C. a. What properties of gallium make it useful in a...

Q: Perform the indicated temperature conversions. a. 275 K to

Perform the indicated temperature conversions. a. 275 K to °C b. 82 °F to °C c. 221 °C to °F d. 240 °F to °C (Notice anything unusual about your answer?)

Q: What does the density of a substance represent?

What does the density of a substance represent?

Q: A sample of matter that is “rigid” has (stronger

A sample of matter that is “rigid” has (stronger/weaker) forces among the particles in the sample than does a sample that is not rigid.

Q: The most common units for density are .

The most common units for density are .

Q: A kilogram of lead occupies a much smaller volume than a kilogram

A kilogram of lead occupies a much smaller volume than a kilogram of water because has a much higher density.

Q: If a solid block of glass, with a volume of exactly

If a solid block of glass, with a volume of exactly 100 in.3, is placed in a basin of water that is full to the brim, then of water will overflow from the basin.

Q: Is the density of a gaseous substance likely to be larger or

Is the density of a gaseous substance likely to be larger or smaller than the density of a liquid or solid substance at the same temperature? Why?

Q: What property of density makes it useful as an aid in identifying

What property of density makes it useful as an aid in identifying substances?

Q: Referring to Table 2.8, which substance listed is most

Referring to Table 2.8, which substance listed is most dense? Which substance is least dense? For the two substances you have identified, for which one would a 1.00-g sample occupy the larger volume?...

Q: Referring to Table 2.8, determine whether magnesium, ethanol

Referring to Table 2.8, determine whether magnesium, ethanol, silver, or salt is the least dense. From table 2.8:

Q: In a sample of a gaseous substance, more than 99%

In a sample of a gaseous substance, more than 99% of the overall volume of the sample is empty space. How is this fact reflected in the properties of a gaseous substance compared with the properties o...

Q: For the masses and volumes indicated, calculate the density in grams

For the masses and volumes indicated, calculate the density in grams per cubic centimeter. a. mass = 4.53 kg; volume = 225 cm3 b. mass = 26.3 g; volume = 25.0 mL c. mass = 1.00 lb; volume = 500. cm...

Q: The element bromine at room temperature is a liquid with a density

The element bromine at room temperature is a liquid with a density of 3.12 g/mL. Calculate the mass of 125 mL of bromine. What volume does 85.0 g of bromine occupy?

Q: Indicate the number of significant digits in the answer when each of

Indicate the number of significant digits in the answer when each of the following expressions is evaluated (you do not have to evaluate the expression). a. (6.25)/(74.1143) b. (1.45)(0.08431)(6.022...

Q: Although some elements are found in an isolated state, most elements

Although some elements are found in an isolated state, most elements are found combined as with other elements.

Q: Write each of the following numbers in standard scientific notation, rounding

Write each of the following numbers in standard scientific notation, rounding off the numbers to three significant digits. a. 424.6174 b. 0.00078145 c. 26,755 d. 0.0006535 e. 72.5654

Q: By how many places must the decimal point be moved, and

By how many places must the decimal point be moved, and in which direction, to convert each of the following to “ordinary” decimal numbers? a. 4.311 * 106 b. 7.895 * 10-5 c. 8.712 * 101 d. 4.995 *...

Q: Sunflower oil has a density of 0.920 g/mL

Sunflower oil has a density of 0.920 g/mL. What is the mass of 4.50 L of sunflower oil? What volume (in L) would 375 g of sunflower oil occupy?

Q: If 1000. mL of linseed oil has a mass of 929

If 1000. mL of linseed oil has a mass of 929 g, calculate the density of linseed oil.

Q: A material will float on the surface of a liquid if the

A material will float on the surface of a liquid if the material has a density less than that of the liquid. Given that the density of water is approximately 1.0 g/mL under many conditions, will a blo...

Q: For Exercises 13–14 Magnesium metal is very malleable and is

For Exercises 13–14 Magnesium metal is very malleable and is able to be pounded and stretched into long, thin, narrow “ribbons” that are often used in the introductory chemistry lab as a source of the...

Q: Which of the following is/are examples of a chemical change

Which of the following is/are examples of a chemical change? a. carving wood b. snow melting c. dry ice subliming (solid CO2 vaporizing into a gas, passing the liquid state) d. burning cookies in...

Q: Use the information in Table 2.8 to calculate the volume

Use the information in Table 2.8 to calculate the volume of 50.0 g of each of the following substances. a. sodium chloride b. mercury c. benzene d. silver From table 2.8:

Q: Use the information in Table 2.8 to calculate the mass

Use the information in Table 2.8 to calculate the mass of 50.0 cm3 of each of the following substances. a. gold b. iron c. lead d. aluminum From table 2.8:

Q: How do we know when a chemical reaction is taking place?

How do we know when a chemical reaction is taking place? Can you think of an example of how each of the five senses (sight, hearing, taste, touch, smell) might be used in detecting when a chemical rea...

Q: Write the name of each of the following ionic substances, using

Write the name of each of the following ionic substances, using -ous or -ic endings to indicate the charge of the cation. a. CuCl b. Fe2O3 c. Hg2Cl2 d. MnCl2 e. TiO2 f. PbO

Q: Write the name of each of the following ionic substances, using

Write the name of each of the following ionic substances, using -ous or -ic endings to indicate the charge of the cation. a. CoCl2 b. CrBr3 c. PbO d. SnO2 e. Co2O3 f. FeCl3

Q: Write the name of each of the following binary compounds of nonmetallic

Write the name of each of the following binary compounds of nonmetallic elements. a. KrF2 b. Se2S6 c. AsH3 d. XeO4 e. BrF3 f. P2S5

Q: Write the name for each of the following binary compounds of nonmetallic

Write the name for each of the following binary compounds of nonmetallic elements. a. ClF5 b. XeCl2 c. SeO2 d. N2O3 e. I2Cl6 f. CS2

Q: Balance each of the following equations that describe precipitation reactions.

Balance each of the following equations that describe precipitation reactions. a. Na2SO4(aq) + CaCl2 (aq) CaSO4(s) + NaCl(aq) b. Co(C2H3O2) 2 (aq) + Na2S(aq)...

Q: The formulas Na2O and N2O look very similar. What is the

The formulas Na2O and N2O look very similar. What is the name for each compound? Why do we use a different naming convention between the two compounds?

Q: For each of the following precipitation reactions, complete and balance the

For each of the following precipitation reactions, complete and balance the equation, indicating clearly which product is the precipitate. If no reaction would be expected, so indicate. a. (NH4)2SO4(...

Q: On the basis of the general solubility rules given in Table 7

On the basis of the general solubility rules given in Table 7.1, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. If no precipitate is l...

Q: What is a net ionic equation? What species are shown in

What is a net ionic equation? What species are shown in such an equation, and which species are not shown?

Q: Lead(II) nitrate is added to four separate beakers that

Lead(II) nitrate is added to four separate beakers that contain the following: Beaker 1 (sodium chloride) Beaker 2 (sodium hydroxide) Beaker 3 (sodium phosphate) Beaker 4 (sodium sulfate) After t...

Q: Why is water an important solvent? Although you have not yet

Why is water an important solvent? Although you have not yet studied water in detail, can you think of some properties of water that make it so important?

Q: Based on the general solubility rules given in Table 7.1

Based on the general solubility rules given in Table 7.1, propose five combinations of aqueous ionic reagents that likely would form a precipitate when they are mixed. Write the balanced full molecula...

Q: On the basis of the general solubility rules given in Table 7

On the basis of the general solubility rules given in Table 7.1, write a balanced molecular equation for the precipitation reactions that take place when the following aqueous solutions are mixed. Und...

Q: On the basis of the general solubility rules given in Table 7

On the basis of the general solubility rules given in Table 7.1, write a balanced molecular equation for the precipitation reactions that take place when the following aqueous solutions are mixed. Und...

Q: Balance each of the following equations that describe precipitation reactions.

Balance each of the following equations that describe precipitation reactions. a. CaCl2(aq) + AgNO3(aq) Ca(NO3)2(aq) + AgCl(s) b. AgNO3(aq) + K2CrO4(aq) A...

Q: Balance each of the following chemical equations. a. FeCl3

Balance each of the following chemical equations. a. FeCl3(aq) + KOH(aq) Fe(OH)3(s) + KCl(aq) b. Pb(C2H3O2)2(aq) + KI(aq) PbI2(s) + KC2H3O2(aq) c. P4O10(s)...

Q: Balance each of the following chemical equations. a. K2SO4

Balance each of the following chemical equations. a. K2SO4(aq) + BaCl2(aq) BaSO4(s) + KCl(aq) b. Fe(s) + H2O(g) FeO(s) + H2(g) c. NaOH(aq) + HClO4(aq...

Q: Balance each of the following chemical equations. a. Na2SO4

Balance each of the following chemical equations. a. Na2SO4(aq) + CaCl2(aq) CaSO4(s) + NaCl(aq) b. Fe(s) + H2O(g) Fe3O4(s) + H2(g) c. Ca(OH)2(aq...

Q: Balance each of the following chemical equations. a. Fe3O4

Balance each of the following chemical equations. a. Fe3O4(s) + H2(g) Fe(l) + H2O(g) b. K2SO4(aq) + BaCl2(aq) BaSO4(s) + KCl(aq) c. HCl(aq...

Q: Balance each of the following chemical equations. a. NaCl

Balance each of the following chemical equations. a. NaCl(s) + SO2(g) + H2O(g) + O2 (g) Na2SO4(s) + HCl(g) b. Br2 (l) + I2 (s) IBr3(s) c. Ca3N2 (s) + H2O(l)...

Q: Balance each of the following chemical equations. a. KO2

Balance each of the following chemical equations. a. KO2(s) + H2O(l) KOH(aq) + O2 (g) + H2O2 (aq) b. Fe2O3(s) + HNO3(aq) Fe(NO3)3(aq) + H2O(l) c. NH3(g) + O2...

Q: Describe briefly what happens when an ionic substance is dissolved in water

Describe briefly what happens when an ionic substance is dissolved in water.

Q: Balance each of the following chemical equations. a. Ba

Balance each of the following chemical equations. a. Ba(NO3)2(aq) + Na2CrO4(aq) BaCrO4(s) + NaNO3(aq) b. PbCl2(aq) + K2SO4(aq) PbSO4(s) + KCl(aq) c. C2H5OH(l...

Q: What salt would form when each of the following strong acid/

What salt would form when each of the following strong acid/ strong base reactions takes place? a. HCl(aq) + KOH(aq) b. RbOH(aq) + HNO3(aq) c. HClO4(aq) + NaOH(aq) d. HBr(aq) + CsOH(aq)

Q: Complete the following acid–base reactions by indicating the acid and

Complete the following acid–base reactions by indicating the acid and base that must have reacted in each case to produce the indicated salt. a. +...

Q: What do we mean when we say that the transfer of electrons

What do we mean when we say that the transfer of electrons can be the “driving force” for a reaction? Give an example of a reaction where this happens.

Q: Balance each of the following oxidation–reduction reactions. a

Balance each of the following oxidation–reduction reactions. a. Co(s) + Br2(l) CoBr3(s) b. Al(s) + H2SO4(aq) Al2(SO4)3(aq) + H2(g) c. Na(s) + H2O(l...

Q: Balance each of the following oxidation–reduction chemical reactions.

Balance each of the following oxidation–reduction chemical reactions. a. P4(s) + O2(g) P4O10(s) b. MgO(s) + C(s) Mg(s) + CO(g) c. Sr(s) + H2O(l)...

Q: a. Give two examples each of a single-displacement reaction

a. Give two examples each of a single-displacement reaction and of a double-replacement reaction. How are the two reaction types similar, and how are they different? b. Give two examples each of a re...

Q: True or false? Coefficients can be fractions when balancing a chemical

True or false? Coefficients can be fractions when balancing a chemical equation. Whether true or false, explain why this can or cannot occur.

Q: Identify each of the following unbalanced reaction equations as belonging to one

Identify each of the following unbalanced reaction equations as belonging to one or more of the following categories: precipitation, acid–base, or oxidation–reduction. a. K2SO4(aq) + Ba(NO3)2(aq)...

Q: Identify each of the following unbalanced reaction equations as belonging to one

Identify each of the following unbalanced reaction equations as belonging to one or more of the following categories: precipitation, acid–base, or oxidation– reduction. a. H2O2(aq)...

Q: How do chemists know that the ions behave independently of one another

How do chemists know that the ions behave independently of one another when an ionic solid is dissolved in water?

Q: The reaction between ammonium perchlorate and aluminum is discussed in the “

The reaction between ammonium perchlorate and aluminum is discussed in the “Chemistry in Focus” segment Oxidation– Reduction Reactions Launch the Space Shuttle. The reaction is labeled as an oxidation...

Q: What is a synthesis or combination reaction? Give an example.

What is a synthesis or combination reaction? Give an example. Can such reactions also be classified in other ways? Give an example of a synthesis reaction that is also a combustion reaction. Give an e...

Q: What is a decomposition reaction? Give an example. Can such

What is a decomposition reaction? Give an example. Can such reactions also be classified in other ways?

Q: Complete and balance each of the following combustion reactions. a

Complete and balance each of the following combustion reactions. a. C6H6(l) + O2(g) b. C5H12(l) + O2(g) c. C2H6O(l) + O2(g)

Q: Complete and balance each of the following combustion reactions. a

Complete and balance each of the following combustion reactions. a. CH4(g) + O2(g) b. C2H2(g) + O2(g) c. C10H8(s) + O2(g)

Q: A metal ion with a 2+ charge has 23 electrons and

A metal ion with a 2+ charge has 23 electrons and forms a compound with a halogen ion that contains 17 protons. a. What is the identity of the metal ion? b. What is the identity of the halogen ion a...

Q: Complete Table 5.A by writing the names and formulas for

Complete Table 5.A by writing the names and formulas for the ionic compounds formed when the cations listed across the top combine with the anions shown in the left-hand column.

Q: Complete Table 5.B by writing the formulas for the ionic

Complete Table 5.B by writing the formulas for the ionic compounds formed when the anions listed across the top combine with the cations shown in the left-hand column.

Q: Balance each of the following chemical equations. a. Cl2

Balance each of the following chemical equations. a. Cl2(g) + KBr(aq) Br2 (l) + KCl(aq) b. Cr(s) + O2 (g) Cr2O3(s) c. P4(s) + H2 (g)...

Q: Balance each of the following chemical equations. a. SiCl4

Balance each of the following chemical equations. a. SiCl4(l) + Mg(s) Si(s) + MgCl2(s) b. NO(g) + Cl2(g) NOCl(g) c. MnO2(s) + Al(s)...

Q: Suppose you are trying to help your friend understand the general solubility

Suppose you are trying to help your friend understand the general solubility rules for ionic substances in water. Explain in general terms to your friend what the solubility rules mean, and give an ex...

Q: For each of the following atomic numbers, use the periodic table

For each of the following atomic numbers, use the periodic table to write the formula (including the charge) for the simple ion that the element is most likely to form. a. 36 b. 31 c. 52 d. 81 e....

Q: For the following pairs of ions, use the principle of electrical

For the following pairs of ions, use the principle of electrical neutrality to predict the formula of the binary compound that the ions are most likely to form. a. Na+ and S2- b. K+ and Cl- c. Ba2+...

Q: Which of the following statements about chemical equations is (are)

Which of the following statements about chemical equations is (are) true? a. When balancing a chemical equation, you can never change the coefficient in front of any chemical formula. b. The coeffic...

Q: Write the name of each of the following ionic substances, using

Write the name of each of the following ionic substances, using the system that includes a Roman numeral to specify the charge of the cation. a. FeBr2 b. CoS c. Co2S3 d. SnO2 e. Hg2Cl2 f. HgCl2...

Q: A member of the alkali metal family whose most stable ion contains

A member of the alkali metal family whose most stable ion contains 36 electrons forms a compound with chlorine. What is the correct formula for this compound?

Q: On the basis of the general solubility rules given in Table 7

On the basis of the general solubility rules given in Table 7.1, predict which of the following substances are not likely to be soluble in water. Indicate which specific rule(s) led to your conclusion...

Q: On the basis of the general solubility rules given in Table 7

On the basis of the general solubility rules given in Table 7.1, predict which of the following substances are likely to be appreciably soluble in water. Indicate which specific rule(s) led to your co...

Q: Write the name of each of the following ionic substances, using

Write the name of each of the following ionic substances, using the system that includes a Roman numeral to specify the charge of the cation. a. SnCl4 b. Fe2S3 c. PbO2 d. Cr2S3 e. CuO f. Cu2O

Q: Write the name of each of the following ionic substances, using

Write the name of each of the following ionic substances, using the system that includes a Roman numeral to specify the charge of the cation. a. FeI3 b. MnCl2 c. HgO d. Cu2S e. CoO f. SnBr4

Q: The “Chemistry in Focus” segment Sugar of Lead discusses Pb

The “Chemistry in Focus” segment Sugar of Lead discusses Pb(C2H3O2)2, which originally was known as sugar of lead. a. Why was it called sugar of lead? b. What is the systematic name for Pb(C2H3O2)2?...

Q: Give the name of each of the following simple binary ionic compounds

Give the name of each of the following simple binary ionic compounds. a. LiI b. MgF2 c. SrO d. AlBr3 e. CaS f. Na2O

Q: These days many products are available to whiten teeth at home.

These days many products are available to whiten teeth at home. Many of these products contain a peroxide that bleaches stains from the teeth. What evidence is there that the bleaching process is a ch...

Q: Phosphorus trichloride is used in the manufacture of certain pesticides and may

Phosphorus trichloride is used in the manufacture of certain pesticides and may be synthesized by direct combination of its constituent elements. Write the unbalanced chemical equation for this proces...

Q: Pure silicon, which is needed in the manufacturing of electronic components

Pure silicon, which is needed in the manufacturing of electronic components, may be prepared by heating silicon dioxide (sand) with carbon at high temperatures, releasing carbon monoxide gas. Write th...

Q: Nitrous oxide gas (systematic name: dinitrogen monoxide) is used

Nitrous oxide gas (systematic name: dinitrogen monoxide) is used by some dental practitioners as an anesthetic. Nitrous oxide (and water vapor as by-product) can be produced in small quantities in the...

Q: Solid zinc is added to an aqueous solution containing dissolved hydrogen chloride

Solid zinc is added to an aqueous solution containing dissolved hydrogen chloride to produce gaseous hydrogen that bubbles out of the solution and zinc chloride that remains dissolved in the water. Wr...

Q: Acetylene gas (C2H2) is often used by plumbers, welders

Acetylene gas (C2H2) is often used by plumbers, welders, and glass blowers because it burns in oxygen with an intensely hot flame. The products of the combustion of acetylene are carbon dioxide and wa...

Q: The burning of high-sulfur fuels has been shown to cause

The burning of high-sulfur fuels has been shown to cause the phenomenon of “acid rain.” When a high-sulfur fuel is burned, the sulfur is converted to sulfur dioxide (SO2) and sulfur trioxide (SO3). Wh...

Q: The Group 2 metals (Ba, Ca, Sr) can

The Group 2 metals (Ba, Ca, Sr) can be produced in the elemental state by the reaction of their oxides with aluminum metal at high temperatures, also producing solid aluminum oxide as a by-product. Wr...

Q: There are fears that the protective ozone layer around the earth is

There are fears that the protective ozone layer around the earth is being depleted. Ozone, O3, is produced by the interaction of ordinary oxygen gas in the atmosphere with ultraviolet light and lightn...

Q: Carbon tetrachloride was widely used for many years as a solvent until

Carbon tetrachloride was widely used for many years as a solvent until its harmful properties became well established. Carbon tetrachloride may be prepared by the reaction of natural gas (methane, CH4...

Q: In each of the following, identify which names are incorrect for

In each of the following, identify which names are incorrect for the given formulas, and give the correct name. a. CaH2, calcium hydride b. PbCl2, lead(IV) chloride c. CrI3, chromium(III) iodide d...

Q: Although these days many people have “self-cleaning” ovens

Although these days many people have “self-cleaning” ovens, if your oven gets really dirty you may have to resort to one of the spray-on oven cleaner preparations sold in supermarkets. What evidence i...

Q: When elemental phosphorus, P4, burns in oxygen gas, it

When elemental phosphorus, P4, burns in oxygen gas, it produces an intensely bright light, a great deal of heat, and massive clouds of white solid phosphorus(V) oxide (P2O5) product. Given these prope...

Q: Calcium oxide is sometimes very challenging to store in the chemistry laboratory

Calcium oxide is sometimes very challenging to store in the chemistry laboratory. This compound reacts with moisture in the air and is converted to calcium hydroxide. If a bottle of calcium oxide is l...

Q: Although they were formerly called the inert gases, the heavier elements

Although they were formerly called the inert gases, the heavier elements of Group 8 do form relatively stable compounds. For example, at high temperatures in the presence of an appropriate catalyst, x...

Q: The element tin often occurs in nature as the oxide, SnO2

The element tin often occurs in nature as the oxide, SnO2. To produce pure tin metal from this sort of tin ore, the ore usually is heated with coal (carbon). This produces pure molten tin, with the ca...

Q: Nitric acid, HNO3, can be produced by reacting high-

Nitric acid, HNO3, can be produced by reacting high-pressure ammonia gas with oxygen gas at around 750 °C in the presence of a platinum catalyst. Water is a by-product of the reaction. Write the unbal...

Q: When balancing chemical equations, beginning students are often tempted to change

When balancing chemical equations, beginning students are often tempted to change the numbers within a formula (the subscripts) to balance the equation. Why is this never permitted? What effect does c...

Q: The “Chemistry in Focus” segment The Beetle That Shoots Straight

The “Chemistry in Focus” segment The Beetle That Shoots Straight discusses the bombardier beetle and the chemical reaction of the decomposition of hydrogen peroxide. H2O2 (aq)...

Q: Balance the equation for the reaction of potassium with water.

Balance the equation for the reaction of potassium with water. K(s) + H2O(l) H2(g) + KOH(aq)

Q: Although this is no longer generally recommended, in the past,

Although this is no longer generally recommended, in the past, small cuts and abrasions on the skin were frequently cleaned using hydrogen peroxide solution. What evidence is there that treating a wou...

Q: In each of the following, identify which names are incorrect for

In each of the following, identify which names are incorrect for the given formulas, and give the correct name. a. CuCl2, copper(I) chloride b. Ag2O, silver oxide c. Li2O, lithium oxide d. CaS, ca...

Q: Acetylene gas, C2H2, is used in welding because it generates

Acetylene gas, C2H2, is used in welding because it generates an extremely hot flame when it is combusted with oxygen. The heat generated is sufficient to melt the metals being welded together. Carbon...

Q: When balancing a chemical equation, which of the following statements is

When balancing a chemical equation, which of the following statements is false? a. Subscripts in the reactants must be conserved in the products. b. Coefficients are used to balance the atoms on bot...

Q: Crude gunpowders often contain a mixture of potassium nitrate and charcoal (

Crude gunpowders often contain a mixture of potassium nitrate and charcoal (carbon). When such a mixture is heated until reaction occurs, a solid residue of potassium carbonate is produced. The explos...

Q: The following demonstration takes place in a two-step process:

The following demonstration takes place in a two-step process: First, solid calcium carbide (CaC2) reacts with liquid water to produce acetylene gas (C2H2) and aqueous calcium hydroxide. Second, the a...

Q: Methanol (methyl alcohol), CH3OH, is a very important industrial

Methanol (methyl alcohol), CH3OH, is a very important industrial chemical. Formerly, methanol was prepared by heating wood to high temperatures in the absence of air. The complex compounds present in...

Q: You have probably had the unpleasant experience of discovering that a flashlight

You have probably had the unpleasant experience of discovering that a flashlight battery has gotten old and begun to leak. Is there evidence that this change is due to a chemical reaction?

Q: The Hall process is an important method by which pure aluminum is

The Hall process is an important method by which pure aluminum is prepared from its oxide (alumina, Al2O3) by indirect reaction with graphite (carbon). Balance the following equation, which is a simpl...

Q: Iron oxide ores, commonly a mixture of FeO and Fe2O3,

Iron oxide ores, commonly a mixture of FeO and Fe2O3, are given the general formula Fe3O4. They yield elemental iron when heated to a very high temperature with either carbon monoxide or elemental hyd...

Q: When steel wool (iron) is heated in pure oxygen gas

When steel wool (iron) is heated in pure oxygen gas, the steel wool bursts into flame and a fine powder consisting of a mixture of iron oxides (FeO and Fe2O3) forms. Write separate unbalanced equation...

Q: One method of producing hydrogen peroxide is to add barium peroxide to

One method of producing hydrogen peroxide is to add barium peroxide to water. A precipitate of barium oxide forms, which may then be filtered off to leave a solution of hydrogen peroxide. Write the ba...

Q: A common experiment to determine the relative reactivity of metallic elements is

A common experiment to determine the relative reactivity of metallic elements is to place a pure sample of one metal into an aqueous solution of a compound of another metallic element. If the pure m...

Q: When elemental boron, B, is burned in oxygen gas,

When elemental boron, B, is burned in oxygen gas, the product is diboron trioxide. If the diboron trioxide is then reacted with a measured quantity of water, it reacts with the water to form what is c...

Q: A common experiment in introductory chemistry courses involves heating a weighed mixture

A common experiment in introductory chemistry courses involves heating a weighed mixture of potassium chlorate, KClO3, and potassium chloride. Potassium chlorate decomposes when heated, producing pota...

Q: A common demonstration in chemistry courses involves adding a tiny speck of

A common demonstration in chemistry courses involves adding a tiny speck of manganese(IV) oxide to a concentrated hydrogen peroxide, H2O2, solution. Hydrogen peroxide is unstable, and it decomposes qu...

Q: Write a balanced chemical equation for the complete combustion of pentene,

Write a balanced chemical equation for the complete combustion of pentene, C7H14. In combustion, pentene reacts with oxygen to produce carbon dioxide and water.

Q: Glass is a mixture of several compounds, but a major constituent

Glass is a mixture of several compounds, but a major constituent of most glass is calcium silicate, CaSiO3. Glass can be etched by treatment with hydrogen fluoride: HF attacks the calcium silicate of...

Q: If you’ve ever left bread in a toaster too long, you

If you’ve ever left bread in a toaster too long, you know that the bread eventually burns and turns black. What evidence is there that this represents a chemical process?

Q: Balance the following chemical equation. LiAlH4(s) +

Balance the following chemical equation. LiAlH4(s) + AlCl3(s) AlH3(s) + LiCl(s)

Q: If you had a “sour stomach,” you might try an

If you had a “sour stomach,” you might try an over-the-counter antacid tablet to relieve the problem. Can you think of evidence that the action of such an antacid is a chemical reaction?

Q: When iron wire is heated in the presence of sulfur, the

When iron wire is heated in the presence of sulfur, the iron soon begins to glow, and a chunky, blue-black mass of iron(II) sulfide is formed. Write the unbalanced chemical equation for this reaction....

Q: When finely divided solid sodium is dropped into a flask containing chlorine

When finely divided solid sodium is dropped into a flask containing chlorine gas, an explosion occurs and a fine powder of sodium chloride is deposited on the walls of the flask. Write the unbalanced...

Q: A common lecture demonstration called “elephant’s toothpaste” demonstrates the reaction

A common lecture demonstration called “elephant’s toothpaste” demonstrates the reaction of hydrogen peroxide producing water and oxygen gas. Write the unbalanced chemical equation for this process.

Q: When a strip of magnesium metal is heated in oxygen, it

When a strip of magnesium metal is heated in oxygen, it bursts into an intensely white flame and produces a finely powdered dust of magnesium oxide. Write the unbalanced chemical equation for this pro...

Q: Which of the following statements is false for the reaction of hydrogen

Which of the following statements is false for the reaction of hydrogen gas with oxygen gas to produce water? (a, b, and c represent coefficients) a H2(g) + b O2(g) c H2O(g) a. T...

Q: When solid red phosphorus, P4, is burned in air,

When solid red phosphorus, P4, is burned in air, the phosphorus combines with oxygen, producing a choking cloud of tetraphosphorus decoxide. Write the unbalanced chemical equation for this reaction.

Q: What are the substances to the left of the arrow in a

What are the substances to the left of the arrow in a chemical equation called? To the right of the arrow? What does the arrow itself mean?

Q: When copper(II) oxide is boiled in an aqueous solution

When copper(II) oxide is boiled in an aqueous solution of sulfuric acid, a strikingly blue solution of copper(II) sulfate forms along with additional water. Write the unbalanced chemical equation for...

Q: When lead(II) sulfide is heated to high temperatures in

When lead(II) sulfide is heated to high temperatures in a stream of pure oxygen gas, solid lead(II) oxide forms with the release of gaseous sulfur dioxide. Write the unbalanced chemical equation for t...

Q: Which of the following statements about chemical reactions is false?

Which of the following statements about chemical reactions is false? a. When balancing a chemical equation, all subscripts must be conserved. b. When one coefficient is doubled, the rest of the coef...

Q: Balance the following chemical equation: CuSO4(aq) +

Balance the following chemical equation: CuSO4(aq) + KI(s) CuI(s) + I2(s) + K2SO4(aq)

Q: Using different shapes to distinguish between different elements, draw a balanced

Using different shapes to distinguish between different elements, draw a balanced equation for the following reaction at the microscopic level. NH3(g) + O2(g) NO(g) + H2O(g)

Q: Balance the following chemical equations. MnO2(s) +

Balance the following chemical equations. MnO2(s) + CO(g) Mn2O3(aq) + CO2(g) Al(s) + H2SO4(aq) Al2(SO4)3(aq) + H2(g) C4H10(g) + O2(g)...

Q: If a sample of pure hydrogen gas is ignited very carefully,

If a sample of pure hydrogen gas is ignited very carefully, the hydrogen burns gently, combining with the oxygen gas of the air to form water vapor. Write the unbalanced chemical equation for this rea...

Q: For the unbalanced chemical equation HCl(g) + O2(

For the unbalanced chemical equation HCl(g) + O2(g) H2O(g) + Cl2(g) a. list the reactant(s). b. list the product(s).

Q: In a chemical reaction, the total number of atoms present after

In a chemical reaction, the total number of atoms present after the reaction is complete is (larger than/smaller than/the same as) the total number of atoms present before the reaction began.

Q: Using the general solubility rules given in Table 7.1,

Using the general solubility rules given in Table 7.1, which of the following ions will form a precipitate with SO42-? a. Ba2+ b. Na+ c. NH4+ d. At least two of the above ions will form a precipit...

Q: On the basis of the general solubility rules given in Table 7

On the basis of the general solubility rules given in Table 7.1, for each of the following compounds, explain why the compound would be expected to be appreciably soluble in water. Indicate which of t...

Q: On the basis of the general solubility rules given in Table 7

On the basis of the general solubility rules given in Table 7.1, for each of the following compounds, explain why the compound would not be expected to be appreciably soluble in water. Indicate which...

Q: What is a “driving force”? What are some of the

What is a “driving force”? What are some of the driving forces discussed in this section that tend to make reactions likely to occur? Can you think of any other possible driving forces?

Q: A solution of zinc nitrate is mixed with a solution of potassium

A solution of zinc nitrate is mixed with a solution of potassium hydroxide. A precipitate forms. Complete and balance the equation for this reaction, including the phases of each reactant and product....

Q: Which of the following most accurately describes a spectator ion?

Which of the following most accurately describes a spectator ion? a. An ion that is used up in a chemical reaction; it is limiting. b. An ion that participates in a chemical reaction but is always p...

Q: Write the balanced molecular, complete ionic, and net ionic equations

Write the balanced molecular, complete ionic, and net ionic equations for the reaction between nickel(II) chloride and sodium sulfide.

Q: Many chromate (CrO42-) salts are insoluble, and most have

Many chromate (CrO42-) salts are insoluble, and most have brilliant colors that have led to their being used as pigments. Write balanced net ionic equations for the reactions of Cu2+, Co3+, Ba2+, and...

Q: Liquid hydrazine, N2H4, has been used as a fuel for

Liquid hydrazine, N2H4, has been used as a fuel for rockets. When the rocket is to be launched, a catalyst causes the liquid hydrazine to decompose quickly into elemental nitrogen and hydrogen gases....

Q: The procedures and principles of qualitative analysis are covered in many introductory

The procedures and principles of qualitative analysis are covered in many introductory chemistry laboratory courses. In qualitative analysis, students learn to analyze mixtures of the common positive...

Q: Many plants are poisonous because their stems and leaves contain oxalic acid

Many plants are poisonous because their stems and leaves contain oxalic acid, H2C2O4, or sodium oxalate, Na2C2O4; when ingested, these substances cause swelling of the respiratory tract and suffocatio...

Q: A reaction in aqueous solution that results in the formation of a

A reaction in aqueous solution that results in the formation of a solid is called a reaction.

Q: Another step in the qualitative analysis of cations (see Exercise 28

Another step in the qualitative analysis of cations (see Exercise 28) involves precipitating some of the metal ions as the insoluble sulfides (followed by subsequent treatment of the mixed sulfide pre...

Q: What is meant by a strong acid? Are the strong acids

What is meant by a strong acid? Are the strong acids also strong electrolytes? Explain.

Q: What is meant by a strong base? Are the strong bases

What is meant by a strong base? Are the strong bases also strong electrolytes? Explain.

Q: The same net ionic process takes place when any strong acid reacts

The same net ionic process takes place when any strong acid reacts with any strong base. Write the equation for that process.

Q: Write the formulas and names of three common strong acids and strong

Write the formulas and names of three common strong acids and strong bases.

Q: If 1000 NaOH units were dissolved in a sample of water,

If 1000 NaOH units were dissolved in a sample of water, the NaOH would produce Na1 ions and OH2 ions.

Q: What is a salt? Give two balanced chemical equations showing how

What is a salt? Give two balanced chemical equations showing how a salt is formed when an acid reacts with a base.

Q: If electricity of sufficient voltage is passed into a solution of potassium

If electricity of sufficient voltage is passed into a solution of potassium iodide in water, a reaction takes place in which elemental hydrogen gas and elemental iodine are produced, leaving a solutio...

Q: Write balanced equations showing how three of the common strong acids ionize

Write balanced equations showing how three of the common strong acids ionize to produce hydrogen ion.

Q: Along with the three strong acids emphasized in the chapter (HCl

Along with the three strong acids emphasized in the chapter (HCl, HNO3, and H2SO4), hydrobromic acid, HBr, and perchloric acid, HClO4, are also strong acids. Write equations for the dissociation of ea...

Q: When writing the chemical equation for a reaction, how do you

When writing the chemical equation for a reaction, how do you indicate that a given reactant is dissolved in water? How do you indicate that a precipitate has formed as a result of the reaction?

Q: What is an oxidation–reduction reaction? What is transferred during

What is an oxidation–reduction reaction? What is transferred during such a reaction?

Q: Give an example of a simple chemical reaction that involves the transfer

Give an example of a simple chemical reaction that involves the transfer of electrons from a metallic element to a nonmetallic element.

Q: The thermite reaction produces so much energy (heat) that the

The thermite reaction produces so much energy (heat) that the iron is initially formed as a liquid. 2Al(s) + Fe2O3(s) 2Fe(s) + Al2O3(s) Describe the transfer of electrons for both...

Q: If atoms of the metal calcium were to react with molecules of

If atoms of the metal calcium were to react with molecules of the nonmetal fluorine, F2, how many electrons would each calcium atom lose? How many electrons would each fluorine atom gain? How many cal...

Q: If oxygen molecules, O2, were to react with magnesium atoms

If oxygen molecules, O2, were to react with magnesium atoms, how many electrons would each magnesium atom lose? How many electrons would each oxygen atom gain? How many magnesium atoms would be needed...

Q: For the reaction Mg(s) + Cl2(g)

For the reaction Mg(s) + Cl2(g) MgCl2(s), illustrate how electrons are gained and lost during the reaction.

Q: For the reaction 2Na(s) + O2(g)

For the reaction 2Na(s) + O2(g) Na2O2(s), show how electrons are gained and lost by the atoms.

Q: Silver oxide may be decomposed by strong heating into silver metal and

Silver oxide may be decomposed by strong heating into silver metal and oxygen gas. Write the unbalanced chemical equation for this process.

Q: How do we define a combustion reaction? In addition to the

How do we define a combustion reaction? In addition to the chemical products, what other products do combustion reactions produce? Give two examples of balanced chemical equations for combustion react...

Q: Reactions involving the combustion of fuel substances make up a subclass of

Reactions involving the combustion of fuel substances make up a subclass of reactions.

Q: When the ionic solute K3PO4 is dissolved in water, what can

When the ionic solute K3PO4 is dissolved in water, what can you say about the number of potassium ions (K+) present in the solution compared with the number of phosphate ions (PO43-) in the solution?...

Q: What is meant by a strong electrolyte? Give two examples of

What is meant by a strong electrolyte? Give two examples of substances that behave in solution as strong electrolytes.

Q: Name each of the following binary compounds, using the periodic table

Name each of the following binary compounds, using the periodic table to determine whether the compound is likely to be ionic (containing a metal and a nonmetal) or nonionic (containing only nonmetals...

Q: What is a binary chemical compound? What are the two major

What is a binary chemical compound? What are the two major types of binary chemical compounds? Give three examples of each type of binary compound.

Q: Many over-the-counter antacid tablets are now formulated using

Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for...

Q: Name each of the following binary compounds, using the periodic table

Name each of the following binary compounds, using the periodic table to determine whether the compound is likely to be ionic (containing a metal and a nonmetal) or nonionic (containing only nonmetals...

Q: Name each of the following binary compounds, using the periodic table

Name each of the following binary compounds, using the periodic table to determine whether the compound is likely to be ionic (containing a metal or a nonmetal) or nonionic (containing only nonmetals)...

Q: What is a polyatomic ion? Give examples of five common polyatomic

What is a polyatomic ion? Give examples of five common polyatomic ions.

Q: A(n) is a polyatomic ion containing at least one

A(n) is a polyatomic ion containing at least one oxygen atom and one or more atoms of at least one other element.

Q: For the oxyanions of sulfur, the ending -ite is used

For the oxyanions of sulfur, the ending -ite is used for SO32- to indicate that it contains than does SO42-.

Q: In naming oxyanions, when there are more than two members in

In naming oxyanions, when there are more than two members in the series for a given element, what prefixes are used to indicate the oxyanions in the series with the fewest and the most oxygen atoms?

Q: Complete the following list by filling in the missing names or formulas

Complete the following list by filling in the missing names or formulas of the oxyanions of chlorine.

Q: A series of oxyanions of iodine, comparable to the series for

A series of oxyanions of iodine, comparable to the series for chlorine discussed in the text, also exists. Write the formulas and names for the oxyanions of iodine.

Q: Write the formula for each of the following phosphorus- containing ions

Write the formula for each of the following phosphorus- containing ions, including the overall charge of the ion. a. phosphide b. phosphate c. phosphite d. hydrogen phosphate

Q: Cations are ions, and anions are ions.

Cations are ions, and anions are ions.

Q: Write the formula for each of the following carbon-containing ions

Write the formula for each of the following carbon-containing ions, including the overall charge of the ion. a. cyanide b. carbonate c. hydrogen carbonate d. acetate

Q: Write the formulas for the following compounds (refer to your answers

Write the formulas for the following compounds (refer to your answers to Problem 30). a. sodium cyanide b. calcium carbonate c. potassium hydrogen carbonate d. magnesium acetate

Q: Carbon occurs in several common polyatomic anions. List the formulas of

Carbon occurs in several common polyatomic anions. List the formulas of as many such anions as you can, along with the names of the anions.

Q: Give the name of each of the following polyatomic ions.

Give the name of each of the following polyatomic ions. a. HCO3- b. C2H3O2- c. CN- d. OH- e. NO2- f. HPO42-

Q: Give the name of each of the following polyatomic ions.

Give the name of each of the following polyatomic ions. a. NH4+ b. H2PO4- c. SO42- d. HSO3- e. ClO4- f. IO3-

Q: Name each of the following compounds, which contain polyatomic ions.

Name each of the following compounds, which contain polyatomic ions. a. NH4NO3 b. Ca(HCO3)2 c. MgSO4 d. Na2HPO4 e. KClO4 f. Ba(C2H3O2)2

Q: Name each of the following compounds, which contain polyatomic ions.

Name each of the following compounds, which contain polyatomic ions. a. NaMnO4 b. AlPO4 c. CrCO3 d. Ca(ClO)2 e. BaCO3 f. CaCrO4

Q: Give a simple definition of an acid.

Give a simple definition of an acid.

Q: Many acids contain the element in addition to hydrogen.

Many acids contain the element in addition to hydrogen.

Q: Name each of the following acids. a. HCl

Name each of the following acids. a. HCl b. H2SO4 c. HNO3 d. HI e. HNO2 f. HClO3 g. HBr h. HF i. HC2H3O2

Q: In naming ionic compounds, we always name the second.

In naming ionic compounds, we always name the second.

Q: Name each of the following acids. a. HOCl

Name each of the following acids. a. HOCl b. H2SO3 c. HBrO3 d. HOI e. HBrO4 f. H2S g. H2Se h. H3PO3

Q: Write the formula for each of the following simple binary ionic compounds

Write the formula for each of the following simple binary ionic compounds. a. cobalt(II) chloride b. cobaltic chloride c. sodium phosphide d. iron(II) oxide e. calcium hydride f. manganese(IV) o...

Q: Write the formula for each of the following simple binary ionic compounds

Write the formula for each of the following simple binary ionic compounds. a. magnesium fluoride b. ferric iodide c. mercuric sulfide d. barium nitride e. plumbous chloride f. stannic fluoride...

Q: Write the formula for each of the following binary compounds of nonmetallic

Write the formula for each of the following binary compounds of nonmetallic elements. a. carbon disulfide b. water c. dinitrogen trioxide d. dichlorine heptoxide e. carbon dioxide f. ammonia g....

Q: Write the formula for each of the following binary compounds of nonmetallic

Write the formula for each of the following binary compounds of nonmetallic elements. a. diphosphorus monoxide b. sulfur dioxide c. diphosphorus pentoxide d. carbon tetrachloride e. nitrogen trib...

Q: Write the formula for each of the following compounds that contain polyatomic

Write the formula for each of the following compounds that contain polyatomic ions. Be sure to enclose the polyatomic ion in parentheses if more than one such ion is needed to balance the oppositely c...

Q: Write the formula for each of the following compounds that contain polyatomic

Write the formula for each of the following compounds that contain polyatomic ions. Be sure to enclose the polyatomic ion in parentheses if more than one such ion is needed to balance the oppositely c...

Q: Write the formula for each of the following acids. a

Write the formula for each of the following acids. a. hydrosulfuric acid b. perbromic acid c. acetic acid d. hydrobromic acid e. chlorous acid f. hydroselenic acid g. sulfurous acid h. perchlo...

Q: Write the formula for each of the following acids. a

Write the formula for each of the following acids. a. hydrocyanic acid b. nitric acid c. sulfuric acid d. phosphoric acid e. hypochlorous acid f. hydrobromic acid g. bromous acid h. hydrofluo...

Q: Write the formula for each of the following substances. a

Write the formula for each of the following substances. a. sodium peroxide b. calcium chlorate c. rubidium hydroxide d. zinc nitrate e. ammonium dichromate f. hydrosulfuric acid g. calcium brom...

Q: In a simple binary ionic compound, which ion (cation/

In a simple binary ionic compound, which ion (cation/anion) has the same name as its parent element?

Q: Write the formula for each of the following substances. a

Write the formula for each of the following substances. a. calcium hydrogen sulfate b. zinc phosphate c. iron(III) perchlorate d. cobaltic hydroxide e. potassium chromate f. aluminum dihydrogen...

Q: Iron forms both 2+ and 3+ cations. Write formulas

Iron forms both 2+ and 3+ cations. Write formulas for the oxide, sulfide, and chloride compound of each iron cation, and give the name of each compound in both the nomenclature method that uses Roman...

Q: Before an electrocardiogram (ECG) is recorded for a cardiac patient

Before an electrocardiogram (ECG) is recorded for a cardiac patient, the ECG leads are usually coated with a moist paste containing sodium chloride. What property of an ionic substance such as NaCl is...

Q: Nitrogen and oxygen form numerous binary compounds, including NO, NO2

Nitrogen and oxygen form numerous binary compounds, including NO, NO2, N2O4, N2O5, and N2O. Give the name of each of these oxides of nitrogen.

Q: On some periodic tables, hydrogen is listed both as a member

On some periodic tables, hydrogen is listed both as a member of Group 1 and as a member of Group 7. Write an equation showing the formation of H+ ion and an equation showing the formation of H- ion.

Q: Examine the following table of formulas and names. Which of the

Examine the following table of formulas and names. Which of the compounds is/are named correctly? Formula……………………………………..Name a. Al2S3………………………………………dialuminum trisulfate b. CuNO3……………………………………….…cop...

Q: Complete the following list by filling in the missing oxyanion or oxyacid

Complete the following list by filling in the missing oxyanion or oxyacid for each pair.

Q: Name the following compounds. a. Ca(C2H3O2)

Name the following compounds. a. Ca(C2H3O2) 2 b. PCl3 c. Cu(MnO4) 2 d. Fe2 (CO3) 3 e. LiHCO3 f. Cr2S3 g. Ca(CN) 2

Q: Name the following compounds. a. AuBr3 b.

Name the following compounds. a. AuBr3 b. Co(CN)3 c. MgHPO4 d. B2H6 e. NH3 f. Ag2SO4 g. Be(OH)2

Q: Name the following compounds. a. HClO3 b.

Name the following compounds. a. HClO3 b. CoCl3 c. B2O3 d. H2O e. HC2H3O2 f. Fe(NO3)3 g. CuSO4

Q: Although we write the formula of sodium chloride as NaCl, we

Although we write the formula of sodium chloride as NaCl, we realize that NaCl is an ionic compound and contains no molecules. Explain.

Q: A compound has the general formula X2O, with X representing an

A compound has the general formula X2O, with X representing an unknown element or ion and O representing oxygen. Which of the following could not be a name for this compound? a. sodium oxide b. iron...

Q: Most metallic elements form oxides, and often the oxide is the

Most metallic elements form oxides, and often the oxide is the most common compound of the element that is found in the earth’s crust. Write the formulas for the oxides of the following metallic eleme...

Q: Consider a hypothetical simple ion M2+. Determine the formula of the

Consider a hypothetical simple ion M2+. Determine the formula of the compound this ion would form with each of the following anions. a. acetate b. permanganate c. oxide d. hydrogen phosphate e. h...

Q: Consider a hypothetical element M, which is capable of forming stable

Consider a hypothetical element M, which is capable of forming stable simple cations that have charges of 1+, 2+, and 3+, respectively. Write the formulas of the compounds formed by the various M cati...

Q: If aqueous solutions of potassium chromate and barium chloride are mixed,

If aqueous solutions of potassium chromate and barium chloride are mixed, a bright yellow solid (barium chromate) forms and settles out of the mixture, leaving potassium chloride in solution. Write a...

Q: When hydrogen sulfide, H2S, gas is bubbled through a solution

When hydrogen sulfide, H2S, gas is bubbled through a solution of lead(II) nitrate, Pb(NO3)2, a black precipitate of lead(II) sulfide, PbS, forms, and nitric acid, HNO3, is produced. Write the unbalanc...

Q: If an electric current is passed through aqueous solutions of sodium chloride

If an electric current is passed through aqueous solutions of sodium chloride, sodium bromide, and sodium iodide, the elemental halogens are produced at one electrode in each case, with hydrogen gas b...

Q: The noble metals gold, silver, and platinum are often used

The noble metals gold, silver, and platinum are often used in fashioning jewelry because they are relatively .

Q: The formula for ammonium phosphate is .

The formula for ammonium phosphate is .

Q: The elements of Group 7 (fluorine, chlorine, bromine,

The elements of Group 7 (fluorine, chlorine, bromine, and iodine) consist of molecules containing atom(s) .

Q: For a metallic element that forms two stable cations, the ending

For a metallic element that forms two stable cations, the ending is used to indicate the cation of lower charge and the ending...

Q: Under what physical state at room temperature do each of the halogen

Under what physical state at room temperature do each of the halogen elements exist?

Q: When an atom gains two electrons, the ion formed has a

When an atom gains two electrons, the ion formed has a charge of .

Q: An ion with one less electron than it has protons has a

An ion with one less electron than it has protons has a charge.

Q: An atom that has lost three electrons will have a charge of

An atom that has lost three electrons will have a charge of .

Q: An ion with two more electrons than it has protons has a

An ion with two more electrons than it has protons has a charge.

Q: For each of the negative ions listed in column 1, use

For each of the negative ions listed in column 1, use the periodic table to find in column 2 the total number of electrons the ion contains. A given answer may be used more than once. Column 1…………………...

Q: For each of the following processes that show the formation of ions

For each of the following processes that show the formation of ions, complete the process by indicating the number of electrons that must be gained or lost to form the ion. Indicate the total number o...

Q: What does “balancing” an equation accomplish?

What does “balancing” an equation accomplish?

Q: Balance the following chemical equations. Fe(s) +

Balance the following chemical equations. Fe(s) + O2(g) Fe2O3(s) PbO2(s) PbO(s) + O2(g) H2O2(l) O2(g) + H2O(l)

Q: Give the name of each of the following simple binary ionic compounds

Give the name of each of the following simple binary ionic compounds. a. BeO b. MgI2 c. Na2S d. Al2O3 e. HCl f. LiF g. Ag2S h. CaH2

Q: We indicate the charge of a metallic element that forms more than

We indicate the charge of a metallic element that forms more than one cation by adding a(n) after the name of the cation.

Q: In which of the following pairs is the name incorrect? Give

In which of the following pairs is the name incorrect? Give the correct name for the formulas indicated. a. Ag2O, disilver monoxide b. N2O, dinitrogen monoxide c. Fe2O3, iron(II) oxide d. PbO2, pl...

Q: Why are the physical states of the reactants and products often indicated

Why are the physical states of the reactants and products often indicated when writing a chemical equation?

Q: Write the name of each of the following ionic substances, using

Write the name of each of the following ionic substances, using -ous or -ic endings to indicate the charge of the cation. a. SnCl2 b. FeO c. SnO2 d. PbS e. Co2S3 f. CrCl2

Q: Name each of the following binary compounds. a. XeF6

Name each of the following binary compounds. a. XeF6 b. OF2 c. AsI3 d. N2O4 e. Cl2O f. SF6

Q: Name each of the following compounds. a. Fe(

Name each of the following compounds. a. Fe(C2H3O2)3 b. BrF c. K2O2 d. SiBr4 e. Cu(MnO4)2 f. CaCrO4

Q: Which oxyanion of nitrogen contains a larger number of oxygen atoms,

Which oxyanion of nitrogen contains a larger number of oxygen atoms, the nitrate ion or the nitrite ion?

Q: Examine the following table of formulas and names. Which of the

Examine the following table of formulas and names. Which of the compounds is/are named incorrectly? Formula……………………………………….Name a. Al2S3……………………dialuminum trisulfide b. KClO3……………………….potassium chlor...

Q: Write the formula for each of the following chromium-containing ions

Write the formula for each of the following chromium-containing ions, including the overall charge of the ion. a. chromous b. chromate c. chromic d. dichromate

Q: Give the name of each of the following polyatomic anions.

Give the name of each of the following polyatomic anions. a. CO32- b. ClO3- c. SO42- d. PO43- e. ClO4- f. MnO4-

Q: Name each of the following compounds, which contain polyatomic ions.

Name each of the following compounds, which contain polyatomic ions. a. LiH2PO4 b. Cu(CN)2 c. Pb(NO3)2 d. Na2HPO4 e. NaClO2 f. Co2(SO4)3

Q: Give the name of each of the following simple binary ionic compounds

Give the name of each of the following simple binary ionic compounds. a. NaBr b. MgCl2 c. AlP d. SrBr2 e. AgI f. K2S

Q: The notation “(l)” after a substance’s formula indicates it exists

The notation “(l)” after a substance’s formula indicates it exists in the state.

Q: Write the formula for each of the following binary compounds of nonmetallic

Write the formula for each of the following binary compounds of nonmetallic elements. a. sulfur dioxide b. dinitrogen monoxide c. xenon tetrafluoride d. tetraphosphorus decoxide e. phosphorus pen...

Q: Write the formula of each of the following ionic substances.

Write the formula of each of the following ionic substances. a. sodium dihydrogen phosphate b. lithium perchlorate c. copper(II) hydrogen carbonate d. potassium acetate e. barium peroxide f. ces...

Q: Write the formula for each of the following compounds, which contain

Write the formula for each of the following compounds, which contain polyatomic ions. Be sure to enclose the polyatomic ion in parentheses if more than one such ion is needed to balance the oppositely...

Q: Complete the following table to predict whether the given atom will gain

Complete the following table to predict whether the given atom will gain or lose electrons in forming the ion most likely to form when in ionic compounds.

Q: What are the formulas of the compounds that correspond to the names

What are the formulas of the compounds that correspond to the names given in the following table?

Q: What are the names of the compounds that correspond to the formulas

What are the names of the compounds that correspond to the formulas given in the following table?

Q: Provide the name of the acid that corresponds to the formula given

Provide the name of the acid that corresponds to the formula given in the following table.

Q: Which of the following statements is(are) correct?

Which of the following statements is(are) correct? a. The symbols for the elements magnesium, aluminum, and xenon are Mn, Al, and Xe, respectively. b. The elements P, As, and Bi are in the same fami...

Q: Elemental boron is produced in one industrial process by heating diboron trioxide

Elemental boron is produced in one industrial process by heating diboron trioxide with magnesium metal, also producing magnesium oxide as a by-product. Write the unbalanced chemical equation for this...

Q: Merchants usually sell small nuts, washers, and bolts by weight

Merchants usually sell small nuts, washers, and bolts by weight (like jelly beans!) rather than by individually counting the items. Suppose a particular type of washer weighs 0.110 g on the average. W...

Q: Write the balanced chemical equation for the complete combustion of heptene,

Write the balanced chemical equation for the complete combustion of heptene, C7H14. In combustion, heptene reacts with oxygen to produce carbon dioxide and water. What is the mole ratio that would ena...

Q: If you have equal mole samples of NO2 and F2, which

If you have equal mole samples of NO2 and F2, which of the following must be true? a. The number of molecules in each sample is the same. b. The number of atoms in each sample is the same. c. The m...

Q: A strikingly beautiful copper compound with the common name “blue vitriol

A strikingly beautiful copper compound with the common name “blue vitriol” has the following elemental composition: 25.45% Cu, 12.84% S, 4.036% H, 57.67% O. Determine the empirical formula of the comp...

Q: Calculate the number of grams of cobalt that contain the same number

Calculate the number of grams of cobalt that contain the same number of atoms as 2.24 g of iron.

Q: Using the average atomic masses given inside the front cover of this

Using the average atomic masses given inside the front cover of this book, calculate the mass in grams of each of the following samples. a. 0.341 mole of potassium nitride b. 2.62 mmol of neon (1 mm...

Q: For each of the following unbalanced equations, calculate how many moles

For each of the following unbalanced equations, calculate how many moles of the second reactant would be required to react completely with 0.413 moles of the first reactant. a. Co(s) + F2(g)...

Q: For each of the following unbalanced equations, calculate how many moles

For each of the following unbalanced equations, calculate how many moles of the second reactant would be required to react completely with 0.557 grams of the first reactant. a. Al(s) + Br2(l)...

Q: When elemental carbon is burned in the open atmosphere, with plenty

When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide. C(s) + O2(g) CO2(g) However, when the amount of oxygen present...

Q: Using the average atomic masses given inside the front cover of this

Using the average atomic masses given inside the front cover of this text, calculate how many moles of each element the following masses represent. a. 1.5 mg of chromium b. 2.0 * 10-3 g of strontium...

Q: Using the average atomic masses given inside the front cover of this

Using the average atomic masses given inside the front cover of this text, calculate the mass in grams of each of the following samples. a. 5.0 moles of potassium b. 0.000305 mole of mercury c. 2.3...

Q: Using the average atomic masses given inside the front cover of this

Using the average atomic masses given inside the front cover of this text, calculate the number of atoms present in each of the following samples. a. 2.89 g of gold b. 0.000259 mole of platinum c....

Q: For each of the following balanced chemical equations, calculate how many

For each of the following balanced chemical equations, calculate how many moles of product(s) would be produced if 0.500 mole of the first reactant were to react completely. a. CO2(g) + 4H2(g)...

Q: Calculate the molar mass for each of the following substances.

Calculate the molar mass for each of the following substances. a. ferrous sulfate b. mercuric iodide c. stannic oxide d. cobaltous chloride e. cupric nitrate

Q: Calculate the molar mass for each of the following substances.

Calculate the molar mass for each of the following substances. a. adipic acid, C6H10O4 b. caffeine, C8H10N4O2 c. eicosane, C20H42 d. cyclohexanol, C6H11OH e. vinyl acetate, C4H6O2 f. dextrose, C...

Q: Calculate the number of moles of the indicated substance present in each

Calculate the number of moles of the indicated substance present in each of the following samples. a. 21.2 g of ammonium sulfide b. 44.3 g of calcium nitrate c. 4.35 g of dichlorine monoxide d. 1....

Q: Calculate the number of moles of the indicated substance present in each

Calculate the number of moles of the indicated substance present in each of the following samples. a. 1.28 g of iron(II) sulfate b. 5.14 mg of mercury(II) iodide c. 9.21 µg of tin(IV) oxide d. 1.26...

Q: If you have equal-mole samples of each of the following

If you have equal-mole samples of each of the following compounds, which compound contains the greatest number of oxygen atoms? a. magnesium nitrate b. dinitrogen pentoxide c. iron(III) phosphate...

Q: Calculate the mass in grams of each of the following samples.

Calculate the mass in grams of each of the following samples. a. 3.09 moles of ammonium carbonate b. 4.01 * 10-6 moles of sodium hydrogen carbonate c. 88.02 moles of carbon dioxide d. 1.29 mmol of...

Q: Calculate the number of molecules present in each of the following samples

Calculate the number of molecules present in each of the following samples. a. 3.45 g of C6H12O6 b. 3.45 moles of C6H12O6 c. 25.0 g of ICl5 d. 1.00 g of B2H6 e. 1.05 mmol of Al(NO3)3

Q: Calculate the number of moles of hydrogen atoms present in each of

Calculate the number of moles of hydrogen atoms present in each of the following samples. a. 2.71 g of ammonia b. 0.824 mole of water c. 6.25 mg of sulfuric acid d. 451 g of ammonium carbonate

Q: Although we tend to make less use of mercury these days because

Although we tend to make less use of mercury these days because of the environmental problems created by its improper disposal, mercury is still an important metal because of its unusual property of e...

Q: Calculate the percent by mass of the element mentioned first in the

Calculate the percent by mass of the element mentioned first in the formulas for each of the following compounds. a. sodium azide, NaN3 b. copper(II) sulfate, CuSO4 c. gold(III) chloride, AuCl3 d....

Q: For each of the following unbalanced chemical equations, calculate how many

For each of the following unbalanced chemical equations, calculate how many moles of each product would be produced by the complete conversion of 0.125 mole of the reactant indicated in boldface. Stat...

Q: Ammonium nitrate has been used as a high explosive because it is

Ammonium nitrate has been used as a high explosive because it is unstable and decomposes into several gaseous substances. The rapid expansion of the gaseous substances produces the explosive force. N...

Q: A 1.2569-g sample of a new compound has

A 1.2569-g sample of a new compound has been analyzed and found to contain the following masses of elements: carbon, 0.7238 g; hydrogen, 0.07088 g; nitrogen, 0.1407 g; oxygen, 0.3214 g. Calculate the...

Q: In the “Chemistry in Focus” segment Cars of the Future

In the “Chemistry in Focus” segment Cars of the Future, the claim is made that the combustion of gasoline for some cars causes about 1 lb of CO2 to be produced for each mile traveled. Estimate the gas...

Q: When 2.004 g of calcium is heated in pure nitrogen

When 2.004 g of calcium is heated in pure nitrogen gas, the sample gains 0.4670 g of nitrogen. Calculate the empirical formula of the calcium nitride formed.

Q: Explain how one determines which reactant in a process is the limiting

Explain how one determines which reactant in a process is the limiting reactant. Does this depend only on the masses of the reactant present? Give an example of how to determine the limiting reactant...

Q: When 1.00 g of metallic chromium is heated with elemental

When 1.00 g of metallic chromium is heated with elemental chlorine gas, 3.045 g of a chromium chloride salt results. Calculate the empirical formula of the compound.

Q: When barium metal is heated in chlorine gas, a binary compound

When barium metal is heated in chlorine gas, a binary compound forms that consists of 65.95% Ba and 34.05% Cl by mass. Calculate the empirical formula of the compound.

Q: Determine the molar mass for the following compounds to four significant figures

Determine the molar mass for the following compounds to four significant figures.

Q: Vitamin B12, cyanocobalamin, is essential for human nutrition. Its

Vitamin B12, cyanocobalamin, is essential for human nutrition. Its molecular formula is C63H88CoN14O14P. A lack of this vitamin in the diet can lead to anemia. Cyanocobalamin is the form of the vitami...

Q: For each of the following unbalanced reactions, suppose exactly 5.

For each of the following unbalanced reactions, suppose exactly 5.00 moles of each reactant are taken. Determine which reactant is limiting, and also determine what mass of the excess reagent will rem...

Q: For each of the following balanced chemical equations, calculate how many

For each of the following balanced chemical equations, calculate how many grams of the product(s) would be produced by complete reaction of 0.125 mole of the first reactant. a. AgNO3(aq) + LiOH(aq)...

Q: For each of the following unbalanced chemical equations, suppose that exactly

For each of the following unbalanced chemical equations, suppose that exactly 5.00 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expecte...

Q: Consider samples of phosphine (PH3), water (H2O), hydrogen

Consider samples of phosphine (PH3), water (H2O), hydrogen sulfide (H2S), and hydrogen fluoride (HF), each with a mass of 119 g. Rank the compounds from the least to the greatest number of hydrogen at...

Q: For each of the following unbalanced chemical equations, suppose 10.

For each of the following unbalanced chemical equations, suppose 10.0 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that i...

Q: For each of the following unbalanced chemical equations, suppose that exactly

For each of the following unbalanced chemical equations, suppose that exactly 1.00 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of the product in boldface...

Q: A compound with molar mass 180.1 g/mol has

A compound with molar mass 180.1 g/mol has the following composition by mass: C ………...40.0% H ………... 6.70% O ………...53.3% Determine the empirical and molecular formulas of the compound.

Q: For each of the following unbalanced chemical equations, suppose 1.

For each of the following unbalanced chemical equations, suppose 1.00 g of each reactant is taken. Show by calculation which reactant is limiting. Calculate the mass of each product that is expected....

Q: For each of the following unbalanced chemical equations, suppose that exactly

For each of the following unbalanced chemical equations, suppose that exactly 15.0 g of each reactant are taken. Using Before–Change–After (BCA) tables, determine which reactant is limiting, and calcu...

Q: Lead(II) carbonate, also called “white lead,”

Lead(II) carbonate, also called “white lead,” was formerly used as a pigment in white paints. However, because of its toxicity, lead can no longer be used in paints intended for residential homes. Lea...

Q: Copper(II) sulfate has been used extensively as a fungicide

Copper(II) sulfate has been used extensively as a fungicide (kills fungus) and herbicide (kills plants). Copper(II) sulfate can be prepared in the laboratory by reaction of copper(II) oxide with sulfu...

Q: Hydrogen peroxide is used as a cleaning agent in the treatment of

Hydrogen peroxide is used as a cleaning agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many microorganisms; it decomposes upon contac...

Q: For each of the following balanced chemical equations, calculate how many

For each of the following balanced chemical equations, calculate how many moles and how many grams of each product would be produced by the complete conversion of 0.50 mole of the reactant indicated i...

Q: Silicon carbide, SiC, is one of the hardest materials known

Silicon carbide, SiC, is one of the hardest materials known. Surpassed in hardness only by diamond, it is sometimes known commercially as carborundum. Silicon carbide is used primarily as an abrasive...

Q: Your text talks about several sorts of “yield” when experiments

Your text talks about several sorts of “yield” when experiments are performed in the laboratory. Students often confuse these terms. Define, compare, and contrast what are meant by theoretical yield,...

Q: An air bag is deployed by utilizing the following reaction (the

An air bag is deployed by utilizing the following reaction (the nitrogen gas produced inflates the air bag): 2NaN3(s) 2Na(s) + 3N2(g) If 10.5 g of NaN3 is decomposed, what theoretica...

Q: The compound sodium thiosulfate pentahydrate, Na2S2O3.5H2O, is important

The compound sodium thiosulfate pentahydrate, Na2S2O3.5H2O, is important commercially to the photography business as “hypo,” because it has the ability to dissolve unreacted silver salts from photogra...

Q: Alkali metal hydroxides are sometimes used to “scrub” excess carbon

Alkali metal hydroxides are sometimes used to “scrub” excess carbon dioxide from the air in closed spaces (such as submarines and spacecraft). For example, lithium hydroxide reacts with carbon dioxide...

Q: Although they were formerly called the inert gases, at least the

Although they were formerly called the inert gases, at least the heavier elements of Group 8 do form relatively stable compounds. For example, xenon combines directly with elemental fluorine at elevat...

Q: Solid copper can be produced by passing gaseous ammonia over solid copper

Solid copper can be produced by passing gaseous ammonia over solid copper(II) oxide at high temperatures. The other products of the reaction are nitrogen gas and water vapor. The balanced equation for...

Q: Natural waters often contain relatively high levels of calcium ion, Ca21

Natural waters often contain relatively high levels of calcium ion, Ca21, and hydrogen carbonate ion (bicarbonate), HCO3-, from the leaching of minerals into the water. When such water is used commerc...

Q: One process for the commercial production of baking soda (sodium hydrogen

One process for the commercial production of baking soda (sodium hydrogen carbonate) involves the following reaction, in which the carbon dioxide is used in its solid form (“dry ice”) both to serve as...

Q: When the sugar glucose, C6H12O6, is burned in air,

When the sugar glucose, C6H12O6, is burned in air, carbon dioxide and water vapor are produced. Write the balanced chemical equation for this process, and calculate the theoretical yield of carbon dio...

Q: For each of the following unbalanced equations, indicate how many moles

For each of the following unbalanced equations, indicate how many moles of the second reactant would be required to react exactly with 0.275 mole of the first reactant. State clearly the mole ratio us...

Q: When elemental copper is strongly heated with sulfur, a mixture of

When elemental copper is strongly heated with sulfur, a mixture of CuS and Cu2S is produced, with CuS predominating. Cu(s) + S(s) / CuS(s) 2Cu(s) + S(s) / Cu2S(s) What is the theoretical yield...

Q: Barium chloride solutions are used in chemical analysis for the quantitative precipitation

Barium chloride solutions are used in chemical analysis for the quantitative precipitation of sulfate ion from solution. Ba2+(aq) + SO42–(aq) / BaSO4(s) Suppose a solution is known to contain on the...

Q: The traditional method of analysis for the amount of chloride ion present

The traditional method of analysis for the amount of chloride ion present in a sample is to dissolve the sample in water and then slowly to add a solution of silver nitrate. Silver chloride is very in...

Q: For each of the following reactions, give the balanced equation for

For each of the following reactions, give the balanced equation for the reaction and state the meaning of the equation in terms of numbers of individual molecules and in terms of moles of molecules....

Q: For each of the following balanced reactions, calculate how many moles

For each of the following balanced reactions, calculate how many moles of each product would be produced by complete conversion of 0.50 mole of the reactant indicated in boldface. Indicate clearly the...

Q: For each of the following balanced equations, indicate how many moles

For each of the following balanced equations, indicate how many moles of the product could be produced by complete reaction of 1.00 g of the reactant indicated in boldface. Indicate clearly the mole r...

Q: Using the average atomic masses given inside the front cover of the

Using the average atomic masses given inside the front cover of the text, calculate the mass in grams of each of the following samples. a. 5.0 moles of nitric acid b. 0.000305 mole of mercury c. 2....

Q: For each of the following incomplete and unbalanced equations, indicate how

For each of the following incomplete and unbalanced equations, indicate how many moles of the second reactant would be required to react completely with 0.145 mole of the first reactant. a. BaCl2(aq)...

Q: One step in the commercial production of sulfuric acid, H2SO4,

One step in the commercial production of sulfuric acid, H2SO4, involves the conversion of sulfur dioxide, SO2, into sulfur trioxide, SO3. 2SO2(g) + O2(g) / 2SO3(g) If 150 kg of SO2 reacts completely,...

Q: Many metals occur naturally as sulfide compounds; examples include ZnS and

Many metals occur naturally as sulfide compounds; examples include ZnS and CoS. Air pollution often accompanies the processing of these ores, because toxic sulfur dioxide is released as the ore is con...

Q: For each of the following unbalanced equations, indicate how many moles

For each of the following unbalanced equations, indicate how many moles of the first product are produced if 0.625 mole of the second product forms. State clearly the mole ratio used for each conversi...

Q: When elemental copper is placed in a solution of silver nitrate,

When elemental copper is placed in a solution of silver nitrate, the following oxidation–reduction reaction takes place, forming elemental silver: Cu(s) + 2AgNO3(aq) / Cu(NO3)2(aq) + 2Ag(s) What mass...

Q: When small quantities of elemental hydrogen gas are needed for laboratory work

When small quantities of elemental hydrogen gas are needed for laboratory work, the hydrogen is often generated by chemical reaction of a metal with acid. For example, zinc reacts with hydrochloric ac...

Q: The gaseous hydrocarbon acetylene, C2H2, is used in welders’ torches

The gaseous hydrocarbon acetylene, C2H2, is used in welders’ torches because of the large amount of heat released when acetylene burns with oxygen. 2C2H2(g) + 5O2(g) / 4CO2(g) + 2H2O(g) How many gram...

Q: For each of the following unbalanced chemical equations, suppose exactly 5

For each of the following unbalanced chemical equations, suppose exactly 5.0 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expected, ass...

Q: For each of the following unbalanced chemical equations, suppose 25.

For each of the following unbalanced chemical equations, suppose 25.0 g of each reactant is taken. Show by calculation which reactant is limiting. Calculate the theoretical yield in grams of the produ...

Q: Hydrazine, N2H4, emits a large quantity of energy when it

Hydrazine, N2H4, emits a large quantity of energy when it reacts with oxygen, which has led to hydrazine’s use as a fuel for rockets: N2H4(l) + O2(g) / N2(g) + 2H2O(g) How many moles of each of the g...

Q: Consider the following reaction: 4NH3(g) + 5O2

Consider the following reaction: 4NH3(g) + 5O2(g) ( 4NO(g) + 6H2O(g) a. If a container were to have only 10 molecules of O2(g) and 10 molecules of NH3(g), how many total molecules (reactant and produ...

Q: Over the years, the thermite reaction has been used for welding

Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid fuel rocket motors. The reaction is Fe2O3(s) + 2Al(s) / 2Fe(l) + Al2O3(s) a. W...

Q: Ammonia gas reacts with sodium metal to form sodium amide (NaNH2

Ammonia gas reacts with sodium metal to form sodium amide (NaNH2) and hydrogen gas. The unbalanced chemical equation for this reaction is as follows: NH3(g) + Na(s) NaNH2(s) +...

Q: Sulfur dioxide gas reacts with sodium hydroxide to form sodium sulfite and

Sulfur dioxide gas reacts with sodium hydroxide to form sodium sulfite and water. The unbalanced chemical equation for this reaction is as follows: SO2(g) + NaOH(s) Na2SO3(s) + H...

Q: What is meant by a state function? Give an example.

What is meant by a state function? Give an example.

Q: The production capacity for acrylonitrile (C3H3N) in the United States

The production capacity for acrylonitrile (C3H3N) in the United States is over 2 billion pounds per year. Acrylonitrile, the building block for polyacrylonitrile fibers and a variety of plastics, is p...

Q: How are the temperature of an object and the thermal energy of

How are the temperature of an object and the thermal energy of an object related?

Q: How is the calorie defined? How does a Calorie differ from

How is the calorie defined? How does a Calorie differ from a calorie? How is the joule related to the calorie?

Q: Convert the following numbers of calories or kilocalories into joules or kilojoules

Convert the following numbers of calories or kilocalories into joules or kilojoules. a. 7845 cal b. 4.55 * 104 cal c. 62.142 kcal d. 43,024 cal

Q: The “Chemistry in Focus” segment Nature Has Hot Plants discusses

The “Chemistry in Focus” segment Nature Has Hot Plants discusses thermogenic, or heat-producing, plants. For some plants, enough heat is generated to increase the temperature of the blossom by 15 °C....

Q: The enthalpy change for the reaction of hydrogen gas with fluorine gas

The enthalpy change for the reaction of hydrogen gas with fluorine gas to produce hydrogen fluoride is 2542 kJ for the equation as written: H2(g) + F2(g) 2HF(g) ∆H = -542 kJ a. Wh...

Q: For the reaction S(s) + O2(g)

For the reaction S(s) + O2(g) SO2(g), ∆H = -296 kJ per mole of SO2 formed. a. Calculate the quantity of heat released when 1.00 g of sulfur is burned in oxygen. b. Calculate the qu...

Q: When ethanol (grain alcohol, C2H5OH) is burned in oxygen

When ethanol (grain alcohol, C2H5OH) is burned in oxygen, approximately 1360 kJ of heat energy is released per mole of ethanol. C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(g) a. What...

Q: Given the following hypothetical data: X(g) +

Given the following hypothetical data: X(g) + Y(g) XY(g) for which ∆H = a kJ X(g) + Z(g) XZ(g) for which ∆H = b kJ Calculate ∆H for the reaction Y(g) + XZ(g)...

Q: Given the following data: C(s) + O2

Given the following data: C(s) + O2(g) CO2(g) ∆H = -393 kJ 2CO(g) + O2(g) 2CO2(g) ∆H = -566 kJ Calculate ∆H for the reaction 2C(s) + O2(g) CO...

Q: In Fig. 10.1, what kind of energy does

In Fig. 10.1, what kind of energy does ball A possess initially when at rest at the top of the hill? What kind of energies are involved as ball A moves down the hill? What kind of energy does ball A p...

Q: Given the following data: S(s) + 3

Given the following data: S(s) + 3/2 O2(g) SO3(g) ∆H = -395.2 kJ 2SO2(g) + O2(g) 2SO3(g) ∆H = -198.2 kJ Calculate ∆H for the reaction S(s) + O2(g)...

Q: Given the following data: C2H2(g) + 5

Given the following data: C2H2(g) + 5/2O2(g) 2CO2(g) + H2O(l) ∆H = -1300. kJ C(s) + O2(g) CO2(g) ∆H = -394 kJ H2(g) + 1/2O2(g) H2O...

Q: What does petroleum consist of? What are some “fractions”

What does petroleum consist of? What are some “fractions” into which petroleum is refined? How are these fractions related to the sizes of the molecules involved?

Q: What is the “greenhouse effect”? Why is a certain level

What is the “greenhouse effect”? Why is a certain level of greenhouse gases beneficial, but too high a level dangerous to life on earth? What is the most common greenhouse gas?

Q: A 50.0-g sample of water at 100.

A 50.0-g sample of water at 100. °C is poured into a 50.0-g sample of water at 25 °C. What will be the final temperature of the water?

Q: A 25.0-g sample of pure iron at 85

A 25.0-g sample of pure iron at 85 °C is dropped into 75 g of water at 20. °C. What is the final temperature of the water–iron mixture?

Q: For each of the substances listed in Table 10.1,

For each of the substances listed in Table 10.1, calculate the quantity of heat required to heat 150. g of the substance by 11.2 °C.

Q: The overall reaction in commercial heat packs can be represented as

The overall reaction in commercial heat packs can be represented as 4Fe(s) + 3O2(g) 2Fe2O3(s) ∆H = -1652 kJ a. How much heat is released when 4.00 moles of iron is reacted with ex...

Q: Consider the following equations: 3A + 6B 3D ∆H

Consider the following equations: 3A + 6B 3D ∆H = -403 kJ/mol E + 2F A ∆H = -105.2 kJ/mol C E + 3D ∆H = +64.8 kJ/mol Suppose the first equation is revers...

Q: It has been determined that the body can generate 5500 kJ of

It has been determined that the body can generate 5500 kJ of energy during one hour of strenuous exercise. Perspiration is the body’s mechanism for eliminating this heat. How many grams and how many l...

Q: Use the average atomic masses given inside the front cover of this

Use the average atomic masses given inside the front cover of this book to calculate the number of moles of the element present in each of the following samples. a. 4.95 g of neon b. 72.5 g of nicke...

Q: Which of the following reactions is/are endothermic? a

Which of the following reactions is/are endothermic? a. CO2(s) CO2(g) b. NH3(g) NH3(l) c. 2H2(g) + O2(g) 2H2O(g) d. H2O(l) H2O(s) e. Cl2(g...

Q: A swimming pool, 10.0 m by 4.0

A swimming pool, 10.0 m by 4.0 m, is filled with water to a depth of 3.0 m at a temperature of 20.2 °C. How much energy is required to raise the temperature of the water to 24.6 °C?

Q: Calculate ∆H for the reaction N2H4(l) +

Calculate ∆H for the reaction N2H4(l) + O2(g) N2(g) + 2H2O(l) given the following data:

Q: The “Chemistry in Focus” segment Atmospheric Effects discusses the greenhouse

The “Chemistry in Focus” segment Atmospheric Effects discusses the greenhouse effect. How do the greenhouse gases CO2, H2O, and CH4 have an effect on the temperature of the atmosphere?

Q: Describe briefly why the study of electromagnetic radiation has been important to

Describe briefly why the study of electromagnetic radiation has been important to our understanding of the arrangement of electrons in atoms.

Q: What does it mean to say that the hydrogen atom has discrete

What does it mean to say that the hydrogen atom has discrete energy levels? How is this fact reflected in the radiation that excited hydrogen atoms emit?

Q: How does the Bohr theory account for the observed phenomenon of the

How does the Bohr theory account for the observed phenomenon of the emission of discrete wavelengths of light by excited atoms?

Q: What major assumption (that was analogous to what had already been

What major assumption (that was analogous to what had already been demonstrated for electromagnetic radiation) did de Broglie and Schrödinger make about the motion of tiny particles?

Q: Section 11.6 uses a “firefly” analogy to illustrate

Section 11.6 uses a “firefly” analogy to illustrate how the wave mechanical model for the atom differs from Bohr’s model. Explain this analogy.

Q: Your text describes the probability map for an s orbital using an

Your text describes the probability map for an s orbital using an analogy to the earth’s atmosphere. Explain this analogy.

Q: The “Chemistry in Focus” segment Plastic That Talks and Listens

The “Chemistry in Focus” segment Plastic That Talks and Listens! discusses polyvinylidene difluoride (PVDF). What is the empirical formula of PVDF? Note: An empirical formula is the simplest whole-num...

Q: Use the average atomic masses given inside the front cover of this

Use the average atomic masses given inside the front cover of this book to calculate the number of moles of the element present in each of the following samples. a. 49.2 g of sulfur b. 7.44 * 104 kg...

Q: What overall shape do the 2p and 3p orbitals have? How

What overall shape do the 2p and 3p orbitals have? How do the 2p orbitals differ from the 3p orbitals? How are they similar?

Q: Although a hydrogen atom has only one electron, the hydrogen atom

Although a hydrogen atom has only one electron, the hydrogen atom possesses a complete set of available orbitals. What purpose do these additional orbitals serve?

Q: Where are the valence electrons found in an atom, and why

Where are the valence electrons found in an atom, and why are these particular electrons most important to the chemical properties of the atom?

Q: Write the complete orbital diagram for each of the following elements,

Write the complete orbital diagram for each of the following elements, using boxes to represent orbitals and arrows to represent electrons. a. helium, Z = 2 b. neon, Z = 10 c. krypton, Z = 36 d. x...

Q: What are some of the physical properties that distinguish the metallic elements

What are some of the physical properties that distinguish the metallic elements from the nonmetals? Are these properties absolute, or do some nonmetallic elements exhibit some metallic properties (and...

Q: Give some similarities that exist among the elements of Group 1.

Give some similarities that exist among the elements of Group 1.

Q: Where are the most nonmetallic elements located on the periodic table?

Where are the most nonmetallic elements located on the periodic table? Why do these elements pull electrons from metallic elements so effectively during a reaction?

Q: The “Chemistry in Focus” segment Fireworks discusses some of the

The “Chemistry in Focus” segment Fireworks discusses some of the chemicals that give rise to the colors of fireworks. How do these colors support the existence of quantized energy levels in atoms?

Q: In each of the following groups, which element is least reactive

In each of the following groups, which element is least reactive? a. Group 1 b. Group 7 c. Group 2 d. Group 6

Q: Arrange the following sets of elements in order of increasing atomic size

Arrange the following sets of elements in order of increasing atomic size. a. Sn, Xe, Rb, Sr b. Rn, He, Xe, Kr c. Pb, Ba, Cs, At

Q: Use the average atomic masses given inside the front cover of this

Use the average atomic masses given inside the front cover of this book to calculate the mass in grams of each of the following samples. a. 0.251 mole of lithium b. 1.51 moles of aluminum c. 8.75 *...

Q: An unknown element is a nonmetal and has a valence-electron

An unknown element is a nonmetal and has a valence-electron configuration of ns2np4. a. How many valence electrons does this element have? b. Possible identities for this element include which of th...

Q: One bit of evidence that the present theory of atomic structure is

One bit of evidence that the present theory of atomic structure is “correct” lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said...

Q: Without referring to your textbook or a periodic table, write the

Without referring to your textbook or a periodic table, write the full electron configuration, the orbital box diagram, and the noble gas shorthand configuration for the elements with the following at...

Q: Without referring to your textbook or a periodic table, write the

Without referring to your textbook or a periodic table, write the full electron configuration, the orbital box diagram, and the noble gas shorthand configuration for the elements with the following at...

Q: In the text (Section 11.6) it was mentioned

In the text (Section 11.6) it was mentioned that current theories of atomic structure suggest that all matter and all energy demonstrate both particle-like and wave-like properties under the appropria...

Q: Which of the following statements is(are) true regarding the

Which of the following statements is(are) true regarding the atom? a. Negatively charged particles are embedded in a positively charged cloud throughout the atom. b. As verified by Rutherford, only...

Q: Answer each of the following questions. Be thorough in your answers

Answer each of the following questions. Be thorough in your answers, and provide complete support. a. Write the ground-state electron configuration for oxygen. b. Draw the orbital diagram for the gr...

Q: Why do we believe that the three electrons in the 2p sublevel

Why do we believe that the three electrons in the 2p sublevel of nitrogen occupy different orbitals?

Q: When describing the electrons in an orbital, we use arrows pointing

When describing the electrons in an orbital, we use arrows pointing upward and downward / to indicate what property?

Q: Why can only two electrons occupy a particular orbital? What is

Why can only two electrons occupy a particular orbital? What is this idea called?

Q: Use the average atomic masses given inside the front cover of this

Use the average atomic masses given inside the front cover of this book to calculate the mass in grams of each of the following samples. a. 0.00552 mole of calcium b. 6.25 mmol of boron (1 mmol = 1⁄...

Q: How does the energy of a principal energy level depend on the

How does the energy of a principal energy level depend on the value of n? Does a higher value of n mean a higher or lower energy?

Q: The number of sublevels in a principal energy level (increases/

The number of sublevels in a principal energy level (increases/ decreases) as n increases.

Q: According to the Pauli exclusion principle, a given orbital can contain

According to the Pauli exclusion principle, a given orbital can contain only electrons.

Q: According to the Pauli exclusion principle, the electrons within a given

According to the Pauli exclusion principle, the electrons within a given orbital must have spins.

Q: Which of the following orbital designations is(are) possible?

Which of the following orbital designations is(are) possible? a. 1s b. 2p c. 2d d. 4f

Q: Which of the following orbital designations is(are) not possible

Which of the following orbital designations is(are) not possible? a. 3f b. 5s c. 4d d. 1p

Q: Which orbital is the first to be filled in any atom?

Which orbital is the first to be filled in any atom? Why?

Q: When a hydrogen atom is in its ground state, in which

When a hydrogen atom is in its ground state, in which orbital is its electron found? Why?

Q: How are the electron arrangements in a given group (vertical column

How are the electron arrangements in a given group (vertical column) of the periodic table related? How is this relationship manifested in the properties of the elements in the given group?

Q: Write the full electron configuration (1s22s2, etc.) for each

Write the full electron configuration (1s22s2, etc.) for each of the following elements. a. magnesium, Z = 12 b. lithium, Z = 3 c. oxygen, Z = 8 d. sulfur, Z = 16

Q: Using the average atomic masses given inside the front cover of this

Using the average atomic masses given inside the front cover of this book, calculate the number of atoms present in each of the following samples. a. 1.50 g of silver, Ag b. 0.0015 mole of copper, C...

Q: What does the wavelength of electromagnetic radiation represent? How is the

What does the wavelength of electromagnetic radiation represent? How is the wavelength of radiation related to the energy of the photons of the radiation?

Q: To which element does each of the following electron configurations correspond?

To which element does each of the following electron configurations correspond? a. 1s22s22p63s23p2 b. 1s22s2 c. 1s22s22p6 d. 1s22s22p63s23p6

Q: Write the full electron configuration (1s22s2, etc.) for each

Write the full electron configuration (1s22s2, etc.) for each of the following elements. a. phosphorus, Z = 15 b. calcium, Z = 20 c. potassium, Z = 19 d. boron, Z = 5

Q: To which element does each of the following electron configurations correspond?

To which element does each of the following electron configurations correspond? a. 1s22s22p63s23p64s23d104p4 b. 1s22s22p63s23p64s23d1 c. 1s22s22p63s23p4 d. 1s22s22p63s23p64s23d104p65s24d105p5

Q: Write the complete orbital diagram for each of the following elements,

Write the complete orbital diagram for each of the following elements, using boxes to represent orbitals and arrows to represent electrons. a. aluminum, Z = 13 b. phosphorus, Z = 15 c. bromine, Z =...

Q: The “Chemistry in Focus” segment A Magnetic Moment discusses the

The “Chemistry in Focus” segment A Magnetic Moment discusses the ability to levitate a frog in a magnetic field because electrons, when sensing a strong magnetic field, respond by opposing it. This is...

Q: For each of the following, give an atom and its complete

For each of the following, give an atom and its complete electron configuration that would be expected to have the indicated number of valence electrons. a. two b. four c. six d. eight

Q: Why do we believe that the valence electrons of calcium and potassium

Why do we believe that the valence electrons of calcium and potassium reside in the 4s orbital rather than in the 3d orbital?

Q: Would you expect the valence electrons of rubidium and strontium to reside

Would you expect the valence electrons of rubidium and strontium to reside in the 5s or the 4d orbitals? Why?

Q: Using the symbol of the previous noble gas to indicate the core

Using the symbol of the previous noble gas to indicate the core electrons, write the electron configuration for each of the following elements. a. arsenic, Z = 33 b. titanium, Z = 22 c. strontium,...

Q: Using the average atomic masses given inside the front cover of this

Using the average atomic masses given inside the front cover of this book, calculate the indicated quantities. a. the mass in grams of 125 iron atoms b. the mass in amu of 125 iron atoms c. the num...

Q: What do we mean by the frequency of electromagnetic radiation? Is

What do we mean by the frequency of electromagnetic radiation? Is the frequency the same as the speed of the electromagnetic radiation?

Q: To which element does each of the following abbreviated electron configurations refer

To which element does each of the following abbreviated electron configurations refer? a. [Ne]3s23p1 b. [Ar]4s1 c. [Ar]4s23d104p5 d. [Kr]5s24d105p2

Q: Using the symbol of the previous noble gas to indicate the core

Using the symbol of the previous noble gas to indicate the core electrons, write the electron configuration for each of the following elements. a. scandium, Z = 21 b. yttrium, Z = 39 c. lanthanum,...

Q: How many valence electrons does each of the following atoms have?

How many valence electrons does each of the following atoms have? a. rubidium, Z = 37 b. arsenic, Z = 33 c. aluminum, Z = 13 d. nickel, Z = 28

Q: How many 3d electrons are found in each of the following elements

How many 3d electrons are found in each of the following elements? a. nickel, Z = 28 b. vanadium, Z = 23 c. manganese, Z = 25 d. iron, Z = 26

Q: Based on the elements’ locations on the periodic table, how many

Based on the elements’ locations on the periodic table, how many 4d electrons would be predicted for each of the following elements? a. ruthenium, Z = 44 b. palladium, Z = 46 c. tin, Z = 50 d. iro...

Q: For each of the following elements, indicate which set of orbitals

For each of the following elements, indicate which set of orbitals is filled last. a. radium, Z = 88 b. iodine, Z = 53 c. gold, Z = 79 d. lead, Z = 82

Q: Write the valence-electron configuration of each of the following elements

Write the valence-electron configuration of each of the following elements, basing your answer on the element’s location on the periodic table. a. uranium, Z = 92 b. manganese, Z = 25 c. mercury, Z...

Q: Write the valence shell electron configuration of each of the following elements

Write the valence shell electron configuration of each of the following elements, basing your answer on the element’s location on the periodic table. a. rubidium, Z = 37 b. barium, Z = 56 c. titani...

Q: The “Chemistry in Focus” segment The Chemistry of Bohrium discusses

The “Chemistry in Focus” segment The Chemistry of Bohrium discusses element 107, bohrium (Bh). What is the expected electron configuration of Bh?

Q: For each of the following unbalanced equations, calculate how many grams

For each of the following unbalanced equations, calculate how many grams of each product would be produced by complete reaction of 12.5 g of the reactant indicated in boldface. Indicate clearly the mo...

Q: The “Chemistry in Focus” segment Light as a Sex Attractant

The “Chemistry in Focus” segment Light as a Sex Attractant discusses fluorescence. In fluorescence, ultraviolet radiation is absorbed and intense white visible light is emitted. Is ultraviolet radiati...

Q: What types of ions do the metals and the nonmetallic elements form

What types of ions do the metals and the nonmetallic elements form? Do the metals lose or gain electrons in doing this? Do the nonmetallic elements gain or lose electrons in doing this?

Q: Give some similarities that exist among the elements of Group 7.

Give some similarities that exist among the elements of Group 7.

Q: Which of the following elements most easily gives up electrons during reactions

Which of the following elements most easily gives up electrons during reactions: Li, K, or Cs? Explain your choice.

Q: Which elements in a given period (horizontal row) of the

Which elements in a given period (horizontal row) of the periodic table lose electrons most easily? Why?

Q: Why do the metallic elements of a given period (horizontal row

Why do the metallic elements of a given period (horizontal row) typically have much lower ionization energies than do the nonmetallic elements of the same period?

Q: What are the metalloids? Where are the metalloids found on the

What are the metalloids? Where are the metalloids found on the periodic table?

Q: In each of the following sets of elements, which element would

In each of the following sets of elements, which element would be expected to have the highest ionization energy? a. Cs, K, Li b. Ba, Sr, Ca c. I, Br, Cl d. Mg, Si, S

Q: In each of the following sets of elements, indicate which element

In each of the following sets of elements, indicate which element has the smallest atomic size. a. Na, K, Rb b. Na, Si, S c. N, P, As d. N, O, F

Q: Consider the bright line spectrum of hydrogen shown in Fig. 11

Consider the bright line spectrum of hydrogen shown in Fig. 11.10. Which line in the spectrum represents photons with the highest energy? With the lowest energy?

Q: Using the average atomic masses given inside the front cover of this

Using the average atomic masses given inside the front cover of this book, calculate how many moles of each substance the following masses represent. a. 4.15 g of silicon, Si b. 2.72 mg of gold(III)...

Q: The speed at which electromagnetic radiation moves through a vacuum is called

The speed at which electromagnetic radiation moves through a vacuum is called the .

Q: The portion of the electromagnetic spectrum between wavelengths of approximately 400 and

The portion of the electromagnetic spectrum between wavelengths of approximately 400 and 700 nanometers is called the region.

Q: A beam of light can be thought of as consisting of a

A beam of light can be thought of as consisting of a stream of light particles called .

Q: The lowest possible energy state of an atom is called the state

The lowest possible energy state of an atom is called the state.

Q: The energy levels of hydrogen (and other atoms) are ,

The energy levels of hydrogen (and other atoms) are , which means that only certain values of energy are allowed.

Q: According to Bohr, the electron in the hydrogen atom moved around

According to Bohr, the electron in the hydrogen atom moved around the nucleus in circular paths called .

Q: When lithium salts are heated in a flame, they emit red

When lithium salts are heated in a flame, they emit red light. When copper salts are heated in a flame in the same manner, they emit green light. Why do we know that lithium salts will never emit gree...

Q: Which of the following statements is false concerning orbitals? a

Which of the following statements is false concerning orbitals? a. An orbital is a region of space where an electron might be found with 90% probability. b. As an electron absorbs more energy, the o...

Q: Electrons found in the outermost principal energy level of an atom are

Electrons found in the outermost principal energy level of an atom are referred to as electrons.

Q: The of electromagnetic radiation represents the number of waves passing a given

The of electromagnetic radiation represents the number of waves passing a given point in space each second.

Q: Give the name and calculate the molar mass for each of the

Give the name and calculate the molar mass for each of the following substances. a. H3PO4 b. Fe2O3 c. NaClO4 d. PbCl2 e. HBr f. Al(OH)3

Q: The current model of the atom in which essentially all of an

The current model of the atom in which essentially all of an atom’s mass is contained in a very small nucleus, whereas most of an atom’s volume is due to the space in which the atom’s electrons move,...

Q: Write the general valence configuration (for example, ns1 for Group

Write the general valence configuration (for example, ns1 for Group 1) for the group in which each of the following elements is found. a. barium, Z = 56 b. bromine, Z = 35 c. tellurium, Z = 52 d....

Q: How many valence electrons does each of the following atoms have?

How many valence electrons does each of the following atoms have? a. titanium, Z = 22 b. iodine, Z = 53 c. radium, Z = 88 d. manganese, Z = 25

Q: What do we mean by the average atomic mass of an element

What do we mean by the average atomic mass of an element? What is “averaged” to arrive at this number?

Q: What do the coefficients of a balanced chemical equation tell us about

What do the coefficients of a balanced chemical equation tell us about the proportions in which atoms and molecules react on an individual (microscopic) basis?

Q: Using the average atomic masses for each of the following elements (

Using the average atomic masses for each of the following elements (see the table inside the front cover of this book), calculate the number of atoms present in each of the following samples. a. 40.0...

Q: What is the average atomic mass (in amu) of iron

What is the average atomic mass (in amu) of iron atoms? What would 299 iron atoms weigh? How many iron atoms are present in a sample of iron that has a mass of 5529.2 amu?

Q: The atomic mass of copper is 63.55 amu. What

The atomic mass of copper is 63.55 amu. What would be the mass of 75 copper atoms? How many copper atoms are contained in a sample of copper that has a mass of 6100.8 amu?

Q: There are iron atoms present in 55.85 g of iron

There are iron atoms present in 55.85 g of iron.

Q: There are 6.022 * 1023 zinc atoms present in g

There are 6.022 * 1023 zinc atoms present in g of zinc.

Q: Give the name and calculate the molar mass for each of the

Give the name and calculate the molar mass for each of the following substances. a. KHCO3 b. Hg2Cl2 c. H2O2 d. BeCl2 e. Al2(SO4)3 f. KClO3

Q: Suppose you have a sample of sodium weighing 11.50 g

Suppose you have a sample of sodium weighing 11.50 g. How many atoms of sodium are present in the sample? What mass of potassium would you need to have the same number of potassium atoms as there are...

Q: Consider a sample of silver weighing 300.0 g. How

Consider a sample of silver weighing 300.0 g. How many atoms of silver are present in the sample? What mass of copper would you need for the copper sample to contain the same number of atoms as the si...

Q: What mass of hydrogen contains the same number of atoms as 7

What mass of hydrogen contains the same number of atoms as 7.00 g of nitrogen?

Q: What mass of cobalt contains the same number of atoms as 57

What mass of cobalt contains the same number of atoms as 57.0 g of fluorine?

Q: If an average sodium atom has a mass of 3.82

If an average sodium atom has a mass of 3.82 * 10-23 g, what is the mass of a magnesium atom in grams?

Q: If an average fluorine atom has a mass of 3.16

If an average fluorine atom has a mass of 3.16 * 10-23 g, what is the average mass of a chlorine atom in grams?

Q: Which has the smaller mass, 1 mole of He atoms or

Which has the smaller mass, 1 mole of He atoms or 4 moles of H atoms?

Q: Which weighs less, 0.25 mole of xenon atoms or

Which weighs less, 0.25 mole of xenon atoms or 2.0 moles of carbon atoms?

Q: What quantity serves as the conversion factor between the mass of a

What quantity serves as the conversion factor between the mass of a sample and how many moles the sample contains?

Q: What does it mean to say that the balanced chemical equation for

What does it mean to say that the balanced chemical equation for a reaction describes the stoichiometry of the reaction?

Q: Write the formula and calculate the molar mass for each of the

Write the formula and calculate the molar mass for each of the following substances. a. barium chloride b. aluminum nitrate c. iron(II) chloride d. sulfur dioxide e. calcium acetate

Q: The vigorous reaction between aluminum and iodine gives the balanced equation:

The vigorous reaction between aluminum and iodine gives the balanced equation: 2Al(s) + 3I2(s) 2AlI3(s). What do the coefficients in this balanced chemical equation tell us about the prop...

Q: Although mass is a property of matter we can conveniently measure in

Although mass is a property of matter we can conveniently measure in the laboratory, the coefficients of a balanced chemical equation are not directly interpreted on the basis of mass. Explain why.

Q: Which of the following statements is true for the reaction of nitrogen

Which of the following statements is true for the reaction of nitrogen gas with hydrogen gas to produce ammonia (NH3)? Choose the best answer. a. Subscripts can be changed to balance this equation, j...

Q: Consider the reaction represented by the chemical equation C(s

Consider the reaction represented by the chemical equation C(s) + O2(g) CO2(g) Because the coefficients of the balanced chemical equation are all equal to 1, we know that exact...

Q: The of a substance is the mass (in grams) of

The of a substance is the mass (in grams) of 1 mole of the substance.

Q: Describe in your own words how the molar mass of the compound

Describe in your own words how the molar mass of the compound below may be calculated.

Q: “Smelling salts,” which are used to revive someone who has

“Smelling salts,” which are used to revive someone who has fainted, typically contain ammonium carbonate, (NH4)2CO3. Ammonium carbonate decomposes readily to form ammonia, carbon dioxide, and water. T...

Q: Calcium carbide, CaC2, can be produced in an electric furnace

Calcium carbide, CaC2, can be produced in an electric furnace by strongly heating calcium oxide (lime) with carbon. The unbalanced equation is CaO(s) + C(s) CaC2(s) + CO(g) Calcium...

Q: Boron nitride reacts with iodine monofluoride in trichlorofluoromethane at 230°C

Boron nitride reacts with iodine monofluoride in trichlorofluoromethane at 230°C to produce pure nitrogen triiodide and by-product (BF3). BN + 3IF NI3 + BF3 a. What mass of iodine mono...

Q: If baking soda (sodium hydrogen carbonate) is heated strongly,

If baking soda (sodium hydrogen carbonate) is heated strongly, the following reaction occurs: 2NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g) Calculate the mass of sodium carbonate that wi...

Q: Define the amu. What is one amu equivalent to in grams

Define the amu. What is one amu equivalent to in grams?

Q: Write the formula and calculate the molar mass for each of the

Write the formula and calculate the molar mass for each of the following substances. a. carbon dioxide b. aluminum phosphate c. iron(III) carbonate d. lead(II) nitrate e. strontium chloride

Q: Although we usually think of substances as “burning” only in

Although we usually think of substances as “burning” only in oxygen gas, the process of rapid oxidation to produce a flame may also take place in other strongly oxidizing gases. For example, when iron...

Q: When yeast is added to a solution of glucose or fructose,

When yeast is added to a solution of glucose or fructose, the sugars are said to undergo fermentation, and ethyl alcohol is produced. C6H12O6(aq) 2C2H5OH(aq) + 2CO2(g) This is...

Q: Sulfurous acid is unstable in aqueous solution and gradually decomposes to water

Sulfurous acid is unstable in aqueous solution and gradually decomposes to water and sulfur dioxide gas (which explains the choking odor associated with sulfurous acid solutions). H2SO3(aq)...

Q: Small quantities of ammonia gas can be generated in the laboratory by

Small quantities of ammonia gas can be generated in the laboratory by heating an ammonium salt with a strong base. For example, ammonium chloride reacts with sodium hydroxide according to the followin...

Q: Elemental phosphorus burns in oxygen with an intensely hot flame, producing

Elemental phosphorus burns in oxygen with an intensely hot flame, producing a brilliant light and clouds of the oxide product. These properties of the combustion of phosphorus have led to its being us...

Q: For the balanced chemical equation for the combination reaction of hydrogen gas

For the balanced chemical equation for the combination reaction of hydrogen gas and oxygen gas 2H2(g) + O2(g) 2H2O(g) explain why we know that 2 g of H2 reacting with 1 g of O2 wil...

Q: represents the ability to do work or to produce heat.

represents the ability to do work or to produce heat.

Q: If common sugars are heated too strongly, they char as they

If common sugars are heated too strongly, they char as they decompose into carbon and water vapor. For example, if sucrose (table sugar) is heated, the reaction is C12H22O11(s) 12C...

Q: Thionyl chloride, SOCl2, is used as a very powerful drying

Thionyl chloride, SOCl2, is used as a very powerful drying agent in many synthetic chemistry experiments in which the presence of even small amounts of water would be detrimental. The unbalanced chemi...

Q: A is a device used to determine the heat associated with a

A is a device used to determine the heat associated with a chemical reaction.

Q: Calculate the number of moles of the indicated substance present in each

Calculate the number of moles of the indicated substance present in each of the following samples. a. 21.4 mg of nitrogen dioxide b. 1.56 g of copper(II) nitrate c. 2.47 g of carbon disulfide d. 5...

Q: Which of the following statements is(are) true?

Which of the following statements is(are) true? a. A balanced equation relates the numbers of molecules of reactants and products (or numbers of moles of reactants and products). b. To convert betwee...

Q: In studying heat flows for chemical processes, what do we mean

In studying heat flows for chemical processes, what do we mean by the terms system and surroundings?

Q: The mass fraction of an element present in a compound can be

The mass fraction of an element present in a compound can be obtained by comparing the mass of the particular element present in 1 mole of the compound to the mass of the compound.

Q: If the amount of a sample doubles, what happens to the

If the amount of a sample doubles, what happens to the percent composition of each element in the compound?

Q: Consider the equation: 2A + B 5C. If 10.

Consider the equation: 2A + B 5C. If 10.0 g of A reacts with 5.00 g of B, how is the limiting reactant determined? Choose the best answer and explain. a. Choose the reactant w...

Q: Balance the following chemical equation, and then answer the question below

Balance the following chemical equation, and then answer the question below. CuSO4(aq) + KI(s) CuI(s) + I2(s) + K2SO4(aq) Which reactant is the limiting reactant? Choose the best...

Q: When a chemical system evolves energy, where does the energy go

When a chemical system evolves energy, where does the energy go?

Q: The combustion of methane, CH4, is an exothermic process.

The combustion of methane, CH4, is an exothermic process. Therefore, the products of this reaction must possess (higher/ lower) total potential energy than do the reactants.

Q: Consider the gasoline in your car’s gas tank. What happens to

Consider the gasoline in your car’s gas tank. What happens to the energy stored in the gasoline when you drive your car? Although the total energy in the universe remains constant, can the energy stor...

Q: Although the total energy of the universe will remain constant, why

Although the total energy of the universe will remain constant, why will energy no longer be useful once everything in the universe is at the same temperature?

Q: Calculate the number of moles of the indicated substance present in each

Calculate the number of moles of the indicated substance present in each of the following samples. a. 47.2 g of aluminum oxide b. 1.34 kg of potassium bromide c. 521 mg of germanium d. 56.2 µg of...

Q: Why are petroleum products especially useful as sources of energy?

Why are petroleum products especially useful as sources of energy?

Q: Why is the “quality” of energy decreasing in the universe

Why is the “quality” of energy decreasing in the universe?

Q: What experimental evidence about a new compound must be known before its

What experimental evidence about a new compound must be known before its formula can be determined?

Q: Explain to a friend who has not yet taken a chemistry course

Explain to a friend who has not yet taken a chemistry course what is meant by the empirical formula of a compound.

Q: Give the empirical formula that corresponds to each of the following molecular

Give the empirical formula that corresponds to each of the following molecular formulas. a. sodium peroxide, Na2O2 b. terephthalic acid, C8H6O4 c. phenobarbital, C12H12N2O3 d. 1,4-dichloro-2-buten...

Q: Which of the following pairs of compounds have the same empirical formula

Which of the following pairs of compounds have the same empirical formula? a. acetylene, C2H2, and benzene, C6H6 b. ethane, C2H6, and butane, C4H10 c. nitrogen dioxide, NO2, and dinitrogen tetroxid...

Q: What are the four “stages” of coal formation? How

What are the four “stages” of coal formation? How do the four types of coal differ?

Q: Are the following processes exothermic or endothermic? a. When

Are the following processes exothermic or endothermic? a. When solid KBr is dissolved in water, the solution gets colder. b. Natural gas (CH4) is burned in a furnace. c. When concentrated sulfuric...

Q: A is some factor that tends to make a process occur.

A is some factor that tends to make a process occur.

Q: The text explains that one reason why the actual yield for a

The text explains that one reason why the actual yield for a reaction may be less than the theoretical yield is side reactions. Suggest some other reasons why the percent yield for a reaction might no...

Q: Calculate the number of moles of the indicated substance in each of

Calculate the number of moles of the indicated substance in each of the following samples. a. 41.5 g of MgCl2 b. 135 mg of Li2O c. 1.21 kg of Cr d. 62.5 g of H2SO4 e. 42.7 g of C6H6 f. 135 g of...

Q: By now, you are familiar with enough chemical compounds to begin

By now, you are familiar with enough chemical compounds to begin to write your own chemical reaction equations. Write two examples of what we mean by a combustion reaction.

Q: According to his prelaboratory theoretical yield calculations, a student’s experiment should

According to his prelaboratory theoretical yield calculations, a student’s experiment should have produced 1.44 g of magnesium oxide. When he weighed his product after reaction, only 1.23 g of magnesi...

Q: Balance each of the following equations that describe synthesis reactions.

Balance each of the following equations that describe synthesis reactions. a. CaO(s) + H2O(l) Ca(OH)2(s) b. Fe(s) + O2(g) Fe2O3(s) c. P2O5(s) + H2O(l)...

Q: Balance each of the following equations that describe synthesis reactions.

Balance each of the following equations that describe synthesis reactions. a. Fe(s) + S8(s) FeS(s) b. Co(s) + O2(g) Co2O3(s) c. Cl2O7(g) + H2O(l) HClO4(aq)

Q: Balance each of the following equations that describe decomposition reactions.

Balance each of the following equations that describe decomposition reactions. a. CaSO4(s) CaO(s) + SO3(g) b. Li2CO3(s) Li2O(s) + CO2(g) c. LiHCO3(s) Li2CO3...

Q: Balance each of the following equations that describe oxidation– reduction reactions

Balance each of the following equations that describe oxidation– reduction reactions. a. Al(s) + Br2(l) AlBr3(s) b. Zn(s) + HClO4(aq) Zn(ClO4)2(aq) + H2(g) c. Na(s) +...

Q: When 3.269 g of zinc is heated in pure oxygen

When 3.269 g of zinc is heated in pure oxygen, the sample gains 0.800 g of oxygen in forming the oxide. Calculate the empirical formula of zinc oxide.

Q: Which of the following ions form compounds with Ag+ that are

Which of the following ions form compounds with Ag+ that are generally soluble in water? a. S2- b. Cl2 c. NO3- d. SO42- e. Na+

Q: Without first writing a full molecular or ionic equation, write the

Without first writing a full molecular or ionic equation, write the net ionic equations for any precipitation reactions that occur when aqueous solutions of the following compounds are mixed. If no re...

Q: Complete and balance each of the following molecular equations for strong acid

Complete and balance each of the following molecular equations for strong acid/strong base reactions. Underline the formula of the salt produced in each reaction. a. HNO3(aq) + KOH(aq)...

Q: Calculate the number of moles of the indicated substance present in each

Calculate the number of moles of the indicated substance present in each of the following samples. a. 1.95 * 10-3 g of lithium carbonate b. 4.23 kg of calcium chloride c. 1.23 mg of strontium chlor...

Q: A favorite demonstration among chemistry instructors, to show that the properties

A favorite demonstration among chemistry instructors, to show that the properties of a compound differ from those of its constituent elements, involves iron filings and powdered sulfur. If the instruc...

Q: Which of the following correctly identifies the precipitate formed when aqueous solutions

Which of the following correctly identifies the precipitate formed when aqueous solutions of the following substances are mixed? Mixed Solutions……………………………………Precipitate Formed a. Na2SO4 (aq) + BaCl...

Q: When 1.00 mg of lithium metal is reacted with fluorine

When 1.00 mg of lithium metal is reacted with fluorine gas (F2), the resulting fluoride salt has a mass of 3.73 mg. Calculate the empirical formula of lithium fluoride.

Q: Below are indicated the formulas of some salts. Such salts could

Below are indicated the formulas of some salts. Such salts could be formed by the reaction of the appropriate strong acid and strong base (with the other product of the reaction being, of course, wate...

Q: For each of the following unbalanced molecular equations, write the corresponding

For each of the following unbalanced molecular equations, write the corresponding balanced net ionic equation for the reaction. a. HCl(aq) + AgNO3(aq) AgCl(s) + HNO3(aq) b. CaCl...

Q: Write the balanced molecular, complete ionic, and net ionic equations

Write the balanced molecular, complete ionic, and net ionic equations for the reaction of ammonium sulfide with iron(III) chloride.

Q: What strong acid and what strong base would react in aqueous solution

What strong acid and what strong base would react in aqueous solution to produce the following salts? a. potassium perchlorate, KClO4 b. cesium nitrate, CsNO3 c. potassium chloride, KCl d. sodium...

Q: For the reaction 2Al(s) + 3I2(s)

For the reaction 2Al(s) + 3I2(s) 2AlI3(s), show how electrons are gained and lost by the atoms.

Q: For the reaction 16Fe(s) + 3S8(s)

For the reaction 16Fe(s) + 3S8(s) 8Fe2S3(s), show how electrons are gained and lost by the atoms.

Q: A compound with empirical formula C2H5O was found in a separate experiment

A compound with empirical formula C2H5O was found in a separate experiment to have a molar mass of approximately 90 g. What is the molecular formula of the compound?

Q: Calculate the mass in grams of each of the following samples.

Calculate the mass in grams of each of the following samples. a. 1.25 moles of aluminum chloride b. 3.35 moles of sodium hydrogen carbonate c. 4.25 millimoles of hydrogen bromide (1 millimole = 1⁄1...

Q: What are the molecular and empirical formulas for the following molecule?

What are the molecular and empirical formulas for the following molecule? Explain your reasoning.

Q: Which of the following statements is/are true regarding solutions?

Which of the following statements is/are true regarding solutions? a. If a solute is dissolved in water, then the resulting solution is considered aqueous. b. If two solutions are mixed and no chemi...

Q: Balance each of the following equations that describe synthesis reactions.

Balance each of the following equations that describe synthesis reactions. a. FeO(s) + O2(g) Fe2O3(s) b. CO(g) + O2(g) CO2(g) c. H2(g) + Cl2(g)...

Q: Balance each of the following equations that describe decomposition reactions.

Balance each of the following equations that describe decomposition reactions. a. NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g) b. NaClO3(s) NaCl(s)...

Q: A compound with empirical formula CH was found by experiment to have

A compound with empirical formula CH was found by experiment to have a molar mass of approximately 78 g. What is the molecular formula of the compound?

Q: A compound with the empirical formula CH2 was found to have a

A compound with the empirical formula CH2 was found to have a molar mass of approximately 84 g. What is the molecular formula of the compound?

Q: True or false? For the reaction represented by the balanced chemical

True or false? For the reaction represented by the balanced chemical equation Mg(OH)2(aq) + 2HCl(aq) 2H2O(l) + MgCl2(aq) for 0.40 mole of Mg(OH)2, 0.20 mol of HCl will be needed.

Q: For each of the following metals, how many electrons will the

For each of the following metals, how many electrons will the metal atoms lose when the metal reacts with a nonmetal? a. sodium b. potassium c. magnesium d. barium e. aluminum

Q: For each of the following nonmetals, how many electrons will each

For each of the following nonmetals, how many electrons will each atom of the nonmetal gain in reacting with a metal? a. oxygen b. fluorine c. nitrogen d. chlorine e. sulfur

Q: Hydrogen gas reacts with each of the halogen elements to form the

Hydrogen gas reacts with each of the halogen elements to form the hydrogen halides (HF, HCl, HBr, HI). Calculate the percent by mass of hydrogen in each of these compounds.

Q: Calculate the mass in grams of each of the following samples.

Calculate the mass in grams of each of the following samples. a. 6.14 * 10-4 moles of sulfur trioxide b. 3.11 * 105 moles of lead(IV) oxide c. 0.495 mole of chloroform, CHCl3 d. 2.45 * 10-8 moles...

Q: Consider the balanced equation C3H8(g) + 5O2(

Consider the balanced equation C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g) What mole ratio enables you to calculate the number of moles of oxygen needed to react exactly with a given number...

Q: When a sodium chromate solution and aluminum bromide solution are mixed,

When a sodium chromate solution and aluminum bromide solution are mixed, a precipitate forms. Complete and balance the equation for this reaction, including the phases of each reactant and product.

Q: Corrosion of metals costs us billions of dollars annually, slowly destroying

Corrosion of metals costs us billions of dollars annually, slowly destroying cars, bridges, and buildings. Corrosion of a metal involves the oxidation of the metal by the oxygen in the air, typically...

Q: Consider a solution with the following ions present: NO3-,

Consider a solution with the following ions present: NO3-, Pb2+, K+, Ag+, Cl-, SO42-, PO43- All are allowed to react, and there are plenty available of each. List all of the solids that will form usi...

Q: Find the item in column 2 that best explains or completes the

Find the item in column 2 that best explains or completes the statement or question in column 1. Column 1 (1) 1 amu (2) 1008 amu (3) mass of the “average” atom of an element (4) number of carbon a...

Q: For the following chemical reactions, determine the precipitate produced when the

For the following chemical reactions, determine the precipitate produced when the two reactants listed below are mixed together. Indicate “none” if no precipitate w...

Q: For the following chemical reactions, determine the precipitate produced when the

For the following chemical reactions, determine the precipitate produced when the two reactants listed below are mixed together. Indicate “none” if no precipitate w...

Q: Given that the molar mass of carbon tetrachloride, CCl4, is

Given that the molar mass of carbon tetrachloride, CCl4, is 153.8 g, calculate the mass in grams of 1 molecule of CCl4.

Q: You have a sample of copper (Cu) and a sample

You have a sample of copper (Cu) and a sample of aluminum (Al). You have an equal number of atoms in each sample. Which of the following statements concerning the masses of the samples is true? a. Th...

Q: A compound was analyzed and found to contain the following percentages of

A compound was analyzed and found to contain the following percentages of elements by mass: carbon, 79.89%; hydrogen, 20.11%. a. Determine the empirical formula of the compound. b. Which of the foll...

Q: Calculate the mass in grams of each of the following samples.

Calculate the mass in grams of each of the following samples. a. 0.251 mole of ethyl alcohol, C2H6O b. 1.26 moles of carbon dioxide c. 9.31 * 10-4 moles of gold(III) chloride d. 7.74 moles of sodi...

Q: Calculate the number of grams of lithium that contain the same number

Calculate the number of grams of lithium that contain the same number of atoms as 1.00 kg of zirconium.

Q: A certain transition metal ion (Mn+) forms a compound with

A certain transition metal ion (Mn+) forms a compound with oxygen (MxOy). The molar mass of the compound is 250.2 g/ mol. If the charge on the transition metal ion is 13, what is the identity of the t...

Q: The mass 1.66 * 10-24 g is equivalent

The mass 1.66 * 10-24 g is equivalent to 1 .

Q: Although exact isotopic masses are known with great precision for most elements

Although exact isotopic masses are known with great precision for most elements, we use the average mass of an element’s atoms in most chemical calculations. Explain.

Q: Using the average atomic masses given in Table 8.1,

Using the average atomic masses given in Table 8.1, calculate the number of atoms present in each of the following samples. a. 160,000 amu of oxygen b. 8139.81 amu of nitrogen c. 13,490 amu of alum...

Q: If an average sodium atom weighs 22.99 amu, how

If an average sodium atom weighs 22.99 amu, how many sodium atoms are contained in 1.98 * 1013 amu of sodium? What will 3.01 * 1023 sodium atoms weigh?

Q: If sodium peroxide is added to water, elemental oxygen gas is

If sodium peroxide is added to water, elemental oxygen gas is generated: Na2O2(s) + H2O(l) NaOH(aq) + O2(g) Suppose 3.25 g of sodium peroxide is added to a large excess of water. Wha...

Q: Before going to lab, a student read in his lab manual

Before going to lab, a student read in his lab manual that the percent yield for a difficult reaction to be studied was likely to be only 40. % of the theoretical yield. The student’s prelab stoichiom...

Q: Consider the following unbalanced chemical equation for the combustion of pentane (

Consider the following unbalanced chemical equation for the combustion of pentane (C5H12): C5H12(l) + O2(g) CO2(g) + H2O(l) If a 20.4-gram sample of pentane is burned in...

Q: A 0.4230-g sample of impure sodium nitrate (

A 0.4230-g sample of impure sodium nitrate (contains sodium nitrate plus inert ingredients) was heated, converting all the sodium nitrate to 0.2339 g of sodium nitrite and oxygen gas. Determine the pe...

Q: Calculate the mass in grams of each of the following samples.

Calculate the mass in grams of each of the following samples. a. 0.994 mole of benzene, C6H6 b. 4.21 moles of calcium hydride c. 1.79 * 10-4 moles of hydrogen peroxide, H2O2 d. 1.22 mmol of glucos...

Q: Consider the following unbalanced chemical equation. LiOH(s)

Consider the following unbalanced chemical equation. LiOH(s) + CO2(g) / Li2CO3(s) + H2O(l) If 67.4 g of lithium hydroxide reacts with excess carbon dioxide, what mass of lithium carbonate will be pro...

Q: Consider the following unbalanced chemical equation: H2S(g)

Consider the following unbalanced chemical equation: H2S(g) + O2(g) SO2(g) + H2O(g) Determine the maximum number of moles of SO2 produced from 8.0 moles of H2S and 3.0 moles...

Q: What do we mean by thermodynamics? What is the first law

What do we mean by thermodynamics? What is the first law of thermodynamics?

Q: The energy, E, of a system represents the sum of

The energy, E, of a system represents the sum of the kinetic and potential energies of all particles within the system.

Q: Calculate ∆E for each of the following cases. a

Calculate ∆E for each of the following cases. a. q = +65 kJ, w = -22 kJ b. q = +200. kJ, w = -73 kJ c. q = -18 kJ, w = -40. kJ

Q: If q for a process is a positive number, then the

If q for a process is a positive number, then the system is (gaining/losing) energy.

Q: For an endothermic process, q will have a (positive/

For an endothermic process, q will have a (positive/negative) sign.

Q: How many anions are there in 5.00 g of calcium

How many anions are there in 5.00 g of calcium bromide?

Q: What is meant by potential energy? Give an example of an

What is meant by potential energy? Give an example of an object or material that possesses potential energy.

Q: The percent by mass of nitrogen is 46.7% for

The percent by mass of nitrogen is 46.7% for a species containing only nitrogen and oxygen. Which of the following could be this species? a. N2O5 b. N2O c. NO2 d. NO e. NO3

Q: Calculate the number of molecules present in each of the following samples

Calculate the number of molecules present in each of the following samples. a. 4.75 mmol of phosphine, PH3 b. 4.75 g of phosphine, PH3 c. 1.25 * 10-2 g of lead(II) acetate, Pb(CH3CO2)2 d. 1.25 * 1...

Q: A system absorbs 215 kJ of heat, and 116 kJ of

A system absorbs 215 kJ of heat, and 116 kJ of work is done on it. Calculate ∆E.

Q: What mass of sodium hydroxide has the same number of oxygen atoms

What mass of sodium hydroxide has the same number of oxygen atoms as 100.0 g of ammonium carbonate?

Q: Write the conversion factors that would be necessary to perform each of

Write the conversion factors that would be necessary to perform each of the following conversions: a. an energy given in calories to its equivalent in joules b. an energy given in joules to its equi...

Q: Topical hydrocortisone is often used to treat a variety of skin conditions

Topical hydrocortisone is often used to treat a variety of skin conditions, such as insect bites, eczema, and rashes. Each molecule of hydrocortisone contains 21 atoms of carbon (plus other atoms). Th...

Q: If 8.40 kJ of heat is needed to raise the

If 8.40 kJ of heat is needed to raise the temperature of a sample of metal from 15 °C to 20 °C, how many kilojoules of heat will be required to raise the temperature of the same sample of metal from 2...

Q: If it takes 654 J of energy to warm a 5.

If it takes 654 J of energy to warm a 5.51-g sample of water, how much energy would be required to warm 55.1 g of water by the same amount?

Q: Convert the following numbers of calories or kilocalories into joules and kilojoules

Convert the following numbers of calories or kilocalories into joules and kilojoules (Remember: kilo means 1000.) a. 75.2 kcal b. 75.2 cal c. 1.41 * 103 cal d. 1.41 kcal

Q: Convert the following numbers of calories into kilocalories. (Remember:

Convert the following numbers of calories into kilocalories. (Remember: kilo means 1000.) a. 8254 cal b. 41.5 cal c. 8.231 * 103 cal d. 752,900 cal

Q: Calculate the number of moles for each compound in the following table

Calculate the number of moles for each compound in the following table.

Q: a. How many atoms of carbon are present in 1.

a. How many atoms of carbon are present in 1.0 g of CH4O? b. How many atoms of carbon are present in 1.0 g of CH3CH2OH? c. How many atoms of nitrogen are present in 25.0 g of CO(NH2)2?

Q: How are the different types of electromagnetic radiation similar? How do

How are the different types of electromagnetic radiation similar? How do they differ?

Q: Calculate the number of molecules present in each of the following samples

Calculate the number of molecules present in each of the following samples. a. 3.54 moles of sulfur dioxide, SO2 b. 3.54 g of sulfur dioxide, SO2 c. 4.46 * 1025 g of ammonia, NH3 d. 4.46 * 1025 mo...

Q: Convert the following numbers of kilojoules into kilocalories. (Remember:

Convert the following numbers of kilojoules into kilocalories. (Remember: kilo means 1000.) a. 652.1 kJ b. 1.00 kJ c. 4.184 kJ d. 4.351 * 103 kJ

Q: The chemical formula for aspirin is C9H8O4. What is the mass

The chemical formula for aspirin is C9H8O4. What is the mass percent for each element in 1 mole of aspirin? (Give your answer to four significant figures.)

Q: Arrange the following substances in order of increasing mass percent of nitrogen

Arrange the following substances in order of increasing mass percent of nitrogen. a. NO b. N2O c. NH3 d. SNH

Q: Perform the indicated conversions. a. 625.2 cal

Perform the indicated conversions. a. 625.2 cal into kilojoules b. 82.41 kJ into joules c. 52.61 kcal into joules d. 124.2 kJ into kilocalories

Q: What is the kinetic energy of a particle of mass m moving

What is the kinetic energy of a particle of mass m moving through space with velocity ν?

Q: Perform the indicated conversions. a. 91.74 kcal

Perform the indicated conversions. a. 91.74 kcal into calories b. 1.781 kJ into calories c. 4.318 * 103 J into kilocalories d. 9.173 * 104 cal into kilojoules

Q: If 69.5 kJ of heat is applied to a 1012

If 69.5 kJ of heat is applied to a 1012-g block of metal, the temperature of the metal increases by 11.4 8(C. Calculate the specific heat capacity of the metal in J/g 8(C.

Q: What quantity of heat energy must have been applied to a block

What quantity of heat energy must have been applied to a block of aluminum weighing 42.7 g if the temperature of the block of aluminum increased by 15.2 °C? (See Table 10.1.) Table 10.1

Q: If 125 J of heat energy is applied to a block of

If 125 J of heat energy is applied to a block of silver weighing 29.3 g, by how many degrees will the temperature of the silver increase? (See Table 10.1.)

Q: If 100. J of heat energy is applied to a 25

If 100. J of heat energy is applied to a 25-g sample of mercury, by how many degrees will the temperature of the sample of mercury increase? (See Table 10.1.)

Q: Calculate the number of moles of carbon atoms present in each of

Calculate the number of moles of carbon atoms present in each of the following samples. a. 1.271 g of ethanol, C2H5OH b. 3.982 g of 1,4-dichlorobenzene, C6H4Cl2 c. 0.4438 g of carbon suboxide, C3O2...

Q: What quantity of heat is required to raise the temperature of 55

What quantity of heat is required to raise the temperature of 55.5 g of gold from 20 8C to 45 8C? (See Table 10.1.)

Q: The “Chemistry in Focus” segment Coffee: Hot and Quick

The “Chemistry in Focus” segment Coffee: Hot and Quick(lime) discusses self-heating cups of coffee using the chemical reaction between quicklime, CaO(s), and water. Is this reaction endothermic or exo...

Q: In the “Chemistry in Focus” segment Firewalking: Magic or

In the “Chemistry in Focus” segment Firewalking: Magic or Science?, it is claimed that one reason people can walk on hot coals is that human tissue is mainly composed of water. Because of this, a larg...

Q: The enthalpy change for a reaction that occurs at constant pressure is

The enthalpy change for a reaction that occurs at constant pressure is (higher than/lower than/the same as) the heat for that reaction.

Q: The total energy of the universe is .

The total energy of the universe is .

Q: The “Chemistry in Focus” segment Burning Calories discusses calories in

The “Chemistry in Focus” segment Burning Calories discusses calories in food. If a food is said to contain 350 calories per serving, determine this value in terms of joules.

Q: Where did the energy stored in wood, coal, petroleum,

Where did the energy stored in wood, coal, petroleum, and natural gas originally come from?

Q: What does natural gas consist of? Where is natural gas commonly

What does natural gas consist of? Where is natural gas commonly found?

Q: What was tetraethyl lead used for in the petroleum industry? Why

What was tetraethyl lead used for in the petroleum industry? Why is it no longer commonly used?

Q: What does it mean to say that “energy spread” and

What does it mean to say that “energy spread” and “matter spread” are driving forces in chemical reactions?

Q: Calculate the number of moles of sulfur atoms present in each of

Calculate the number of moles of sulfur atoms present in each of the following samples. a. 2.01 g of sodium sulfate b. 2.01 g of sodium sulfite c. 2.01 g of sodium sulfide d. 2.01 g of sodium thio...

Q: If a reaction occurs readily but has an endothermic heat of reaction

If a reaction occurs readily but has an endothermic heat of reaction, what must be the driving force for the reaction?

Q: Does a double-displacement reaction such as NaCl(aq

Does a double-displacement reaction such as NaCl(aq) + AgNO3(aq) AgCl(s) + NaNO3(aq) result in a matter spread or in a concentration of matter?

Q: What do we mean by entropy? Why does the entropy of

What do we mean by entropy? Why does the entropy of the universe increase during a spontaneous process?

Q: A chunk of ice at room temperature melts, even though the

A chunk of ice at room temperature melts, even though the process is endothermic. Why?

Q: Which of the following is an endothermic process? a.

Which of the following is an endothermic process? a. combustion of gasoline in a car engine b. sublimation of carbon dioxide; CO2(s) CO2(g) c. water condensing on a cold pipe d. freezing...

Q: Which of the following statements is(are) true?

Which of the following statements is(are) true? a. Energy is changed in form in a process, but it is not produced or consumed. b. Heat is a flow of energy between two objects due to a temperature di...

Q: Perform the indicated conversions. a. 85.21 cal

Perform the indicated conversions. a. 85.21 cal into joules b. 672.1 J into calories c. 8.921 kJ into joules d. 556.3 cal into kilojoules

Q: Calculate the amount of energy required (in calories) to heat

Calculate the amount of energy required (in calories) to heat 145 g of water from 22.3 °C to 75.0 °C.

Q: It takes 1.25 kJ of energy to heat a certain

It takes 1.25 kJ of energy to heat a certain sample of pure silver from 12.0 °C to 15.2 °C. Calculate the mass of the sample of silver.

Q: Students often confuse what is meant by heat and temperature. Define

Students often confuse what is meant by heat and temperature. Define each. How are the two concepts related?

Q: Using the average atomic masses given inside the front cover of this

Using the average atomic masses given inside the front cover of this book, calculate the number of moles of each substance contained in the following masses. a. 2.01 * 10-2 g of silver b. 45.2 mg of...

Q: What quantity of heat energy would have to be applied to a

What quantity of heat energy would have to be applied to a 25.1-g block of iron in order to raise the temperature of the iron sample by 17.5 °C? (See Table 10.1.)

Q: The specific heat capacity of gold is 0.13 J/

The specific heat capacity of gold is 0.13 J/g °C. Calculate the specific heat capacity of gold in cal/g °C.

Q: Calculate the amount of energy required (in joules) to heat

Calculate the amount of energy required (in joules) to heat 2.5 kg of water from 18.5 °C to 55.0 °C.

Q: If 10. J of heat is applied to 5.0

If 10. J of heat is applied to 5.0-g samples of each of the substances listed in Table 10.1, which substance’s temperature will increase the most? Which substance’s temperature will increase the least...

Q: If 7.24 kJ of heat is applied to a 952

If 7.24 kJ of heat is applied to a 952-g block of metal, the temperature increases by 10.7 °C. Calculate the specific heat capacity of the metal in J/g °C.

Q: A system releases 213 kJ of heat and has a calculated ∆

A system releases 213 kJ of heat and has a calculated ∆E of -45 kJ. How much work was done on the system?

Q: Calculate ∆E for each of the following. a.

Calculate ∆E for each of the following. a. q = -47 kJ, w = +88 kJ b. q = +82 kJ, w = +47 kJ c. q = +47 kJ, w = 0 d. In which of these cases do the surroundings do work on the system?

Q: Calculate the enthalpy change when 5.00 g of propane is

Calculate the enthalpy change when 5.00 g of propane is burned with excess oxygen according to the reaction C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l) ∆H = -2221 kJ/mol

Q: Which of the following processes is(are) exothermic?

Which of the following processes is(are) exothermic? a. combustion of methane (e.g., Bunsen burner) b. melting of ice c. evaporation of acetone (e.g., fingernail polish remover) d. steam condensin...

Q: The specific heat capacity of graphite is 0.71 J/

The specific heat capacity of graphite is 0.71 J/g °C. Calculate the energy required to raise the temperature of 2.4 moles of graphite by 25.0 °C.

Q: Using the average atomic masses given inside the front cover of this

Using the average atomic masses given inside the front cover of this book, calculate the mass in grams of each of the following samples. a. 2.17 moles of germanium, Ge b. 4.24 mmol of lead(II) chlor...

Q: Consider the reaction B2H6(g) + 3O2(g

Consider the reaction B2H6(g) + 3O2(g) B2O3(s) + 3H2O(g) ∆H = -2035 kJ Calculate the amount of heat released when 54.0 g of diborane is combusted.

Q: The random motions of the components of an object constitute the of

The random motions of the components of an object constitute the of that object.

Q: An atom has a small charged core called the nucleus, with

An atom has a small charged core called the nucleus, with charged electrons moving in the space around the nucleus.

Q: The energy of a photon of visible light emitted by an excited

The energy of a photon of visible light emitted by an excited atom is the energy change that takes place within the atom itself.

Q: Light waves move through space at a speed of meters per second

Light waves move through space at a speed of meters per second.

Q: How does the attractive force that the nucleus exerts on an electron

How does the attractive force that the nucleus exerts on an electron change with the principal energy level of the electron?

Q: Based on the ground-state electron configuration of iodine, how

Based on the ground-state electron configuration of iodine, how many electrons occupy the p and d orbitals?

Q: Element X, which has a valence shell configuration of ns2np4,

Element X, which has a valence shell configuration of ns2np4, was isolated in a laboratory. Which of the following statements is(are) true concerning element X? a. Element X has chemical properties s...

Q: Write the full electron configuration (1s22s2, etc.) for each

Write the full electron configuration (1s22s2, etc.) for each of the following elements. a. bromine, Z = 35 b. xenon, Z = 54 c. barium, Z = 56 d. selenium, Z = 34

Q: Write the complete orbital diagram for each of the following elements,

Write the complete orbital diagram for each of the following elements, using boxes to represent orbitals and arrows to represent electrons. a. scandium, Z = 21 b. sulfur, Z = 16 c. potassium, Z = 1...

Q: Calculate the percent by mass of each element in the following compounds

Calculate the percent by mass of each element in the following compounds. a. HClO3 b. UF4 c. CaH2 d. Ag2S e. NaHSO3 f. MnO2

Q: What does the ground state of an atom represent?

What does the ground state of an atom represent?

Q: How many valence electrons does each of the following atoms have?

How many valence electrons does each of the following atoms have? a. nitrogen, Z = 7 b. chlorine, Z = 17 c. sodium, Z = 11 d. aluminum, Z = 13

Q: What name is given to the series of ten elements in which

What name is given to the series of ten elements in which the electrons are filling the 3d sublevel?

Q: Rank the following elements in order of increasing atomic size: Ge

Rank the following elements in order of increasing atomic size: Ge, S, F, Rb, Mn.

Q: Using the symbol of the previous noble gas to indicate core electrons

Using the symbol of the previous noble gas to indicate core electrons, write the valence shell electron configuration for each of the following elements. a. titanium, Z = 22 b. selenium, Z = 34 c....

Q: Arrange the following atoms in order of increasing size (assuming all

Arrange the following atoms in order of increasing size (assuming all atoms are in their ground states). a. [Kr]5s24d105p6 b. [Kr]5s24d105p1 c. [Kr]5s24d105p3

Q: Write the shorthand valence shell electron configuration of each of the following

Write the shorthand valence shell electron configuration of each of the following elements, basing your answer on the element’s location on the periodic table. a. nickel, Z = 28 b. niobium, Z = 41...

Q: Which of the following statements about the periodic table is false?

Which of the following statements about the periodic table is false? a. Elements in the same column have similar reactivities because their valence electrons tend to be located in the same types of o...

Q: In each of the following sets of elements, indicate which element

In each of the following sets of elements, indicate which element shows the most active chemical behavior. a. B, Al, In b. Na, Al, S c. B, C, F

Q: In each of the following sets of elements, indicate which element

In each of the following sets of elements, indicate which element has the smallest atomic size. a. Ba, Ca, Ra b. P, Si, Al c. Rb, Cs, K

Q: Calculate the percent by mass of each element in the following compounds

Calculate the percent by mass of each element in the following compounds. a. ZnO b. Na2S c. Mg(OH)2 d. H2O2 e. CaH2 f. K2O

Q: Determine the maximum number of electrons that can have each of the

Determine the maximum number of electrons that can have each of the following designations: 2f, 2dxy, 3p, 5dyz, and 4p.

Q: An excited atom can release some or all of its excess energy

An excited atom can release some or all of its excess energy by emitting a(n) and thus move to a lower energy state.

Q: Which of the following statements is(are) true?

Which of the following statements is(are) true? a. The 2s orbital in the hydrogen atom is larger than the 3s orbital also in the hydrogen atom. b. The Bohr model of the hydrogen atom has been found...

Q: Give the electron configurations for the following atoms. Do not use

Give the electron configurations for the following atoms. Do not use the noble gas notation. Write out the complete electron configuration.

Q: Identify the following three elements. a. The ground-

Identify the following three elements. a. The ground-state electron configuration is [Kr]5s24d105p4. b. The ground-state electron configuration is [Ar]4s23d104p2. c. An excited state of this elemen...

Q: Give the electron configurations for the following atoms. Use the noble

Give the electron configurations for the following atoms. Use the noble gas notation.

Q: Compare the atomic sizes of each pair of atoms. State the

Compare the atomic sizes of each pair of atoms. State the larger atom for each pair.

Q: Compare the ionization energies of each pair of atoms. State the

Compare the ionization energies of each pair of atoms. State the atom with the larger ionization energy for each pair.

Q: Three elements have the electron configurations 1s22s22p63s2, 1s22s22p63s23p4, and 1s22s22p63s23p64s2

Three elements have the electron configurations 1s22s22p63s2, 1s22s22p63s23p4, and 1s22s22p63s23p64s2. The first ionization energies of these elements (not in the same order) are 0.590, 0.999, and 0.7...

Q: How is the energy carried per photon of light related to the

How is the energy carried per photon of light related to the wavelength of the light? Does short-wavelength light carry more energy or less energy than long-wavelength light?

Q: Calculate the percent by mass of the element listed first in the

Calculate the percent by mass of the element listed first in the formulas for each of the following compounds. a. methane, CH4 b. sodium nitrate, NaNO3 c. carbon monoxide, CO d. nitrogen dioxide,...

Q: When an atom energy from outside, the atom goes from a

When an atom energy from outside, the atom goes from a lower energy state to a higher energy state.

Q: Because a given element’s atoms emit only certain photons of light,

Because a given element’s atoms emit only certain photons of light, only certain are occurring in those particular atoms.

Q: How does the energy possessed by an emitted photon compare to the

How does the energy possessed by an emitted photon compare to the difference in energy levels that gave rise to the emission of the photon?

Q: The energy levels of hydrogen (and other atoms) are said

The energy levels of hydrogen (and other atoms) are said to be , which means that only certain energy values are allowed.

Q: What questions were left unanswered by Rutherford’s experiments?

What questions were left unanswered by Rutherford’s experiments?

Q: When a tube containing hydrogen atoms is energized by passing several thousand

When a tube containing hydrogen atoms is energized by passing several thousand volts of electricity into the tube, the hydrogen emits light that, when passed through a prism, resolves into the â...

Q: What are the essential points of Bohr’s theory of the structure of

What are the essential points of Bohr’s theory of the structure of the hydrogen atom?

Q: According to Bohr, what happens to the electron when a hydrogen

According to Bohr, what happens to the electron when a hydrogen atom absorbs a photon of light of sufficient energy?

Q: Why was Bohr’s theory for the hydrogen atom initially accepted, and

Why was Bohr’s theory for the hydrogen atom initially accepted, and why was it ultimately discarded?

Q: Discuss briefly the difference between an orbit (as described by Bohr

Discuss briefly the difference between an orbit (as described by Bohr for hydrogen) and an orbital (as described by the more modern, wave mechanical picture of the atom).

Q: Calculate the percent by mass of the element listed first in the

Calculate the percent by mass of the element listed first in the formulas for each of the following compounds. a. copper(II) bromide, CuBr2 b. copper(I) bromide, CuBr c. iron(II) chloride, FeCl2 d...

Q: In the 1920s, de Broglie and Schrödinger developed what is now

In the 1920s, de Broglie and Schrödinger developed what is now called wave mechanics or quantum mechanics. Which of the following statements with regard to this model is(are) true? a. The position of...

Q: What is electromagnetic radiation? At what speed does electromagnetic radiation travel

What is electromagnetic radiation? At what speed does electromagnetic radiation travel?

Q: Consider the following representation of a set of p orbitals for an

Consider the following representation of a set of p orbitals for an atom: Which of the following statements is(are) true? a. The areas represented by the p orbitals are positively charged clouds wi...

Q: What are the differences between the 2s orbital and the 1s orbital

What are the differences between the 2s orbital and the 1s orbital of hydrogen? How are they similar?

Q: The higher the principal energy level, n, the (closer

The higher the principal energy level, n, the (closer to/farther from) the nucleus is the electron.

Q: When the electron in hydrogen is in the n = 3 principal

When the electron in hydrogen is in the n = 3 principal energy level, the atom is in a/an state.

Q: Complete the following table. /

Complete the following table.

Q: Calculate the percent by mass of the element listed first in the

Calculate the percent by mass of the element listed first in the formulas for each of the following compounds. a. adipic acid, C6H10O4 b. ammonium nitrate, NH4NO3 c. caffeine, C8H10N4O2 d. chlorin...

Q: Using the average atomic masses for each of the following elements (

Using the average atomic masses for each of the following elements (see the table inside the cover of this book), calculate the mass (in amu) of each of the following samples. a. 125 carbon atoms b....

Q: What is the mass percent of oxygen in each of the following

What is the mass percent of oxygen in each of the following compounds? a. carbon dioxide b. sodium nitrate c. iron(III) phosphate d. ammonium carbonate e. aluminum sulfate

Q: For each of the following samples of ionic substances, calculate the

For each of the following samples of ionic substances, calculate the number of moles and mass of the positive ions present in each sample. a. 4.25 g of ammonium iodide, NH4I b. 6.31 moles of ammoniu...

Q: For each of the following ionic substances, calculate the percentage of

For each of the following ionic substances, calculate the percentage of the overall molar mass of the compound that is represented by the negative ions in the substance. a. ammonium sulfide b. calci...

Q: Lead(II) oxide from an ore can be reduced to

Lead(II) oxide from an ore can be reduced to elemental lead by heating in a furnace with carbon. PbO(s) + C(s) Pb(l) + CO(g) Calculate the expected yield of lead if 50.0 kg of lead...

Q: If steel wool (iron) is heated until it glows and

If steel wool (iron) is heated until it glows and is placed in a bottle containing pure oxygen, the iron reacts spectacularly to produce iron(III) oxide. Fe(s) + O2(g) Fe2O3(s)...

Q: A common method for determining how much chloride ion is present in

A common method for determining how much chloride ion is present in a sample is to precipitate the chloride from an aqueous solution of the sample with silver nitrate solution and then to weigh the si...

Q: Although many sulfate salts are soluble in water, calcium sulfate is

Although many sulfate salts are soluble in water, calcium sulfate is not (Table 7.1). Therefore, a solution of calcium chloride will react with sodium sulfate solution to produce a precipitate of calc...

Q: A compound was analyzed and was found to contain the following percentages

A compound was analyzed and was found to contain the following percentages of the elements by mass: barium, 89.56%; oxygen, 10.44%. Determine the empirical formula of the compound.

Q: A compound was analyzed and was found to contain the following percentages

A compound was analyzed and was found to contain the following percentages of the elements by mass: nitrogen, 11.64%; chlorine, 88.36%. Determine the empirical formula of the compound.

Q: A 0.5998-g sample of a new compound has

A 0.5998-g sample of a new compound has been analyzed and found to contain the following masses of elements: carbon, 0.2322 g; hydrogen, 0.05848 g; oxygen, 0.3091 g. Calculate the empirical formula of...

Q: For each of the following reactions, give the balanced chemical equation

For each of the following reactions, give the balanced chemical equation for the reaction and state the meaning of the equation in terms of individual molecules and in terms of moles of molecules. a....

Q: A compound was analyzed and was found to contain the following percentages

A compound was analyzed and was found to contain the following percentages of the elements by mass: boron, 78.14%; hydrogen, 21.86%. Determine the empirical formula of the compound.

Q: If a 1.271-g sample of aluminum metal is

If a 1.271-g sample of aluminum metal is heated in a chlorine gas atmosphere, the mass of aluminum chloride produced is 6.280 g. Calculate the empirical formula of aluminum chloride.

Q: By now, you are familiar with enough chemical compounds to begin

By now, you are familiar with enough chemical compounds to begin to write your own chemical reaction equations. Write two examples each of what we mean by a synthesis reaction and by a decomposition r...

Q: A compound was analyzed and was found to contain the following percentages

A compound was analyzed and was found to contain the following percentages of the elements by mass: tin, 45.56%; chlorine, 54.43%. Determine the empirical formula of the compound.

Q: If cobalt metal is mixed with excess sulfur and heated strongly,

If cobalt metal is mixed with excess sulfur and heated strongly, a sulfide is produced that contains 55.06% cobalt by mass. Calculate the empirical formula of the sulfide.

Q: If 1.25 g of aluminum metal is heated in an

If 1.25 g of aluminum metal is heated in an atmosphere of fluorine gas, 3.89 g of aluminum fluoride results. Determine the empirical formula of aluminum fluoride.

Q: If 2.50 g of aluminum metal is heated in a

If 2.50 g of aluminum metal is heated in a stream of fluorine gas, it is found that 5.28 g of fluorine will combine with the aluminum. Determine the empirical formula of the compound that results.

Q: Distinguish between the molecular equation, the complete ionic equation, and

Distinguish between the molecular equation, the complete ionic equation, and the net ionic equation for a reaction in solution. Which type of equation most clearly shows the species that actually reac...

Q: A compound was analyzed and was found to contain the following percentages

A compound was analyzed and was found to contain the following percentages of the elements by mass: lithium, 46.46%; oxygen, 53.54%. Determine the empirical formula of the compound.

Q: A compound has the following percentage composition by mass: copper,

A compound has the following percentage composition by mass: copper, 33.88%; nitrogen, 14.94%; oxygen, 51.18%. Determine the empirical formula of the compound.

Q: For each of the following reactions, give the balanced equation for

For each of the following reactions, give the balanced equation for the reaction and state the meaning of the equation in terms of the numbers of individual molecules and in terms of moles of molecule...

Q: When lithium metal is heated strongly in an atmosphere of pure nitrogen

When lithium metal is heated strongly in an atmosphere of pure nitrogen, the product contains 59.78% Li and 40.22% N on a mass basis. Determine the empirical formula of the compound.

Q: For the cations listed in the left-hand column, give

For the cations listed in the left-hand column, give the formulas of the precipitates that would form with each of the anions in the right-hand column. If no precipitate is expected for a particular c...

Q: Tetraphenylporphyrin is a synthetic compound that resembles naturally occurring porphyrins. Porphyrins

Tetraphenylporphyrin is a synthetic compound that resembles naturally occurring porphyrins. Porphyrins are found in hemoglobin and cytochromes, which are important to biological functions in humans. T...

Q: On the basis of the general solubility rules given in Table 7

On the basis of the general solubility rules given in Table 7.1, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. If no precipitate is l...

Q: Phosphorus and chlorine form two binary compounds, in which the percentages

Phosphorus and chlorine form two binary compounds, in which the percentages of phosphorus are 22.55% and 14.87%, respectively. Calculate the empirical formulas of the two binary phosphorus–chlorine co...

Q: How does the molecular formula of a compound differ from the empirical

How does the molecular formula of a compound differ from the empirical formula? Can a compound’s empirical and molecular formulas be the same? Explain.

Q: A compound used in the nuclear industry has the following composition:

A compound used in the nuclear industry has the following composition: uranium, 67.61%; fluorine, 32.39%. Determine the empirical formula of the compound.

Q: A binary compound of boron and hydrogen has the following percentage composition

A binary compound of boron and hydrogen has the following percentage composition: 78.14% boron, 21.86% hydrogen. If the molar mass of the compound is determined by experiment to be between 27 and 28 g...

Q: A compound has been analyzed and has been found to have the

A compound has been analyzed and has been found to have the following composition: copper, 66.75%; phosphorus, 10.84%; oxygen, 22.41%. Determine the empirical formula of the compound.

Q: Using the average atomic masses given inside the front cover of the

Using the average atomic masses given inside the front cover of the text, calculate how many moles of each substance the following masses represent. a. 4.21 g of copper(II) sulfate b. 7.94 g of bari...

Q: If you spilled a cup of freshly brewed hot tea on yourself

If you spilled a cup of freshly brewed hot tea on yourself, you would be burned. If you spilled the same quantity of iced tea on yourself, you would not be burned. Explain.

Q: Balance the equation for each of the following oxidation– reduction chemical

Balance the equation for each of the following oxidation– reduction chemical reactions. a. Na(s) + O2(g) Na2O2(s) b. Fe(s) + H2SO4(aq) FeSO4(aq) + H2(g) c. Al2O3(s)...

Q: Identify each of the following unbalanced reaction equations as belonging to one

Identify each of the following unbalanced reaction equations as belonging to one or more of the following categories: precipitation, acid–base, or oxidation–reduction. a. Fe(s) + H2SO4(aq)...

Q: A compound containing only sulfur and nitrogen is 69.6%

A compound containing only sulfur and nitrogen is 69.6% S by mass. The molar mass is 184 g/mol. What is the correct name for this compound?

Q: Use the periodic table shown in Fig. 4.9 to

Use the periodic table shown in Fig. 4.9 to determine the atomic mass (per mole) or molar mass of each of the substances in column 1, and find that mass in column 2. Column 1…&ac...

Q: Complete the following table. /

Complete the following table.

Q: Write a balanced oxidation–reduction equation for the reaction of each

Write a balanced oxidation–reduction equation for the reaction of each of the metals in the left-hand column with each of the nonmetals in the right-hand column. Ba……………O2 K………………S Mg…………..Cl2 Rb………....

Q: Fill in the following table as if it is a well plate

Fill in the following table as if it is a well plate and you are mixing two aqueous compounds at a time to see if a precipitate forms. If a precipitate is expected to form, indicate that by writing th...

Q: Although the metals of Group 2 of the periodic table are not

Although the metals of Group 2 of the periodic table are not nearly as reactive as those of Group 1, many of the Group 2 metals will combine with common nonmetals, especially at elevated temperatures....

Q: When a 2.118-g sample of copper is heated

When a 2.118-g sample of copper is heated in an atmosphere in which the amount of oxygen present is restricted, the sample gains 0.2666 g of oxygen in forming a reddish-brown oxide. However, when 2.11...

Q: A compound having an approximate molar mass of 165–170 g

A compound having an approximate molar mass of 165–170 g has the following percentage composition by mass: carbon, 42.87%; hydrogen, 3.598%; oxygen, 28.55%; nitrogen, 25.00%. Determine the empirical a...

Q: Consider the balanced chemical equation 4Al(s) + 3O2

Consider the balanced chemical equation 4Al(s) + 3O2(g) 2Al2O3(s). What mole ratio would you use to calculate how many moles of oxygen gas would be needed to react comp...

Q: True or false? When solutions of barium hydroxide and sulfuric acid

True or false? When solutions of barium hydroxide and sulfuric acid are mixed, the net ionic equation is: Ba2+(aq) + SO42-(aq) BaSO4(s) because only the species involved in making t...

Q: Classify the reactions represented by the following unbalanced equations by as many

Classify the reactions represented by the following unbalanced equations by as many methods as possible. Balance the equations. a. I4O9(s) I2O6(s) + I2(s) + O2(g) b. Mg(s) +...

Q: Calculate the mass of carbon in grams, the percent carbon by

Calculate the mass of carbon in grams, the percent carbon by mass, and the number of individual carbon atoms present in each of the following samples. a. 7.819 g of carbon suboxide, C3O2 b. 1.53 * 1...

Q: Complete the following table. /

Complete the following table.

Q: Consider a hypothetical compound composed of elements X, Y, and

Consider a hypothetical compound composed of elements X, Y, and Z with the empirical formula X2YZ3. Given that the atomic masses of X, Y, and Z are 41.2, 57.7, and 63.9, respectively, calculate the pe...

Q: Give a balanced molecular chemical equation to illustrate each of the following

Give a balanced molecular chemical equation to illustrate each of the following types of reactions. a. a synthesis (combination) reaction b. a precipitation reaction c. a double-displacement reacti...

Q: A binary compound of magnesium and nitrogen is analyzed, and 1

A binary compound of magnesium and nitrogen is analyzed, and 1.2791 g of the compound is found to contain 0.9240 g of magnesium. When a second sample of this compound is treated with water and heated,...

Q: Calculate the number of atoms of each element present in each of

Calculate the number of atoms of each element present in each of the following samples. a. 4.21 g of water b. 6.81 g of carbon dioxide c. 0.000221 g of benzene, C6H6 d. 2.26 moles of C12H22O11

Q: Calculate the mass in grams of each of the following samples.

Calculate the mass in grams of each of the following samples. a. 10,000,000,000 nitrogen molecules b. 2.49 * 1020 carbon dioxide molecules c. 7.0983 moles of sodium chloride d. 9.012 * 10-6 moles...

Q: Calculate the mass in grams of hydrogen present in 2.500

Calculate the mass in grams of hydrogen present in 2.500 g of each of the following compounds. a. benzene, C6H6 b. calcium hydride, CaH2 c. ethyl alcohol, C2H5OH d. serine, C3H7O3N

Q: Which of the following substances exhibit hydrogen bonding interactions? a

Which of the following substances exhibit hydrogen bonding interactions? a. CCl2H2 b. BeF2 c. NO3- d. HCN

Q: What is steel?

What is steel?

Q: Some properties of potassium metal are summarized in the following table:

Some properties of potassium metal are summarized in the following table: Normal melting point…………………….63.5 °C Normal boiling point……………………765.7 °C Molar heat of fusion…………….2.334 kJ/mol Molar heat...

Q: Are changes in state physical or chemical changes for molecular solids?

Are changes in state physical or chemical changes for molecular solids? Why?

Q: Why is there no change in intramolecular forces when a solid is

Why is there no change in intramolecular forces when a solid is melted? Are intramolecular forces stronger or weaker than intermolecular forces?

Q: The molar heat of vaporization of carbon disulfide, CS2, is

The molar heat of vaporization of carbon disulfide, CS2, is 28.4 kJ/mol at its normal boiling point of 46 °C. How much energy (heat) is required to vaporize 1.0 g of CS2 at 46 °C? How much heat is evo...

Q: For each of the following sets of pressure/volume data,

For each of the following sets of pressure/volume data, calculate the new volume of the gas sample after the pressure change is made. Assume that the temperature and the amount of gas remain the same....

Q: Which is stronger, a dipole–dipole attraction between two molecules

Which is stronger, a dipole–dipole attraction between two molecules or a covalent bond between two atoms within the same molecule? Explain.

Q: For a liquid to boil, the intermolecular forces in the liquid

For a liquid to boil, the intermolecular forces in the liquid must be overcome. Based on the types of intermolecular forces present, arrange the expected boiling points of the liquid states of the fol...

Q: Discuss the types of intermolecular forces acting in the liquid state of

Discuss the types of intermolecular forces acting in the liquid state of each of the following substances. a. N2 b. NH3 c. He d. CO2 (linear, nonpolar)

Q: Discuss the types of intermolecular forces acting in the liquid state of

Discuss the types of intermolecular forces acting in the liquid state of each of the following substances. a. Ar b. H2O c. SeO2 d. BF3 (trigonal planar, nonpolar)

Q: What do we mean when we say a liquid is volatile?

What do we mean when we say a liquid is volatile? Do volatile liquids have large or small vapor pressures? What types of intermolecular forces occur in highly volatile liquids?

Q: Which type of bonding, ionic or covalent, generally results in

Which type of bonding, ionic or covalent, generally results in higher boiling points? Explain.

Q: What types of intermolecular forces exist in a crystal of ice?

What types of intermolecular forces exist in a crystal of ice? How do these forces differ from the types of intermolecular forces that exist in a crystal of solid oxygen?

Q: The envisions a metal as a cluster of positive ions through which

The envisions a metal as a cluster of positive ions through which the valence electrons are able to move freely.

Q: Water is unusual in that its solid form (ice) is

Water is unusual in that its solid form (ice) is less dense than its liquid form. Discuss some implications of this fact.

Q: Water at 100 °C (its normal boiling point) could

Water at 100 °C (its normal boiling point) could certainly give you a bad burn if it were spilled on the skin, but steam at 100 °C could give you a much worse burn. Explain.

Q: For each of the following sets of pressure/volume data,

For each of the following sets of pressure/volume data, calculate the new volume of the gas sample after the pressure change is made. Assume that the temperature and the amount of gas remain the same....

Q: Formaldehyde has the formula CH2O, where C is the central atom

Formaldehyde has the formula CH2O, where C is the central atom. The molecules in a sample of formaldehyde are attracted to each other by a combination of a. dipole–dipole forces and ionic forces. b....

Q: Draw the Lewis structures for the following species to assist you in

Draw the Lewis structures for the following species to assist you in answering the questions: SeCl2, ICl, BH3, NO2-. a. Which of the species is(are) polar? b. Which of the species exhibits hydrogen-b...

Q: The “Chemistry in Focus” segment Gorilla Glass discusses the glass

The “Chemistry in Focus” segment Gorilla Glass discusses the glass currently used for products such as smartphones. Which addition to common glass is not an ionic solid?

Q: The “Chemistry in Focus” segment Diamonds in the Ruff discusses

The “Chemistry in Focus” segment Diamonds in the Ruff discusses using the ashes of pets to produce diamonds. A diamond is an atomic solid. Why? Why are diamonds also referred to as network solids?

Q: Which of the following compound(s) exhibit only London dispersion

Which of the following compound(s) exhibit only London dispersion intermolecular forces? Which compound(s) exhibit hydrogen-bonding forces? Considering only the compounds without hydrogen-bonding inte...

Q: Identify the most important type of forces (ionic, hydrogen bonding

Identify the most important type of forces (ionic, hydrogen bonding, dipole–dipole, or London dispersion forces) among atoms or molecules present in the solids of each of the followi...

Q: Rank the following compounds from lowest to highest boiling point.

Rank the following compounds from lowest to highest boiling point. a. CH3CH2CH2Cl b. CH3CH2Cl c. CH3CH2CH2CH2Cl d. CH3Cl

Q: Rank the following compounds from lowest to highest melting point.

Rank the following compounds from lowest to highest melting point. a. CH4 b. MgO c. H2O d. H2S

Q: The energy required to break a given chemical bond is called the

The energy required to break a given chemical bond is called the .

Q: What sorts of elements react to form ionic compounds?

What sorts of elements react to form ionic compounds?

Q: For each of the following sets of pressure/volume data,

For each of the following sets of pressure/volume data, calculate the missing quantity. Assume that the temperature and the amount of gas remain constant. a. V = 19.3 L at 102.1 kPa; V = 10.0 L at ?...

Q: In general terms, what is a covalent bond?

In general terms, what is a covalent bond?

Q: Describe the type of bonding that exists in the Cl2(g

Describe the type of bonding that exists in the Cl2(g) molecule. How does this type of bonding differ from that found in the HCl(g) molecule? How is it similar?

Q: What are the common units used to measure pressure? Which unit

What are the common units used to measure pressure? Which unit is an experimental unit derived from the device used to measure atmospheric pressure?

Q: The relative ability of an atom in a molecule to attract electrons

The relative ability of an atom in a molecule to attract electrons to itself is called the atom’s .

Q: Make the indicated pressure conversions. a. 14.9

Make the indicated pressure conversions. a. 14.9 psi to atmospheres b. 795 torr to atmospheres c. 743 mm Hg to kilopascals d. 99,436 Pa to kilopascals

Q: A bond between atoms having a (small/large) difference

A bond between atoms having a (small/large) difference in electronegativity will be ionic.

Q: What factor determines the relative level of polarity of a polar covalent

What factor determines the relative level of polarity of a polar covalent bond?

Q: The introduction to this chapter says that “we live immersed in

The introduction to this chapter says that “we live immersed in a gaseous solution.” What does that mean?

Q: In each of the following groups, which element is the most

In each of the following groups, which element is the most electronegative? Which is the least electronegative? a. Cs, Ba, At b. Ba, Sr, Ra c. O, Rb, Mg

Q: On the basis of the electronegativity values given in Fig. 12

On the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be ionic, covalent, or polar covalent. a. O-O b. Al-O c. B-O From...

Q: The molar heat of fusion of benzene is 9.92 kJ

The molar heat of fusion of benzene is 9.92 kJ/mol. Its molar heat of vaporization is 30.7 kJ/mol. Calculate the heat required to melt 8.25 g of benzene at its normal melting point. Calculate the heat...

Q: On the basis of the electronegativity values given in Fig. 12

On the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be covalent, polar covalent, or ionic. a. S-S b. S-H c. S-K From...

Q: The volume of a sample of ideal gas is inversely proportional to

The volume of a sample of ideal gas is inversely proportional to the of the gas at constant temperature.

Q: A mathematical expression that summarizes Boyle’s law is .

A mathematical expression that summarizes Boyle’s law is .

Q: Make the indicated pressure conversions. a. 17.3

Make the indicated pressure conversions. a. 17.3 psi to kilopascals b. 1.15 atm to psi c. 4.25 atm to mm Hg d. 224 psi to atmospheres

Q: Pretend that you’re talking to a friend who has not yet taken

Pretend that you’re talking to a friend who has not yet taken any science courses, and describe how you would explain Boyle’s law to her.

Q: In Fig. 13.4, when additional mercury is added

In Fig. 13.4, when additional mercury is added to the righthand arm of the J-shaped tube, the volume of the gas trapped above the mercury in the left-hand arm of the J-tube decreases. Explain.

Q: Which bond in each of the following pairs has less ionic character

Which bond in each of the following pairs has less ionic character? a. Na-O or Na-N b. K-S or K-P c. Na-Cl or K-Cl d. Na-Cl or Mg-Cl

Q: What volume of gas would result if 225 mL of neon gas

What volume of gas would result if 225 mL of neon gas is compressed from 1.02 atm to 2.99 atm at constant temperature?

Q: Why is the presence of a dipole moment in the water molecule

Why is the presence of a dipole moment in the water molecule so important? What are some properties of water that are determined by its polarity?

Q: In each of the following diatomic molecules, which end of the

In each of the following diatomic molecules, which end of the molecule is negative relative to the other end? a. hydrogen chloride, HCl b. carbon monoxide, CO c. bromine monofluoride, BrF

Q: The molar heats of fusion and vaporization for water are 6.

The molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of liquid water is 4.18 J/g °C. What quantity of heat energy is requi...

Q: In each of the following diatomic molecules, which end of the

In each of the following diatomic molecules, which end of the molecule is positive relative to the other end? a. hydrogen fluoride, HF b. chlorine monofluoride, ClF c. iodine monochloride, ICl

Q: For each of the following bonds, draw a figure indicating the

For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative. a. C-F b. Si-C c. C-O d. B-C

Q: For each of the following bonds, draw a figure indicating the

For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative. a. S-P b. S-F c. S-Cl d. S-Br

Q: For each of the following bonds, draw a figure indicating the

For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative. a. Si-H b. P-H c. S-H d. Cl-H

Q: For each of the following bonds, draw a figure indicating the

For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative. a. H-C b. N-O c. N-S d. N-C

Q: A sample of gas in a balloon has an initial temperature of

A sample of gas in a balloon has an initial temperature of 18 °C and a volume of 1340 L. If the temperature changes to 87 °C and there is no overall change of pressure or amount of gas, what is the ne...

Q: The metallic elements lose electrons when reacting, and the resulting positive

The metallic elements lose electrons when reacting, and the resulting positive ions have an electron configuration analogous to the noble gas element.

Q: Nonmetals form negative ions by (losing/gaining) enough electrons

Nonmetals form negative ions by (losing/gaining) enough electrons to achieve the electron configuration of the next noble gas.

Q: If the pressure on a 1.04-L sample of

If the pressure on a 1.04-L sample of gas is doubled at constant temperature, what will be the new volume of the gas?

Q: A sample of helium gas with a volume of 29.2

A sample of helium gas with a volume of 29.2 mL at 785 mm Hg is compressed at constant temperature until its volume is 15.1 mL. What will be the new pressure in the sample?

Q: The boiling points of the noble gas elements are listed below.

The boiling points of the noble gas elements are listed below. Comment on the trend in the boiling points. Why do the boiling points vary in this manner?

Q: Which simple ion would each of the following elements be expected to

Which simple ion would each of the following elements be expected to form? Which noble gas has an analogous electron configuration to each of the ions? a. bromine, Z = 35 b. cesium, Z = 55 c. phosp...

Q: For each of the following numbers of electrons, give the formula

For each of the following numbers of electrons, give the formula of a positive ion that would have that number of electrons, and write the complete electron configuration for each ion. a. 10 electron...

Q: What is the expected ground-state electron configuration for Te-

What is the expected ground-state electron configuration for Te-2?

Q: If a 375-mL sample of neon gas is heated from

If a 375-mL sample of neon gas is heated from 24 °C to 72 °C at constant pressure, what will be the volume of the sample at the higher temperature?

Q: A sample of gas has a volume of 127 mL in a

A sample of gas has a volume of 127 mL in a boiling water bath at 100 °C. Calculate the volume of the sample of gas at 10 °C intervals after the heat source is turned off and the gas sample begins to...

Q: Name the noble gas atom that has the same electron configuration as

Name the noble gas atom that has the same electron configuration as each of the ions in the following compounds. a. barium sulfide, BaS b. strontium fluoride, SrF2 c. magnesium oxide, MgO d. alumi...

Q: Atoms form ions so as to achieve electron configurations similar to those

Atoms form ions so as to achieve electron configurations similar to those of the noble gases. For the following pairs of noble gas configurations, give the formulas of two simple ionic compounds that...

Q: Is the formula we write for an ionic compound the molecular formula

Is the formula we write for an ionic compound the molecular formula or the empirical formula? Why?

Q: If 1.04 g of chlorine gas occupies a volume of

If 1.04 g of chlorine gas occupies a volume of 872 mL at a particular temperature and pressure, what volume will 2.08 g of chlorine gas occupy under the same conditions?

Q: Why are cations always smaller than the atoms from which they are

Why are cations always smaller than the atoms from which they are formed?

Q: The normal boiling point of water is unusually high, compared to

The normal boiling point of water is unusually high, compared to the boiling points of H2S, H2Se, and H2Te. Explain this observation in terms of the hydrogen bonding that exists in water, but that doe...

Q: Why are anions always larger than the atoms from which they are

Why are anions always larger than the atoms from which they are formed?

Q: What pressure (in atmospheres) is required to compress 1.

What pressure (in atmospheres) is required to compress 1.00 L of gas at 760. mm Hg pressure to a volume of 50.0 mL?

Q: Under what conditions do real gases behave most ideally?

Under what conditions do real gases behave most ideally?

Q: Pretend that you’re talking to a friend who has not yet taken

Pretend that you’re talking to a friend who has not yet taken any science courses, and describe how you would explain the concept of absolute zero to him.

Q: Figures 13.7 and 13.8 show volume/temperature

Figures 13.7 and 13.8 show volume/temperature data for several samples of gases. Why do all the lines seem to extrapolate to the same point at 2273 °C? Explain.

Q: Why are the valence electrons of an atom the only electrons likely

Why are the valence electrons of an atom the only electrons likely to be involved in bonding to other atoms?

Q: The volume of a sample of ideal gas is proportional to its

The volume of a sample of ideal gas is proportional to its temperature (K) at constant pressure.

Q: What type of structure must each atom in a compound usually exhibit

What type of structure must each atom in a compound usually exhibit for the compound to be stable?

Q: When elements in the second and third periods occur in compounds,

When elements in the second and third periods occur in compounds, what number of electrons in the valence shell represents the most stable electron arrangement? Why?

Q: How many electrons are involved when two atoms in a molecule are

How many electrons are involved when two atoms in a molecule are connected by a “double bond”? Write the Lewis structure of a molecule containing a double bond.

Q: What does it mean when we say that in forming bonds,

What does it mean when we say that in forming bonds, atoms try to achieve an electron configuration analogous to a noble gas?

Q: What does it mean when two atoms in a molecule are connected

What does it mean when two atoms in a molecule are connected by a “triple bond”? Write the Lewis structure of a molecule containing a triple bond.

Q: Write the simple Lewis structure for each of the following atoms.

Write the simple Lewis structure for each of the following atoms. a. I (Z = 53) b. Al (Z = 13) c. Xe (Z = 54) d. Sr (Z = 38)

Q: Write the simple Lewis structure for each of the following atoms.

Write the simple Lewis structure for each of the following atoms. a. Mg (Z = 12) b. Br (Z = 35) c. S (Z = 16) d. Si (Z = 14)

Q: At what temperature will a 1.0-g sample of

At what temperature will a 1.0-g sample of neon gas exert a pressure of 500. torr in a 5.0-L container?

Q: At what temperature would 4.25 g of oxygen gas,

At what temperature would 4.25 g of oxygen gas, O2, exert a pressure of 784 mm Hg in a 2.51-L container?

Q: What pressure exists in a 200-L tank containing 5.

What pressure exists in a 200-L tank containing 5.0 kg of neon gas at 300. K?

Q: Which flask will have the higher pressure: a 5.00

Which flask will have the higher pressure: a 5.00-L flask containing 4.15 g of helium at 298 K, or a 10.0-L flask containing 56.2 g of argon at 303 K?

Q: Suppose a 24.3-mL sample of helium gas at

Suppose a 24.3-mL sample of helium gas at 25 °C and 1.01 atm is heated to 50. °C and compressed to a volume of 15.2 mL. What will be the pressure of the sample?

Q: Which of the following species exhibits resonance? CH4, OCl2

Which of the following species exhibits resonance? CH4, OCl2, NO2-, HCN (C is the central atom)

Q: The “Chemistry in Focus” segment Broccoli—Miracle Food?

The “Chemistry in Focus” segment Broccoli—Miracle Food? discusses the health benefits of eating broccoli and gives a Lewis structure for sulforaphane, a chemical in broccoli. Draw possible resonance s...

Q: Figure 13.1 shows an experiment that can be used effectively

Figure 13.1 shows an experiment that can be used effectively to demonstrate the pressure exerted by the atmosphere. Write an explanation of this experiment to a friend who has not yet taken any scienc...

Q: When 50 mL of liquid water at 25 °C is added

When 50 mL of liquid water at 25 °C is added to 50 mL of ethanol (ethyl alcohol), also at 25 °C, the combined volume of the mixture is considerably less than 100 mL. Give a possible explanation.

Q: The “Chemistry in Focus” segment Hiding Carbon Dioxide discusses attempts

The “Chemistry in Focus” segment Hiding Carbon Dioxide discusses attempts at sequestering (storing) underground CO2 produced at power plants so as to diminish the greenhouse effect. Draw all resonance...

Q: A mathematical expression that summarizes Charles’s law is .

A mathematical expression that summarizes Charles’s law is .

Q: Suppose a 375-mL sample of neon gas at 78 °

Suppose a 375-mL sample of neon gas at 78 °C is cooled to 22 °C at constant pressure. What will be the new volume of the neon sample?

Q: Suppose 1.25 L of argon is cooled from 291 K

Suppose 1.25 L of argon is cooled from 291 K to 78 K. What will be the new volume of the argon sample?

Q: Suppose a 125-mL sample of argon is cooled from 450

Suppose a 125-mL sample of argon is cooled from 450 K to 250 K at constant pressure. What will be the volume of the sample at the lower temperature?

Q: What is the geometric structure of the water molecule? How many

What is the geometric structure of the water molecule? How many pairs of valence electrons are there on the oxygen atom in the water molecule? What is the approximate H-O-H bond angle in water?

Q: What is the geometric structure of the ammonia molecule? How many

What is the geometric structure of the ammonia molecule? How many pairs of electrons surround the nitrogen atom in NH3? What is the approximate H-N-H bond angle in ammonia?

Q: What is the geometric structure of the boron trifluoride molecule, BF3

What is the geometric structure of the boron trifluoride molecule, BF3? How many pairs of valence electrons are present on the boron atom in BF3? What are the approximate F-B-F bond angles in BF3?

Q: What is the geometric structure of the SiF4 molecule? How many

What is the geometric structure of the SiF4 molecule? How many pairs of valence electrons are present on the silicon atom of SiF4? What are the approximate F-Si-F bond angles in SiF4?

Q: Why is the geometric structure of a molecule important, especially for

Why is the geometric structure of a molecule important, especially for biological molecules?

Q: For each of the following sets of volume/temperature data,

For each of the following sets of volume/temperature data, calculate the missing quantity after the change is made. Assume that the pressure and the amount of gas remain the same. a. V = 2.03 L at 24...

Q: At conditions of constant temperature and pressure, the volume of a

At conditions of constant temperature and pressure, the volume of a sample of ideal gas is proportional to the number of moles of gas present.

Q: How is the structure around a given atom related to repulsion between

How is the structure around a given atom related to repulsion between valence electron pairs on the atom?

Q: Why are all diatomic molecules linear, regardless of the number of

Why are all diatomic molecules linear, regardless of the number of valence electron pairs on the atoms involved?

Q: What do we assume about the volume of the actual molecules themselves

What do we assume about the volume of the actual molecules themselves in a sample of gas, compared to the bulk volume of the gas overall? Why?

Q: Although both the BF3 and NF3 molecules contain the same number of

Although both the BF3 and NF3 molecules contain the same number of atoms, the BF3 molecule is flat, whereas the NF3 molecule is trigonal pyramidal. Explain.

Q: Temperature is a measure of the average of the molecules in a

Temperature is a measure of the average of the molecules in a sample of gas.

Q: For the indicated atom in each of the following molecules or ions

For the indicated atom in each of the following molecules or ions, give the number and arrangement of the electron pairs around that atom. a. S in SO32- b. S in HSO3- c. S in HS-

Q: Using the VSEPR theory, predict the molecular structure of each of

Using the VSEPR theory, predict the molecular structure of each of the following molecules. a. NCl3 b. H2Se c. SiCl4

Q: Using the VSEPR theory, predict the molecular structure of each of

Using the VSEPR theory, predict the molecular structure of each of the following molecules. a. CBr4 b. PH3 c. OCl2

Q: Using the VSEPR theory, predict the molecular structure of each of

Using the VSEPR theory, predict the molecular structure of each of the following polyatomic ions. a. sulfate ion, SO42- b. phosphate ion, PO43- c. ammonium ion, NH4+

Q: Explain how the atoms in covalent molecules achieve electron configurations similar to

Explain how the atoms in covalent molecules achieve electron configurations similar to those of the noble gases. How does this differ from the situation in ionic compounds?

Q: What conditions are considered “standard temperature and pressure” (STP

What conditions are considered “standard temperature and pressure” (STP) for gases? Suggest a reason why these particular conditions might have been chosen for STP.

Q: For each of the following molecules or ions, indicate the bond

For each of the following molecules or ions, indicate the bond angle expected between the central atom and any two adjacent hydrogen atoms. a. H2O b. NH3 c. NH4+ d. CH4

Q: For each of the following molecules or ions, indicate the bond

For each of the following molecules or ions, indicate the bond angle expected between the central atom and any two adjacent chlorine atoms. a. Cl2O b. NCl3 c. CCl4 d. C2Cl4

Q: The “Chemistry in Focus” segment Taste—It’s the Structure

The “Chemistry in Focus” segment Taste—It’s the Structure That Counts discusses artificial sweeteners. What are the expected bond angles around the nitrogen atom in aspartame?

Q: A mathematical expression that summarizes Avogadro’s law is .

A mathematical expression that summarizes Avogadro’s law is .

Q: Consider the following order: Li < N < F. For

Consider the following order: Li < N < F. For which of the following properties does the order show the correct trend? a. size b. electronegativity c. metallic character d. number of unpaired elec...

Q: In ionic bonding, a. the electrons are shared between

In ionic bonding, a. the electrons are shared between the atoms. b. the process of forming an ionic bond is highly endothermic overall. c. the bonding that occurs is usually between two nonmetal at...

Q: The geometric arrangement of electron pairs around a given atom is determined

The geometric arrangement of electron pairs around a given atom is determined principally by the tendency to minimize between the electron pairs.

Q: Arrange the following bonds from the least polar to the most polar

Arrange the following bonds from the least polar to the most polar bond: C-F, Na-F, Ga-F, Si-F

Q: In each case, which of the following pairs of bonded elements

In each case, which of the following pairs of bonded elements forms the more polar bond? a. Br-Cl or Br-F b. As-S or As-O c. Pb-C or Pb-Si

Q: Which simple ion would each of the following elements be expected to

Which simple ion would each of the following elements be expected to form? What noble gas has an analogous electron configuration to each of the ions? a. chlorine, Z = 17 b. strontium, Z = 38 c. ox...

Q: Which of the following statements is false concerning bonding? a

Which of the following statements is false concerning bonding? a. Elements with extremely different electronegativities tend to form ionic bonds with each other. b. In an N-O bond, electron density...

Q: A(n) chemical bond represents the equal sharing of a

A(n) chemical bond represents the equal sharing of a pair of electrons between two nuclei.

Q: For each of the following pairs of elements, identify which element

For each of the following pairs of elements, identify which element would be expected to be more electronegative. It should not be necessary to look at a table of actual electronegativity values. a....

Q: On the basis of the electronegativity values given in Fig. 12

On the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be ionic, covalent, or polar covalent. a. H-O b. O-O c. H-H d. H-...

Q: Which of the following molecules contain polar covalent bonds? a

Which of the following molecules contain polar covalent bonds? a. carbon monoxide, CO b. chlorine, Cl2 c. iodine monochloride, ICl d. phosphorus, P4

Q: Consider the following unbalanced chemical equation for the combination reaction of sodium

Consider the following unbalanced chemical equation for the combination reaction of sodium metal and chlorine gas: Na(s) + Cl2(g) / NaCl(s) What volume of chlorine gas, measured at STP, is necessary...

Q: The electrons involved in a C-F bond could be considered

The electrons involved in a C-F bond could be considered a. closer to C because carbon has a larger radius and thus exerts greater control over the shared electrons. b. closer to F because fluorine...

Q: For each of the following bonds, draw a figure indicating the

For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative. a. N-Cl b. N-P c. N-S d. N-C

Q: Which of the following contains a metal ion that does not have

Which of the following contains a metal ion that does not have a noble gas electron configuration? AgCl, BaCl2, TiO2, ScF3, KNO3

Q: What simple ion does each of the following elements most commonly form

What simple ion does each of the following elements most commonly form? a. sodium b. iodine c. potassium d. calcium e. sulfur f. magnesium g. aluminum h. nitrogen

Q: For each of the following sets of volume/temperature data,

For each of the following sets of volume/temperature data, calculate the missing quantity. Assume that the pressure and the mass of gas remain constant. a. V = 2.01 * 102 L at 1150 °C; V = 5.00 L at...

Q: A widely used weather instrument called a barometer can be built from

A widely used weather instrument called a barometer can be built from a long, thin tube of glass that is sealed at one end. The tube is completely filled with mercury and then inverted into a small po...

Q: Which noble gas has the same electron configuration as each of the

Which noble gas has the same electron configuration as each of the ions in the following compounds? a. calcium bromide, CaBr2 b. aluminum selenide, Al2Se3 c. strontium oxide, SrO d. potassium sulf...

Q: For each of the following pairs, indicate which is smaller.

For each of the following pairs, indicate which is smaller. a. Rb+ or Na+ b. Mg2+ or Al3+ c. F- or I- d. Na+ or K+

Q: Write the Lewis structure for each of the following atoms.

Write the Lewis structure for each of the following atoms. a. He (Z = 2) b. Br (Z = 35) c. Sr (Z = 38) d. Ne (Z = 10) e. I (Z = 53) f. Ra (Z = 88)

Q: Welders commonly use an apparatus that contains a tank of acetylene (

Welders commonly use an apparatus that contains a tank of acetylene (C2H2) gas and a tank of oxygen gas. When burned in pure oxygen, acetylene generates a large amount of heat. 2C2H2(g) + 5O2(g) / 2H2...

Q: Consider the following reaction: Zn(s)+ 2HCl(

Consider the following reaction: Zn(s)+ 2HCl(aq) ZnCl2(aq) + H2(g) What mass of zinc metal should be taken so as to produce 125 mL of H2 measured at STP when reacted with excess...

Q: Select which of the following ions has the Lewis structure:

Select which of the following ions has the Lewis structure: a. B22- b. C22- c. N22- d. O22- e. F22-

Q: Write a Lewis structure for each of the following simple molecules.

Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those molecules that exhibit...

Q: Chemicals placed in a microwave oven and exposed to microwave radiation can

Chemicals placed in a microwave oven and exposed to microwave radiation can increase in temperature if they possess a net dipole moment. Which of the following molecules can get hot in an operating mi...

Q: Sulfur trioxide, SO3, is produced in enormous quantities each year

Sulfur trioxide, SO3, is produced in enormous quantities each year for use in the synthesis of sulfuric acid. S(s) + O2(g) SO2(g) 2SO2(g) + O2(g) 2SO3(g) What volume...

Q: For each of the following sets of volume/temperature data,

For each of the following sets of volume/temperature data, calculate the missing quantity. Assume that the pressure and the mass of gas remain constant. a. V = 25.0 L at 0 °C; V = 50.0 L at? °C b. V...

Q: For the indicated atom in each of the following molecules, give

For the indicated atom in each of the following molecules, give the number and the arrangement of the electron pairs around that atom. a. C in CCl4 b. Ge in GeH4 c. B in BF3

Q: Using the VSEPR theory, predict the molecular structure of each of

Using the VSEPR theory, predict the molecular structure of each of the following molecules. a. Cl2O b. OF2 c. SiCl4

Q: Using the VSEPR theory, predict the molecular structure of each of

Using the VSEPR theory, predict the molecular structure of each of the following polyatomic ions. a. chlorate ion b. chlorite ion c. perchlorate ion

Q: For each of the following molecules, indicate the bond angle expected

For each of the following molecules, indicate the bond angle expected between the central atom and any two adjacent chlorine atoms. a. Cl2O b. CCl4 c. BeCl2 d. BCl3

Q: Using the VSEPR theory, predict the molecular structure of each of

Using the VSEPR theory, predict the molecular structure of each of the following molecules or ions containing multiple bonds. a. SO2 b. SO3 c. HCO3- (hydrogen is bonded to oxygen) d. HCN

Q: Using the VSEPR theory, predict the molecular structure of each of

Using the VSEPR theory, predict the molecular structure of each of the following molecules or ions containing multiple bonds. a. CO32- b. HNO3 (hydrogen is bonded to oxygen) c. NO2- d. C2H2

Q: What is the expected ground-state electron configuration for the element

What is the expected ground-state electron configuration for the element with one unpaired 5p electron that forms a covalent compound with fluorine?

Q: When doing any calculation involving gas samples, we must express the

When doing any calculation involving gas samples, we must express the temperature in terms of the temperature scale.

Q: Classify the bonding in each of the following molecules as ionic,

Classify the bonding in each of the following molecules as ionic, polar covalent, or nonpolar covalent. a. H2 b. K3P c. NaI d. SO2 e. HF f. CCl4 g. CF4 h. K2S

Q: Compare the electronegativities of each pair of atoms. State the element

Compare the electronegativities of each pair of atoms. State the element of each pair that has the greater electronegativity.

Q: For each of the following sets of volume/temperature data,

For each of the following sets of volume/temperature data, calculate the missing quantity after the change is made. Assume that the pressure and the amount of gas remain the same. a. V = 9.14 L at 24...

Q: List the bonds P-Cl, P-F, O

List the bonds P-Cl, P-F, O-F, and Si-F from least polar to most polar.

Q: For a mixture of gases in the same container, the total

For a mixture of gases in the same container, the total pressure exerted by the mixture of gases is the of the pressures that those gases would exert if they were alone...

Q: Write electron configurations for the most stable ion formed by each of

Write electron configurations for the most stable ion formed by each of the following elements. Do not use the noble gas notation. Write out the complete electron configuration.

Q: Which of the following compounds or ions exhibit resonance? a

Which of the following compounds or ions exhibit resonance? a. O3 b. CNO- c. AsI3 d. CO32- e. AsF3

Q: The formulas of several chemical substances are given in the table below

The formulas of several chemical substances are given in the table below. For each substance in the table, give its chemical name and predict its molecular structure.

Q: Carbon dioxide gas, in the dry state, may be produced

Carbon dioxide gas, in the dry state, may be produced by heating calcium carbonate. CaCO3(s) / CaO(s) + CO2(g) What volume of CO2, collected dry at 55 °C and a pressure of 774 torr, is produced by co...

Q: You have 1 mole of an ideal gas in a balloon.

You have 1 mole of an ideal gas in a balloon. How must the volume change so that the pressure in the balloon doubles and the temperature in °C is halved (assume the temperature is a positive value)?...

Q: What is the pressure inside a 10.0-L flask

What is the pressure inside a 10.0-L flask containing 14.2 g of N2 at 26 °C?

Q: Suppose two separate 100.0-L tanks are to be

Suppose two separate 100.0-L tanks are to be filled, one with helium and one with hydrogen. What mass of each gas is needed to produce a pressure of 2.70 atm in its respective tank at 24 °C?

Q: At what temperature does 4.00 g of helium gas have

At what temperature does 4.00 g of helium gas have a pressure of 1.00 atm in a 22.4-L vessel?

Q: On the basis of their electron configurations, predict the formula of

On the basis of their electron configurations, predict the formula of the simple binary ionic compounds likely to form when the following pairs of elements react with each other. a. aluminum, Al, and...

Q: If 10.0 g of liquid helium at 1.7

If 10.0 g of liquid helium at 1.7 K is completely vaporized, what volume does the helium occupy at STP?

Q: If 0.214 mole of argon gas occupies a volume of

If 0.214 mole of argon gas occupies a volume of 652 mL at a particular temperature and pressure, what volume would 0.375 mole of argon occupy under the same conditions?

Q: Convert the following pressures into mm Hg. a. 0

Convert the following pressures into mm Hg. a. 0.903 atm b. 2.1240 * 106 Pa c. 445 kPa d. 342 torr

Q: If the pressure on a 2.10 * 104 mL sample

If the pressure on a 2.10 * 104 mL sample of gas is doubled at constant temperature, what will be the new volume of the gas?

Q: A sample of a gas at 0.780 atm occupies a

A sample of a gas at 0.780 atm occupies a volume of 0.501 L. If the temperature remains constant, what will be the new pressure if the volume increases to 0.794 L?

Q: An expandable vessel contains 729 mL of gas at 22 °C

An expandable vessel contains 729 mL of gas at 22 °C. What volume will the gas sample in the vessel have if it is placed in a boiling water bath (100. °C)?

Q: If a gaseous mixture is made of 3.50 g of

If a gaseous mixture is made of 3.50 g of He and 5.75 g of Ar in an evacuated 2.05-L container at 25 °C, what will be the partial pressure of Ar in the container?

Q: If a 0.475-L sample of neon gas is

If a 0.475-L sample of neon gas is heated from 27 °C to 82 °C at constant pressure, what will be the volume of the sample at the higher temperature?

Q: If 5.12 g of oxygen gas occupies a volume of

If 5.12 g of oxygen gas occupies a volume of 6.21 L at a certain temperature and pressure, what volume will 25.0 g of oxygen gas occupy under the same conditions?

Q: If 0.00901 mole of neon gas at a particular temperature

If 0.00901 mole of neon gas at a particular temperature and pressure occupies a volume of 242 mL, what volume would 0.00703 mole of neon occupy under the same conditions?

Q: On the basis of their electron configurations, predict the formula of

On the basis of their electron configurations, predict the formula of the simple binary ionic compound likely to form when the following pairs of elements react with each other. a. aluminum and bromi...

Q: If 3.25 moles of argon gas occupies a volume of

If 3.25 moles of argon gas occupies a volume of 100. L at a particular temperature and pressure, what volume does 14.15 moles of argon occupy under the same conditions?

Q: If 2.71 g of argon gas occupies a volume of

If 2.71 g of argon gas occupies a volume of 4.21 L, what volume will 1.29 moles of argon occupy under the same conditions?

Q: If two gases that do not react with each other are placed

If two gases that do not react with each other are placed in the same container, they will completely with each other.

Q: What mass of neon gas is required to fill a 5.

What mass of neon gas is required to fill a 5.00-L container to a pressure of 1.02 atm at 25 °C?

Q: Why are the dipole–dipole interactions between polar molecules not important

Why are the dipole–dipole interactions between polar molecules not important in the vapor phase?

Q: Describe a simple mercury barometer. How is such a barometer used

Describe a simple mercury barometer. How is such a barometer used to measure the pressure of the atmosphere?

Q: On the basis of the smaller units that make up the crystals

On the basis of the smaller units that make up the crystals, cite three types of crystalline solids. For each type of crystalline solid, give an example of a substance that forms that type of solid.

Q: How do ionic solids differ in structure from molecular solids? What

How do ionic solids differ in structure from molecular solids? What are the fundamental particles in each? Give two examples of each type of solid and indicate the individual particles that make up th...

Q: Describe in general terms the structure of ionic solids such as NaCl

Describe in general terms the structure of ionic solids such as NaCl. How are the ions packed in the crystal?

Q: Ionic solids are generally considerably harder than most molecular solids. Explain

Ionic solids are generally considerably harder than most molecular solids. Explain.

Q: When dry ammonia gas (NH3) is bubbled into a 125

When dry ammonia gas (NH3) is bubbled into a 125-mL sample of water, the volume of the sample (initially, at least) decreases slightly. Suggest a reason for this.

Q: For each of the following pairs, indicate which species is smaller

For each of the following pairs, indicate which species is smaller. Explain your reasoning in terms of the electron structure of each species. a. H or H- b. N or N3- c. Al or Al3+ d. F or Cl

Q: For each of the following pairs, indicate which species is larger

For each of the following pairs, indicate which species is larger. Explain your reasoning in terms of the electron structure of each species. a. Mg2+ or Mg b. Ca2+ or K+ c. Rb+ or Br- d. Se2- or S...

Q: For each of the following pairs, indicate which is smaller.

For each of the following pairs, indicate which is smaller. a. Fe or Fe3+ b. Cl or Cl- c. Al3+ or Na+

Q: For each of the following pairs, indicate which is larger.

For each of the following pairs, indicate which is larger. a. I or F b. F or F- c. Na+ or F-

Q: Given the following sets of values for three of the gas variables

Given the following sets of values for three of the gas variables, calculate the unknown quantity. a. P = 782.4 mm Hg; V = ?; n = 0.1021 mol; T = 26.2 °C b. P = ? mm Hg; V = 27.5 mL; n = 0.007812 mol...

Q: Consider a sample of ice being heated from -5 °C

Consider a sample of ice being heated from -5 °C to +5 °C. Describe on both a macroscopic and a microscopic basis what happens to the ice as the temperature reaches 0 °C.

Q: Explain what the “duet” and “octet” rules are

Explain what the “duet” and “octet” rules are and how they are used to describe the arrangement of electrons in a molecule.

Q: What do we mean by an ideal gas?

What do we mean by an ideal gas?

Q: Show how Boyle’s gas law can be derived from the ideal gas

Show how Boyle’s gas law can be derived from the ideal gas law.

Q: Show how Charles’s gas law can be derived from the ideal gas

Show how Charles’s gas law can be derived from the ideal gas law.

Q: Given each of the following sets of values for an ideal gas

Given each of the following sets of values for an ideal gas, calculate the unknown quantity. a. P = 782 mm Hg; V =? n = 0.210 mol; T = 27 °C b. P =? mm Hg; V = 644 mL; n = 0.0921 mol; T = 303 K c....

Q: What mass of helium gas is needed to pressurize a 100.

What mass of helium gas is needed to pressurize a 100.0-L tank to 255 atm at 25 °C? What mass of oxygen gas would be needed to pressurize a similar tank to the same specifications?

Q: If you’ve ever opened a bottle of rubbing alcohol or other solvent

If you’ve ever opened a bottle of rubbing alcohol or other solvent on a warm day, you may have heard a little “whoosh” as the vapor that had built up above the liquid escapes. Describe on a microscopi...

Q: Give the total number of valence electrons in each of the following

Give the total number of valence electrons in each of the following molecules. a. N2O b. B2H6 c. C3H8 d. NCl3

Q: Give the total number of valence electrons in each of the following

Give the total number of valence electrons in each of the following molecules. a. B2O3 b. CO2 c. C2H6O d. NO2

Q: Write a Lewis structure for each of the following simple molecules.

Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. a. NBr3 b. HF c. CBr4 d. C2H...

Q: Compare and contrast the bonding found in the H2 (g)

Compare and contrast the bonding found in the H2 (g) and HF(g) molecules with that found in NaF(s).

Q: Write a Lewis structure for each of the following simple molecules.

Write a Lewis structure for each of the following simple molecules. Show all bonding valence electrons pairs as lines and all nonbonding valence electron pairs as dots. a. H2S b. SiF4 c. C2H4 d. C...

Q: Write a Lewis structure for each of the following simple molecules.

Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. a. C2H6 b. NF3 c. C4H10 d. S...

Q: In carbon compounds a given group of atoms can often be arranged

In carbon compounds a given group of atoms can often be arranged in more than one way. This means that more than one structure may be possible for the same atoms. For example, both the molecules dieth...

Q: What do we mean by a dynamic equilibrium? Describe how the

What do we mean by a dynamic equilibrium? Describe how the development of a vapor pressure above a liquid represents such an equilibrium.

Q: Consider Fig. 14.10. Imagine you are talking to

Consider Fig. 14.10. Imagine you are talking to a friend who has not taken any science courses, and explain how the figure demonstrates the concept of vapor pressure and enables it to be measured. Fr...

Q: Write a Lewis structure for each of the following polyatomic ions.

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit reson...

Q: Write a Lewis structure for each of the following polyatomic ions.

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit reson...

Q: Write a Lewis structure for each of the following polyatomic ions.

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit reson...

Q: Write a Lewis structure for each of the following polyatomic ions.

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit reson...

Q: A tank contains a mixture of 52.5 g of oxygen

A tank contains a mixture of 52.5 g of oxygen gas and 65.1 g of carbon dioxide gas at 27 °C. The total pressure in the tank is 9.21 atm. Calculate the partial pressure (in atm) of each gas in the mixt...

Q: What evidence do we have that the solid form of water is

What evidence do we have that the solid form of water is less dense than the liquid form of water at its freezing/melting point?

Q: What mass of neon gas would be required to fill a 3

What mass of neon gas would be required to fill a 3.00-L flask to a pressure of 925 mm Hg at 26 °C? What mass of argon gas would be required to fill a similar flask to the same pressure at the same te...

Q: Explain why the measured properties of a mixture of gases depend only

Explain why the measured properties of a mixture of gases depend only on the total number of moles of particles, not on the identity of the individual gas particles. How is this observation summarized...

Q: Determine the partial pressure of each gas as shown in this figure

Determine the partial pressure of each gas as shown in this figure. Note: The relative numbers of each type of gas are depicted in the figure.

Q: We often collect small samples of gases in the laboratory by bubbling

We often collect small samples of gases in the laboratory by bubbling the gas into a bottle or flask containing water. Explain why the gas becomes saturated with water vapor and how we must take the p...

Q: What general principles determine the molecular structure (shape) of a

What general principles determine the molecular structure (shape) of a molecule?

Q: If a gaseous mixture is made of 2.41 g of

If a gaseous mixture is made of 2.41 g of He and 2.79 g of Ne in an evacuated 1.04-L container at 25 °C, what will be the partial pressure of each gas and the total pressure in the container?

Q: Suppose that 1.28 g of neon gas and 2.

Suppose that 1.28 g of neon gas and 2.49 g of argon gas are confined in a 9.87-L container at 27 °C. What would be the pressure in the container?

Q: Although the valence electron pairs in ammonia have a tetrahedral arrangement,

Although the valence electron pairs in ammonia have a tetrahedral arrangement, the overall geometric structure of the ammonia molecule is not described as being tetrahedral. Explain.

Q: Small quantities of hydrogen gas can be prepared in the laboratory by

Small quantities of hydrogen gas can be prepared in the laboratory by the addition of aqueous hydrochloric acid to metallic zinc. Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g) Typically, the hyd...

Q: For the indicated atom in each of the following molecules or ions

For the indicated atom in each of the following molecules or ions, give the number and arrangement of the electron pairs around that atom. a. As in AsO43- b. Se in SeO42- c. S in H2S

Q: What does it mean to say that a bond is polar?

What does it mean to say that a bond is polar? Give two examples of molecules with polar bonds. Indicate in your examples the direction of the polarity.

Q: Consider the following molecules: CH3OH, CH4, H2O, C2H6

Consider the following molecules: CH3OH, CH4, H2O, C2H6. a. Draw the Lewis structure for each molecule, and indicate whether each is polar or nonpolar. b. At room temperature, two of these compounds...

Q: How is the phenomenon of temperature explained on the basis of the

How is the phenomenon of temperature explained on the basis of the kinetic molecular theory? What microscopic property of gas molecules is reflected in the temperature measured?

Q: Explain, in terms of the kinetic molecular theory, how an

Explain, in terms of the kinetic molecular theory, how an increase in the temperature of a gas confined to a rigid container causes an increase in the pressure of the gas.

Q: Which substance in each pair would be expected to have a lower

Which substance in each pair would be expected to have a lower boiling point? Explain your reasoning. a. CH3OH or CH3CH2CH2OH b. CH3CH3 or CH3CH2OH c. H2O or CH4

Q: Using the VSEPR theory, predict the molecular structure of each of

Using the VSEPR theory, predict the molecular structure of each of the following polyatomic ions. a. dihydrogen phosphate ion, H2PO4- b. perchlorate ion, ClO4- c. sulfite ion, SO32-

Q: Calcium oxide can be used to “scrub” carbon dioxide from

Calcium oxide can be used to “scrub” carbon dioxide from air. CaO(s) + CO2(g) CaCO3(s) What mass of CO2 could be absorbed by 1.25 g of CaO? What volume would this CO2 occupy at S...

Q: Which substance in each pair would be expected to be more volatile

Which substance in each pair would be expected to be more volatile at a particular temperature? Explain your reasoning. a. H2O(l) or H2S(l) b. H2O(l) or CH3OH(l) c. CH3OH(l) or CH3CH2OH(l)

Q: Consider the following reaction for the combustion of octane, C8H18:

Consider the following reaction for the combustion of octane, C8H18: 2C8H18(l) + 25O2(g) / 16CO2(g) + 18H20(l) What volume of oxygen gas at STP would be needed for the complete combustion of 10.0 g o...

Q: For each of the following molecules, predict both the molecular structure

For each of the following molecules, predict both the molecular structure and bond angles around the central atom. a. SeS2 b. SeS3 c. SO2 d. CS2

Q: Ammonia and gaseous hydrogen chloride combine to form ammonium chloride.

Ammonia and gaseous hydrogen chloride combine to form ammonium chloride. NH3(g) + HCl(g) NH4Cl(s) If 4.21 L of NH3(g) at 27 °C and 1.02 atm is combined with 5.35 L of HCl(g) at 26 °C...

Q: Explain the difference between intramolecular and intermolecular forces.

Explain the difference between intramolecular and intermolecular forces.

Q: Calcium carbide, CaC2, reacts with water to produce acetylene gas

Calcium carbide, CaC2, reacts with water to produce acetylene gas, C2H2. CaC2(s) + 2H2O(l) C2H2(g) + Ca(OH)2(s) What volume of acetylene at 25 °C and 1.01 atm is generated by th...

Q: Although we generally think of combustion reactions as involving oxygen gas,

Although we generally think of combustion reactions as involving oxygen gas, other rapid oxidation reactions are also referred to as combustions. For example, if magnesium metal is placed into chlorin...

Q: If water is added to magnesium nitride, ammonia gas is produced

If water is added to magnesium nitride, ammonia gas is produced when the mixture is heated. Mg3N2(s) + 3H2O(l) 3MgO(s) + 2NH3(g) If 10.3 g of magnesium nitride is trea...

Q: Two molecules that contain the same number of each kind of atom

Two molecules that contain the same number of each kind of atom but that have different molecular structures are said to be isomers of each other. For example, both ethyl alcohol and dimethyl ether (s...

Q: Consider the following unbalanced chemical equation in which element X is unknown

Consider the following unbalanced chemical equation in which element X is unknown: X(s) + F2(g) ( XF3(s) If 9.15 g of element X(s) is completely reacted with 4.00 L of fluorine gas at 250 °C and...

Q: A common prank on college campuses is to switch the salt and

A common prank on college campuses is to switch the salt and sugar on dining hall tables, which is usually easy because the substances look so much alike. Yet, despite the similarity in their appearan...

Q: The forces holding together a molecular solid are much (stronger/

The forces holding together a molecular solid are much (stronger/ weaker) than the forces between particles in an ionic solid.

Q: A mixture contains 5.00 g each of O2, N2

A mixture contains 5.00 g each of O2, N2, CO2, and Ne gas. Calculate the volume of this mixture at STP. Calculate the partial pressure of each gas in the mixture at STP.

Q: Dinitrogen monoxide, N2O, reacts with propane, C3H8, to

Dinitrogen monoxide, N2O, reacts with propane, C3H8, to form nitrogen, N2; carbon dioxide, CO2; and water, H2O. a. Write a balanced chemical equation for this reaction, treating all substances as gas...

Q: On the basis of the electronegativity values given in Fig. 12

On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs. a. N-P or N-O b. N-C or N-O c. N-S or N-C d. N-F or N-S

Q: In general terms, what is a chemical bond?

In general terms, what is a chemical bond?

Q: Describe in detail the microscopic processes that take place when a solid

Describe in detail the microscopic processes that take place when a solid melts and when a liquid boils. What kind of forces must be overcome? Are any chemical bonds broken during these processes?

Q: Explain the overall trend in the following melting points in terms of

Explain the overall trend in the following melting points in terms of the forces among particles in the solids indicated. Hydrogen, H2………………….-259 °C Ethyl alcohol, C2H5OH………-114 °C Water, H2O………………...

Q: During the making of steel, iron(II) oxide is

During the making of steel, iron(II) oxide is reduced to metallic iron by treatment with carbon monoxide gas. FeO(s) + CO(g) / Fe(s) + CO2(g) Suppose 1.45 kg of Fe reacts. What volume of CO(g) is req...

Q: What is a network solid? Give an example of a network

What is a network solid? Give an example of a network solid and describe the bonding in such a solid. How does a network solid differ from a molecular solid?

Q: What is an alloy? Explain the differences in structure between substitutional

What is an alloy? Explain the differences in structure between substitutional and interstitial alloys. Give an example of each type.

Q: On the basis of their electron configurations, predict the formula of

On the basis of their electron configurations, predict the formula of the simple binary ionic compound likely to form when the following pairs of elements react with each other. a. sodium, Na, and se...

Q: Which of the following statements is(are) true?

Which of the following statements is(are) true? a. At constant temperature, the lighter the gas molecules, the faster the average velocity of the gas molecules. b. At constant temperature, the heavi...

Q: Consider the flasks in the following diagrams. /

Consider the flasks in the following diagrams. Assuming the connecting tube has negligible volume, draw what each diagram will look like after the stopcock between the two flasks is opened. Also, so...

Q: When a person has a severe fever, one therapy to reduce

When a person has a severe fever, one therapy to reduce the fever is an “alcohol rub.” Explain how the evaporation of alcohol from the person’s skin removes heat energy from the body.

Q: What is the total number of valence electrons in each of the

What is the total number of valence electrons in each of the following molecules? a. HNO3 b. H2SO4 c. H3PO4 d. HClO4

Q: Write a Lewis structure for each of the following simple molecules.

Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. a. GeH4 b. ICl c. NI3 d. PF3...

Q: In each of the following groups, which element is the most

In each of the following groups, which element is the most electronegative? Which is the least electro negative? a. K, Na, H b. F, Br, Na c. B, N, F

Q: When ammonium carbonate is heated, three gases are produced by its

When ammonium carbonate is heated, three gases are produced by its decomposition. (NH4)2CO3(s) 2NH3(g) + CO2(g) + H2O(g) What total volume of gas is produced, measured at 45...

Q: A helium tank contains 25.2 L of helium at 8

A helium tank contains 25.2 L of helium at 8.40 atm pressure. Determine how many 1.50-L balloons at 755 mm Hg can be inflated with the gas in the tank, assuming that the tank will also have to contain...

Q: Carbon dioxide gas, saturated with water vapor, can be produced

Carbon dioxide gas, saturated with water vapor, can be produced by the addition of aqueous acid to calcium carbonate. CaCO3(s) + 2H+(aq) / Ca2+(aq) + H2O(l) + CO2(g) How many moles of CO2(g), collect...

Q: Why is the molecular structure of H2O nonlinear, whereas that of

Why is the molecular structure of H2O nonlinear, whereas that of BeF2 is linear, even though both molecules consist of three atoms?

Q: As weather balloons rise from the earth’s surface, the pressure of

As weather balloons rise from the earth’s surface, the pressure of the atmosphere becomes less, tending to cause the volume of the balloons to expand. However, the temperature is much lower in the upp...

Q: What are some important uses of water, both in nature and

What are some important uses of water, both in nature and in industry? What is the liquid range for water?

Q: Describe, on both a microscopic and a macroscopic basis, what

Describe, on both a microscopic and a macroscopic basis, what happens to a sample of water as it is cooled from room temperature to 50 °C below its normal freezing point.

Q: Cake mixes and other packaged foods that require cooking often contain special

Cake mixes and other packaged foods that require cooking often contain special directions for use at high elevations. Typically these directions indicate that the food should be cooked longer above 50...

Q: A 2.50-L container at 1.00 atm

A 2.50-L container at 1.00 atm and 248°C is filled with 5.41 g of a monatomic gas. a. Determine the identity of the gas. b. Assuming the 2.50-L container is a large elastic balloon, predict what wil...

Q: For each of the following sets of pressure/volume data,

For each of the following sets of pressure/volume data, calculate the missing quantity. Assume that the temperature and the amount of gas remain constant. a. V = 123 L at 4.56 atm; V =? at 1002 mm Hg...

Q: Convert the following pressures into pascals. a. 774 torr

Convert the following pressures into pascals. a. 774 torr b. 0.965 atm c. 112.5 kPa d. 801 mm Hg

Q: What do we call the energies required, respectively, to melt

What do we call the energies required, respectively, to melt and to vaporize 1 mole of a substance? Which of these energies is always larger for a given substance? Why?

Q: Consider the following series of atoms or ions: S2-, S

Consider the following series of atoms or ions: S2-, S, S2+, Cs+, Sr2+. a. Which of the species has the smallest size? b. Which of the species has the largest ionization energy?

Q: A particular balloon is designed by its manufacturer to be inflated to

A particular balloon is designed by its manufacturer to be inflated to a volume of no more than 2.5 L. If the balloon is filled with 2.0 L of helium at sea level, is released, and rises to an altitude...

Q: What are London dispersion forces and how do they arise in a

What are London dispersion forces and how do they arise in a nonpolar molecule? Are London forces typically stronger or weaker than dipole–dipole attractions between polar molecules? Are London forces...

Q: Describe in detail the microscopic processes that take place when a liquid

Describe in detail the microscopic processes that take place when a liquid boils. What kind of forces must be overcome? Are any chemical bonds broken during these processes?

Q: Arrange the atoms and/or ions in the following groups in

Arrange the atoms and/or ions in the following groups in order of decreasing size. a. O, O+, O2- b. Fe2+, Ni2+, Zn2+ c. Ca2+, K+, Cl-

Q: For each of the following sets of volume/temperature data,

For each of the following sets of volume/temperature data, calculate the missing quantity. Assume that the pressure and the amount of gas remain constant. a. V = 22.4 L at 0 °C; V = 44.4 L at? K b....

Q: Although the noble gas elements are monatomic and could not give rise

Although the noble gas elements are monatomic and could not give rise to dipole–dipole forces or hydrogen bonding, these elements still can be liquefied and solidified. Explain.

Q: You have a gas in a container fitted with a piston,

You have a gas in a container fitted with a piston, and you change one of the conditions of the gas such that a change takes place, as shown below: State three distinct changes you can make to accom...

Q: Given each of the following sets of values for three of the

Given each of the following sets of values for three of the gas variables, calculate the unknown quantity. a. P = 21.2 atm; V = 142 mL; n = 0.432 mol; T =? K b. P =? atm; V = 1.23 mL; n = 0.000115 m...

Q: Make the indicated pressure conversions. a. 1.54

Make the indicated pressure conversions. a. 1.54 * 105 Pa to atmospheres b. 1.21 atm to pascals c. 97,345 Pa to mm Hg d. 1.32 kPa to pascals

Q: Given each of the following sets of values for three of the

Given each of the following sets of values for three of the gas variables, calculate the unknown quantity. a. P = 1.034 atm; V = 21.2 mL; n = 0.00432 mol; T =? K b. P =? atm; V = 1.73 mL; n = 0.0001...

Q: Describe, on a microscopic basis, the processes of evaporation and

Describe, on a microscopic basis, the processes of evaporation and condensation. Which process requires an input of energy? Why?

Q: Which of the following statements about intermolecular forces is(are)

Which of the following statements about intermolecular forces is(are) true? a. London dispersion forces are the only type of intermolecular force that nonpolar molecules exhibit. b. Molecules that ha...

Q: Which of the following statements is(are) true?

Which of the following statements is(are) true? a. LiF will have a higher vapor pressure at 25 °C than H2S. b. HF will have a lower vapor pressure at 250 °C than HBr. c. Cl2 will have a higher boil...

Q: A 22-g sample of neon gas exerts a pressure of

A 22-g sample of neon gas exerts a pressure of 2.0 atm at a certain temperature and volume. What pressure does a 44-g sample of argon gas exert at these conditions of temperature and volume?

Q: If 3.20 g of nitrogen gas occupies a volume of

If 3.20 g of nitrogen gas occupies a volume of 1.71 L at 0 °C and a pressure of 1.50 atm, what would the volume become if 8.80 g of nitrogen gas were added at constant conditions of temperature and pr...

Q: An aluminum can contain a small amount of water and is boiled

An aluminum can contain a small amount of water and is boiled with the lid removed. The heat is then turned off, and the can is sealed. Over time, the can crumples. a. Why doesn’...

Q: A mixture at 33 °C contains H2 at 325 torr,

A mixture at 33 °C contains H2 at 325 torr, N2 at 475 torr, and O2 at 650. torr. a. What is the total pressure of the gases in the system? b. Which gas contains the greatest number of moles?

Q: You have two rigid gas cylinders. Gas cylinder A has a

You have two rigid gas cylinders. Gas cylinder A has a volume of 48.2 L and contains N2(g) at 8.35 atm at 25 °C. Gas cylinder B has a volume of 22.0 L and contains He(g) at 25 °C. When the two cylinde...

Q: Consider the following chemical equation: N2(g) +

Consider the following chemical equation: N2(g) + 3H2(g) 2NH3(g) What volumes of nitrogen gas and hydrogen gas, each measured at 11 °C and 0.998 atm, are needed to produce 5.00...

Q: Discuss the similarities and differences between the arrangements of molecules and the

Discuss the similarities and differences between the arrangements of molecules and the forces between molecules in liquid water versus steam, and in liquid water versus ice.

Q: The following demonstration takes place in a two-step process:

The following demonstration takes place in a two-step process: First, solid calcium carbide (CaC2) reacts with liquid water to produce acetylene gas (C2H2) and aqueous calcium hydroxide. Second, the a...

Q: Consider the following unbalanced chemical equation: Cu2S(s)

Consider the following unbalanced chemical equation: Cu2S(s) + O2(g) Cu2O(s) + SO2(g) What volume of oxygen gas, measured at 27.5 °C and 0.998 atm, is required to react with...

Q: When sodium bicarbonate, NaHCO3(s), is heated, sodium

When sodium bicarbonate, NaHCO3(s), is heated, sodium carbonate is produced, with the evolution of water vapor and carbon dioxide gas. 2NaHCO3(s) / Na2CO3(s) + H2O(g) + CO2(g) What total volume of ga...

Q: What volume does 35 moles of N2 occupy at STP?

What volume does 35 moles of N2 occupy at STP?

Q: A sample of oxygen gas has a volume of 125 L at

A sample of oxygen gas has a volume of 125 L at 25 °C and a pressure of 0.987 atm. Calculate the volume of this oxygen sample at STP.

Q: Consider the flasks in the following diagrams. /

Consider the flasks in the following diagrams. a. Which is greater, the initial pressure of helium or the initial pressure of neon? How much greater? b. Assuming the connecting tube has negligible...

Q: What volume of CO2 measured at STP is produced when 27.

What volume of CO2 measured at STP is produced when 27.5 g of CaCO3 is decomposed? CaCO3(s) / CaO(s) + CO2(g)

Q: Concentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal

Concentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal ions (such as Mn or Fe): 2H2O2(aq) 2H2O(l) + O2(g) What volume of pure O2(g)...

Q: The “Chemistry in Focus” segment The Chemistry of Air Bags

The “Chemistry in Focus” segment The Chemistry of Air Bags discusses how the decomposition of sodium azide inflates the air bag. Use the balanced chemical equation in the segment to determine the mass...

Q: The “Chemistry in Focus” segment Breath Fingerprinting discusses using breath

The “Chemistry in Focus” segment Breath Fingerprinting discusses using breath analysis to diagnose diseases. The volume of the average human breath is approximately 500 mL, and carbon dioxide (CO2) ma...

Q: Which of the following molecules contain polar covalent bonds? a

Which of the following molecules contain polar covalent bonds? a. water, H2O b. carbon monoxide, CO c. fluorine, F2 d. nitrogen, N2

Q: Complete the following table for an ideal gas. /

Complete the following table for an ideal gas.

Q: A glass vessel contains 28 g of nitrogen gas. Assuming ideal

A glass vessel contains 28 g of nitrogen gas. Assuming ideal behavior, which of the processes listed below would double the pressure exerted on the walls of the vessel? a. Adding 28 g of oxygen gas...

Q: A steel cylinder contains 150.0 moles of argon gas at

A steel cylinder contains 150.0 moles of argon gas at a temperature of 25 °C and a pressure of 8.93 MPa. After some argon has been used, the pressure is 2.00 MPa at a temperature of 19 °C. What mass o...

Q: A certain flexible weather balloon contains helium gas at a volume of

A certain flexible weather balloon contains helium gas at a volume of 855 L. Initially, the balloon is at sea level where the temperature is 25 °C and the barometric pressure is 730 torr. The balloon...

Q: A large flask with a volume of 936 mL is evacuated and

A large flask with a volume of 936 mL is evacuated and found to have a mass of 134.66 g. It is then filled to a pressure of 0.967 atm at 31 °C with a gas of unknown molar mass and then reweighed to gi...

Q: A 20.0-L nickel container was charged with 0

A 20.0-L nickel container was charged with 0.859 atm of xenon gas and 1.37 atm of fluorine gas at 400 °C. The xenon and fluorine react to form xenon tetrafluoride. What mass of xenon tetrafluoride can...

Q: Consider the unbalanced chemical equation: CaSiO3(s) +

Consider the unbalanced chemical equation: CaSiO3(s) + HF(g) / CaF2(aq) + SiF4(g) + H2O(l) Suppose a 32.9-g sample of CaSiO3 is reacted with 31.8 L of HF at 27.0 °C and 1.00 atm. Assuming the reactio...

Q: Which of the following statements is(are) true?

Which of the following statements is(are) true? a. If the number of moles of a gas is doubled, the volume will double, assuming the pressure and temperature of the gas remain constant. b. If the tempe...

Q: Determine the pressure in a 125-L tank containing 56.

Determine the pressure in a 125-L tank containing 56.2 kg of oxygen gas at 21 °C.

Q: What volume will 2.04 g of helium gas occupy at

What volume will 2.04 g of helium gas occupy at 100. °C and 785 mm Hg pressure?

Q: Which of the following molecules contain polar covalent bonds? a

Which of the following molecules contain polar covalent bonds? a. phosphorus, P4 b. oxygen, O2 c. ozone, O3 d. hydrogen fluoride, HF

Q: At what temperature (in °C) will a 5.

At what temperature (in °C) will a 5.00-g sample of neon gas exert a pressure of 1.10 atm in a 7.00-L container?

Q: Suppose that a 1.25-g sample of neon gas

Suppose that a 1.25-g sample of neon gas is confined in a 10.1-L container at 25 °C. What will be the pressure in the container? Suppose the temperature is then raised to 50 °C. What will the new pres...

Q: Suppose that 1.29 g of argon gas is confined to

Suppose that 1.29 g of argon gas is confined to a volume of 2.41 L at 29 °C. What would be the pressure in the container? What would the pressure become if the temperature were raised to 42 °C without...

Q: What will the volume of the sample become if 459 mL of

What will the volume of the sample become if 459 mL of an ideal gas at 27 °C and 1.05 atm is cooled to 15 °C and 0.997 atm?

Q: The “Chemistry in Focus” segment Snacks Need Chemistry, Too

The “Chemistry in Focus” segment Snacks Need Chemistry, Too! discusses why popcorn “pops.” You can estimate the pressure inside a kernel of popcorn at the time of popping by using the ideal gas law. B...

Q: Make the indicated pressure conversions. a. 45.2

Make the indicated pressure conversions. a. 45.2 kPa to atmospheres b. 755 mm Hg to atmospheres c. 802 torr to kilopascals d. 1.04 atm to millimeters of mercury

Q: A sample of oxygen gas is saturated with water vapor at 27

A sample of oxygen gas is saturated with water vapor at 27 °C. The total pressure of the mixture is 772 torr, and the vapor pressure of water is 26.7 torr at 27 °C. What is the partial pressure of the...

Q: A 500.-mL sample of O2 gas at 24 °C

A 500.-mL sample of O2 gas at 24 °C was prepared by decomposing a 3% aqueous solution of hydrogen peroxide, H2O2, in the presence of a small amount of manganese catalyst by the reaction 2H2O2 (aq)...

Q: What is a scientific law? What is a theory? How

What is a scientific law? What is a theory? How do these concepts differ? Does a law explain a theory, or does a theory attempt to explain a law?

Q: When is a scientific theory considered to be successful? Are all

When is a scientific theory considered to be successful? Are all theories successful? Will a theory that has been successful in the past necessarily be successful in the future?

Q: On the basis of the electronegativity values given in Fig. 12

On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs. a. H-F or H-Cl b. H-Cl or H-I c. H-Br or H-Cl d. H-I or H-Br...

Q: Collisions of the molecules in a sample of gas with the walls

Collisions of the molecules in a sample of gas with the walls of the container are responsible for the gas’s observed .

Q: The kinetic molecular theory of gases suggests that gas particles exert attractive

The kinetic molecular theory of gases suggests that gas particles exert attractive or repulsive forces on each other.

Q: What is the molar volume of a gas? Do all gases

What is the molar volume of a gas? Do all gases that behave ideally have the same molar volume?

Q: Consider the following reaction: C(s) + O2

Consider the following reaction: C(s) + O2(g) CO2(g) What volume of oxygen gas at 25 °C and 1.02 atm would be required to react completely with 1.25 g of carbon?

Q: Make the indicated pressure conversions. a. 699 mm Hg

Make the indicated pressure conversions. a. 699 mm Hg to atmospheres b. 18.2 psi to mm Hg c. 862 mm Hg to torr d. 795 mm Hg to psi

Q: Many transition metal salts are hydrates: they contain a fixed number

Many transition metal salts are hydrates: they contain a fixed number of water molecules bound per formula unit of the salt. For example, copper(II) sulfate most commonly exists as the pentahydrate, C...

Q: What volume does a mixture of 14.2 g of He

What volume does a mixture of 14.2 g of He and 21.6 g of H2 occupy at 28 °C and 0.985 atm?

Q: A sample of helium gas occupies a volume of 25.2

A sample of helium gas occupies a volume of 25.2 mL at 95 °C and a pressure of 892 mm Hg. Calculate the volume of the gas at STP.

Q: Consider the following chemical equation: N2(g) +

Consider the following chemical equation: N2(g) + 3H2(g) ( 2NH3(g) What minimum total volume of reactant gases is needed to produce 4.00 g of ammonia if the volume of each gas is measured at 11 °C an...

Q: Gases have (higher/lower) densities than liquids or solids

Gases have (higher/lower) densities than liquids or solids.

Q: On the basis of the electronegativity values given in Fig. 12

On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs. a. O-Cl or O-Br b. N-O or N-F c. P-S or P-O d. H-O or H-N Fr...

Q: The forces that connect two hydrogen atoms to an oxygen atom in

The forces that connect two hydrogen atoms to an oxygen atom in a water molecule are (intermo lecular/intramolecular), but the forces that hold water molecules close together in an ice cube are (inter...

Q: The energy required to melt 1 mole of a solid is called

The energy required to melt 1 mole of a solid is called the .

Q: The following data have been collected for substance X. Construct a

The following data have been collected for substance X. Construct a heating curve for substance X. (The drawing does not need to be absolutely to scale, but it should clearly show relative differences...

Q: The molar heat of fusion of aluminum metal is 10.79

The molar heat of fusion of aluminum metal is 10.79 kJ/mol, whereas its heat of vaporization is 293.4 kJ/mol. a. Why is the heat of fusion of aluminum so much smaller than the heat of vaporization?...

Q: The molar heats of fusion and vaporization for silver are 11.

The molar heats of fusion and vaporization for silver are 11.3 kJ/mol and 250. kJ/mol, respectively. Silver’s normal melting point is 962 °C, and its normal boiling point is 2212 °C. What quantity of...

Q: It requires 113 J to melt 1.00 g of sodium

It requires 113 J to melt 1.00 g of sodium metal at its normal melting point of 98 °C. Calculate the molar heat of fusion of sodium.

Q: Consider the iodine monochloride molecule, ICl. Because chlorine is more

Consider the iodine monochloride molecule, ICl. Because chlorine is more electronegative than iodine, this molecule is a dipole. How would you expect iodine monochloride molecules in the gaseous state...

Q: Liquids and solids are (more/less) compressible than are

Liquids and solids are (more/less) compressible than are gases.

Q: Dipole–dipole forces become as the distance between the dipoles decreases

Dipole–dipole forces become as the distance between the dipoles decreases (gets closer together).

Q: The text implies that hydrogen bonding is a special case of very

The text implies that hydrogen bonding is a special case of very strong dipole–dipole interactions possible among only certain atoms. What atoms in addition to hydrogen are necessary for hydrogen bond...

Q: Which bond in each of the following pairs has the greater ionic

Which bond in each of the following pairs has the greater ionic character? a. Na-F or Na-I b. Ca-S or Ca-O c. Li-Cl or Cs-Cl d. Mg-N or Mg-P

Q: are relatively weak forces that exist among noble gas atoms and

are relatively weak forces that exist among noble gas atoms and nonpolar molecules that involve an accidental dipole that induces a momentary dipole in a neighbor.

Q: What type of intermolecular forces is active in the liquid state of

What type of intermolecular forces is active in the liquid state of each of the following substances? a. Ne b. CO c. CH3OH d. Cl2

Q: Discuss the types of intermolecular forces acting in the liquid state of

Discuss the types of intermolecular forces acting in the liquid state of each of the following substances. a. Xe b. NH3 c. F2 d. ICl

Q: The heats of fusion of three substances are listed below. Explain

The heats of fusion of three substances are listed below. Explain the trend this list reflects. HI…………………2.87 kJ/mol HBr………………2.41 kJ/mol HCl………………1.99 kJ/mol

Q: What is evaporation? What is condensation? Which of these processes

What is evaporation? What is condensation? Which of these processes is endothermic and which is exothermic?

Q: Although water and ammonia differ in molar mass by only one unit

Although water and ammonia differ in molar mass by only one unit, the boiling point of water is over 100 °C higher than that of ammonia. What forces in liquid water that do not exist in liquid ammonia...

Q: What are crystalline solids? What kind of microscopic structure do such

What are crystalline solids? What kind of microscopic structure do such solids have? How is this microscopic structure reflected in the macroscopic appearance of such solids?

Q: The enthalpy (∆H) of vaporization of water is about seven

The enthalpy (∆H) of vaporization of water is about seven times larger than water’s enthalpy of fusion (41 kJ/mol vs. 6 kJ/mol). What does this tell us about the relative similarities among the solid,...

Q: What types of forces exist between the individual particles in an ionic

What types of forces exist between the individual particles in an ionic solid? Are these forces relatively strong or relatively weak?

Q: Ionic solids do not conduct electricity in the solid state, but

Ionic solids do not conduct electricity in the solid state, but are strong conductors in the liquid state and when dissolved in water. Explain.

Q: How are the three states of matter similar, and how do

How are the three states of matter similar, and how do they differ?

Q: For each of the following sets of pressure/volume data,

For each of the following sets of pressure/volume data, calculate the missing quantity. Assume that the temperature and the amount of gas remain constant. a. V = 53.2 mL at 785 mm Hg; V = ? mL at 700...

Q: The “Chemistry in Focus” segment Metal with a Memory discusses

The “Chemistry in Focus” segment Metal with a Memory discusses Nitinol, an alloy that “remembers” a shape originally impressed in it. Which elements comprise Nitinol, and why is it classified as an al...

Q: For Exercises 51–60 choose one of the following terms to

For Exercises 51–60 choose one of the following terms to match the definition or description given. a. alloy b. specific heat c. crystalline solid d. dipole–dipole attraction e. equilibrium vapor...

Q: For Exercises 51–60 choose one of the following terms to

For Exercises 51–60 choose one of the following terms to match the definition or description given. a. alloy b. specific heat c. crystalline solid d. dipole–dipole attraction e. equilibrium vapor...

Q: For Exercises 51–60 choose one of the following terms to

For Exercises 51–60 choose one of the following terms to match the definition or description given. a. alloy b. specific heat c. crystalline solid d. dipole–dipole attraction e. equilibrium vapor...

Q: For Exercises 51–60 choose one of the following terms to

For Exercises 51–60 choose one of the following terms to match the definition or description given. a. alloy b. specific heat c. crystalline solid d. dipole–dipole attraction e. equilibrium vapor...

Q: For Exercises 51–60 choose one of the following terms to

For Exercises 51–60 choose one of the following terms to match the definition or description given. a. alloy b. specific heat c. crystalline solid d. dipole–dipole attraction e. equilibrium vapor...

Q: For Exercises 51–60 choose one of the following terms to

For Exercises 51–60 choose one of the following terms to match the definition or description given. a. alloy b. specific heat c. crystalline solid d. dipole–dipole attraction e. equilibrium vapor...

Q: For Exercises 51–60 choose one of the following terms to

For Exercises 51–60 choose one of the following terms to match the definition or description given. a. alloy b. specific heat c. crystalline solid d. dipole–dipole attraction e. equilibrium vapor...

Q: For Exercises 51–60 choose one of the following terms to

For Exercises 51–60 choose one of the following terms to match the definition or description given. a. alloy b. specific heat c. crystalline solid d. dipole–dipole attraction e. equilibrium vapor...

Q: For Exercises 51–60 choose one of the following terms to

For Exercises 51–60 choose one of the following terms to match the definition or description given. a. alloy b. specific heat c. crystalline solid d. dipole–dipole attraction e. equilibrium vapor...

Q: What is a dipole moment? Give four examples of molecules that

What is a dipole moment? Give four examples of molecules that possess dipole moments, and draw the direction of the dipole as shown in Section 12.3.

Q: Sketch a heating/cooling curve for water, starting out at

Sketch a heating/cooling curve for water, starting out at -20 °C and going up to 120 °C, applying heat to the sample at a constant rate. Mark on your sketch the portions of the curve that represent th...

Q: For Exercises 51–60 choose one of the following terms to

For Exercises 51–60 choose one of the following terms to match the definition or description given. a. alloy b. specific heat c. crystalline solid d. dipole–dipole attraction e. equilibrium vapor...

Q: Given the densities and conditions of ice, liquid water, and

Given the densities and conditions of ice, liquid water, and steam listed in Table 14.1, calculate the volume of 1.0 g of water under each of these circumstances. From table 14.1

Q: Which of the substances in each of the following sets would be

Which of the substances in each of the following sets would be expected to have the highest boiling point? Explain why. a. Ga, KBr, O2 b. Hg, NaCl, He c. H2, O2, H2O

Q: What are some physical properties that historically led chemists to classify various

What are some physical properties that historically led chemists to classify various substances as acids and bases?

Q: How do chemists recognize a system that has reached a state of

How do chemists recognize a system that has reached a state of chemical equilibrium? When writing chemical equations, how do we indicate reactions that come to a state of chemical equilibrium?

Q: For each hydrogen or hydroxide ion concentration listed, calculate the concentration

For each hydrogen or hydroxide ion concentration listed, calculate the concentration of the complementary ion and the pH and pOH of the solution. a. [H+] = 5.72 * 10-4 M b. [OH-] = 8.91 * 10-5 M c....

Q: Calculate [OH-] in each of the following solutions, and

Calculate [OH-] in each of the following solutions, and indicate whether the solution is acidic, basic, or neutral. a. [H+] = 4.21 * 10-7 M b. [H+] = 0.00035 M c. [H+] = 0.00000010 M d. [H+] = 9.9...

Q: You mix 225.0 mL of a 2.5 M

You mix 225.0 mL of a 2.5 M HCl solution with 150.0 mL of a 0.75 M HCl solution. What is the molarity of the final solution?

Q: Calculate the hydrogen ion concentration, in moles per liter, for

Calculate the hydrogen ion concentration, in moles per liter, for solutions with each of the following pH or pOH values. a. pOH = 0.90 b. pH = 0.90 c. pOH = 10.3 d. pH = 5.33

Q: Calculate the hydrogen ion concentration and the pH of each of the

Calculate the hydrogen ion concentration and the pH of each of the following solutions of strong acids. a. 1.4 * 10-3 M HClO4 b. 3.0 * 10-5 M HCl c. 5.0 * 10-2 M HNO3 d. 0.0010 M HCl

Q: A 15.0% (by mass) NaCl solution is

A 15.0% (by mass) NaCl solution is available. Determine what mass of the solution should be taken to obtain the following quantities of NaCl. a. 10.0 g b. 25.0 g c. 100.0 g d. 1.00 lb

Q: Calculate the hydrogen ion concentration, in moles per liter, for

Calculate the hydrogen ion concentration, in moles per liter, for solutions with each of the following pH or pOH values. a. pH = 5.41 b. pOH = 12.04 c. pH = 11.91 d. pOH = 3.89

Q: Write the formulas for three combinations of weak acid and salt that

Write the formulas for three combinations of weak acid and salt that would act as buffered solutions. For each of your combinations, write chemical equations showing how the components of the buffered...

Q: Consider 0.25 M solutions of the following salts: NaCl

Consider 0.25 M solutions of the following salts: NaCl, RbOCl, KI, Ba(ClO4)2, and NH4NO3. For each salt, indicate whether the solution is acidic, basic, or neutral.

Q: The three common silver halides (AgCl, AgBr, and AgI

The three common silver halides (AgCl, AgBr, and AgI) are all sparingly soluble salts. Given the values for Ksp for these salts below, calculate the concentration of silver ion, in mol/L, in a saturat...

Q: What does it mean to say that a state of chemical or

What does it mean to say that a state of chemical or physical equilibrium is dynamic?

Q: Approximately 1.5 * 10-3 g of iron(

Approximately 1.5 * 10-3 g of iron(II) hydroxide, Fe(OH)2(s), dissolves per liter of water at 18 °C. Calculate Ksp for Fe(OH)2(s) at this temperature.

Q: Chromium(III) hydroxide dissolves in water only to the extent

Chromium(III) hydroxide dissolves in water only to the extent of 8.21 * 10-5 M at 25 °C. Calculate Ksp for Cr(OH)3 at this temperature.

Q: Approximately 0.14 g of nickel(II) hydroxide,

Approximately 0.14 g of nickel(II) hydroxide, Ni(OH)2(s), dissolves per liter of water at 20 °C. Calculate Ksp for Ni(OH)2(s) at this temperature.

Q: For each of the following solutions, the mass of the solute

For each of the following solutions, the mass of the solute is given, followed by the total volume of solution prepared. Calculate the molarity. a. 5.0 g of BaCl2; 2.5 L b. 3.5 g of KBr; 75 mL c. 2...

Q: You are given 1.00 gram of each of five substances

You are given 1.00 gram of each of five substances. In which of the substances will there be the greatest number of potassium ions when dissolved in water? a. potassium chloride b. potassium chlorat...

Q: Magnesium fluoride dissolves in water to the extent of 8.0

Magnesium fluoride dissolves in water to the extent of 8.0 * 10-2 g/L at 25 °C. Calculate the solubility of MgF2(s) in moles per liter, and calculate Ksp for MgF2 at 25 °C.

Q: When 200.0 mL of 0.10 M Zn(

When 200.0 mL of 0.10 M Zn(NO3)2 is mixed with 100.0 mL of 0.10 M KOH, a precipitate forms. a. How many moles of precipitate can form in this reaction? b. Calculate the concentration of Zn2+ ions in...

Q: Lead(II) chloride, PbCl2(s), dissolves in

Lead(II) chloride, PbCl2(s), dissolves in water to the extent of approximately 3.6 * 10-2 M at 20 °C. Calculate Ksp for PbCl2(s), and calculate its solubility in grams per liter.

Q: How many moles and how many grams of the indicated solute does

How many moles and how many grams of the indicated solute does each of the following solutions contain? a. 4.25 L of 0.105 M KCl solution b. 15.1 mL of 0.225 M NaNO3 solution c. 25 mL of 3.0 M HCl...

Q: Suppose a reaction has the equilibrium constant K = 4.5

Suppose a reaction has the equilibrium constant K = 4.5 * 10-6 at a particular temperature. If an experiment is set up with this reaction, will there be large relative concentrations of products prese...

Q: Consider an initial mixture of N2 and H2 gases that can be

Consider an initial mixture of N2 and H2 gases that can be represented as follows: The gases react to form ammonia gas (NH3) as represented by the following concentration profile: a. Label each plot...

Q: Calculate the number of moles of each ion present in each of

Calculate the number of moles of each ion present in each of the following solutions. a. 1.25 L of 0.250 M Na3PO4 solution b. 3.5 mL of 6.0 M H2SO4 solution c. 25 mL of 0.15 M AlCl3 solution d. 1....

Q: Mercury(I) chloride, Hg2Cl2, was formerly administered orally

Mercury(I) chloride, Hg2Cl2, was formerly administered orally as a purgative. Although we usually think of mercury compounds as highly toxic, the Ksp of mercury(I) chloride is small enough (1.3 * 10-1...

Q: Calculate the new molarity when 150. mL of water is added

Calculate the new molarity when 150. mL of water is added to each of the following solutions. a. 125 mL of 0.200 M HBr b. 155 mL of 0.250 M Ca(C2H3O2)2 c. 0.500 L of 0.250 M H3PO4 d. 15 mL of 18.0...

Q: The solubility product of iron(III) hydroxide is very small

The solubility product of iron(III) hydroxide is very small: Ksp = 4 * 10-38 at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH...

Q: Consider the reaction between 1.0 L of 3.0

Consider the reaction between 1.0 L of 3.0 M AgNO3(aq) and 1.0 L of 1.0 M CuCl2(aq), according to the equation: 2AgNO3(aq) + CuCl2(aq) ( 2AgCl(s) + Cu(NO3)2(aq) Which of the following will increase t...

Q: Consider the following reaction at some temperature: H2O( g

Consider the following reaction at some temperature: H2O( g) + CO( g) ⇌ H2( g) + CO2( g) K = 2.0 Some molecules of H2O and CO are placed in a 1.0-L container as shown b...

Q: An aqueous solution of ammonium sulfide is mixed with an aqueous solution

An aqueous solution of ammonium sulfide is mixed with an aqueous solution of iron(III) chloride. a. Write a balanced molecular equation, complete ionic equation, and net ionic equation for the two so...

Q: For a given reaction at a given temperature, the special ratio

For a given reaction at a given temperature, the special ratio of products to reactants defined by the equilibrium constant is always equal to the same number. Explain why this is true, no matter what...

Q: Suppose K = 4.5 * 10-3 at a

Suppose K = 4.5 * 10-3 at a certain temperature for the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g) If it is found that the concentration of PCl5 is twice the concentration of PCl3, what must be the concentr...

Q: What volume of 0.250 M HCl is required to neutralize

What volume of 0.250 M HCl is required to neutralize each of the following solutions? a. 25.0 mL of 0.103 M sodium hydroxide, NaOH b. 50.0 mL of 0.00501 M calcium hydroxide, Ca(OH)2 c. 20.0 mL of 0...

Q: In general terms, what does the equilibrium constant for a reaction

In general terms, what does the equilibrium constant for a reaction represent? What is the algebraic form of the equilibrium constant for a typical reaction? What do square brackets indicate when we w...

Q: For each of the following solutions, the mass of solute taken

For each of the following solutions, the mass of solute taken is indicated, as well as the total volume of solution prepared. Calculate the normality of each solution. a. 15.0 g of HCl; 500. mL b. 4...

Q: As you know from Chapter 7, most metal carbonate salts are

As you know from Chapter 7, most metal carbonate salts are sparingly soluble in water. Below are listed several metal carbonates along with their solubility products, Ksp. For each salt, write the equ...

Q: Teeth and bones are composed, to a first approximation, of

Teeth and bones are composed, to a first approximation, of calcium phosphate, Ca3(PO4)2(s). The Ksp for this salt is 1.3 * 10-32 at 25 °C. Calculate the concentration of calcium ion in a saturated sol...

Q: How many milliliters of 0.105 M NaOH are required to

How many milliliters of 0.105 M NaOH are required to neutralize exactly 14.2 mL of 0.141 M H3PO4?

Q: Explain why the development of a vapor pressure above a liquid in

Explain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state...

Q: You mix 100.0 mL of 0.100 M calcium

You mix 100.0 mL of 0.100 M calcium chloride with 100.0 mL of 0.100 M silver nitrate. What species are in solution when the reaction is complete? a. calcium ion, chloride ion, nitrate ion, water b....

Q: Consider the reaction between 0.156 L of 0.105

Consider the reaction between 0.156 L of 0.105 M magnesium nitrate and 0.166 L of 0.106 M potassium hydroxide. a. What mass of precipitate will form? b. What is the concentration of nitrate ions lef...

Q: Consider the following generic reaction: 2A2B( g) ⇌

Consider the following generic reaction: 2A2B( g) ⇌ 2A2( g) + B2( g) Some molecules of A2B are placed in a 1.0-L container. As time passes, several snapshots of the reaction mixture...

Q: A solution is prepared by dissolving 0.6706 g of oxalic

A solution is prepared by dissolving 0.6706 g of oxalic acid (H2C2O4) in enough water to make 100.0 mL of solution. A 10.00-mL aliquot (portion) of this solution is then diluted to a final volume of 2...

Q: What volume of 0.100 M NaOH is required to precipitate

What volume of 0.100 M NaOH is required to precipitate all of the nickel(II) ions from 150.0 mL of a 0.249 M solution of Ni(NO3)2?

Q: There is only one value of the equilibrium constant for a particular

There is only one value of the equilibrium constant for a particular system at a particular temperature, but there are an infinite number of equilibrium positions. Explain.

Q: A 500.0-mL sample of 0.200 M

A 500.0-mL sample of 0.200 M sodium phosphate is mixed with 400.0 mL of 0.289 M barium chloride. What is the mass of the solid produced?

Q: A 450.0-mL sample of a 0.257

A 450.0-mL sample of a 0.257 M solution of silver nitrate is mixed with 400.0 mL of 0.200 M calcium chloride. What is the concentration of Cl- in solution after the reaction is complete?

Q: A 50.00-mL sample of aqueous Ca(OH

A 50.00-mL sample of aqueous Ca(OH)2 requires 34.66 mL of a 0.944 M nitric acid for neutralization. Calculate the concentration (molarity) of the original solution of calcium hydroxide.

Q: When organic compounds containing sulfur are burned, sulfur dioxide is produced

When organic compounds containing sulfur are burned, sulfur dioxide is produced. The amount of SO2 formed can be determined by the reaction with hydrogen peroxide: H2O2(aq) + SO2(g)...

Q: Acetate ion, C2H3O2-, has a stronger affinity for protons than

Acetate ion, C2H3O2-, has a stronger affinity for protons than does water. Therefore, when dissolved in water, acetate ion behaves as a(n) .

Q: Draw the structure of the carboxyl group, -COOH. Show

Draw the structure of the carboxyl group, -COOH. Show how a molecule containing the carboxyl group behaves as an acid when dissolved in water.

Q: Because of , even pure water contains measurable quantities of H+

Because of , even pure water contains measurable quantities of H+ and OH-.

Q: The number of in the logarithm of a number is equal to

The number of in the logarithm of a number is equal to the number of significant figures in the number.

Q: A solution with pH = 9 has a (higher/lower

A solution with pH = 9 has a (higher/lower) hydrogen ion concentration than a solution with pOH = 9.

Q: A 0.20 M HCl solution contains M hydrogen ion and

A 0.20 M HCl solution contains M hydrogen ion and M chloride ion concentrations.

Q: Calculate the percent by mass of solute in each of the following

Calculate the percent by mass of solute in each of the following solutions. a. 2.14 g of potassium chloride dissolved in 12.5 g of water b. 2.14 g of potassium chloride dissolved in 25.0 g of water...

Q: A(n) solution contains a conjugate acid–base pair

A(n) solution contains a conjugate acid–base pair and through this is able to resist changes in its pH.

Q: In each of the following chemical equations, identify the conjugate acid

In each of the following chemical equations, identify the conjugate acid–base pairs. a. HF(aq) + H2O(l) ⇌ F-(aq) 1 H3O+(aq) b. CN-(aq) + H2O(l) ⇌ HCN(aq) + OH-(aq) c. HCO3-(aq) + H2O(l) ⇌ H2CO3(aq)...

Q: Of the following combinations, which would act as buffered solutions?

Of the following combinations, which would act as buffered solutions? a. HClO2 and KClO2 b. H2S and Na2S c. HCOOH and NaHCO d. HClO and HClO4

Q: Calculate the pH corresponding to each of the pOH values listed,

Calculate the pH corresponding to each of the pOH values listed, and indicate whether each solution is acidic, basic, or neutral. a. pOH = 4.32 b. pOH = 8.90 c. pOH = 1.81 d. pOH = 13.1

Q: Write the equilibrium expression for each of the following heterogeneous equilibria.

Write the equilibrium expression for each of the following heterogeneous equilibria. a. 4Al(s) + 3O2( g) ⇌ 2Al2O3(s) b. NH3( g) + HCl( g) ⇌ NH4Cl(s) c. 2Mg(s) + O2( g) ⇌ 2MgO(s)

Q: Write the equilibrium expression for each of the following heterogeneous equilibria.

Write the equilibrium expression for each of the following heterogeneous equilibria. a. P4(s) + 5O2( g) ⇌ P4O10(s) b. CO2( g) + 2NaOH(s) ⇌ Na2CO3(s) + H2O( g) c. NH4NO3(s) ⇌ N2O( g) + 2H2O( g)

Q: Suppose the reaction system 2NO(g) + O2(

Suppose the reaction system 2NO(g) + O2(g) ⇌ 2NO2(g) has already reached equilibrium. Predict the effect of each of the following changes on the position of the equilibrium. Tell whether the equilibr...

Q: The reaction PCl3(l) + Cl2(g)

The reaction PCl3(l) + Cl2(g) ⇌ PCl5(s) liberates 124 kJ of energy per mole of PCl3 reacted. Will an increase in temperature shift the equilibrium position toward products or toward reactants?

Q: For the process CO(g) + H2O(g

For the process CO(g) + H2O(g) ⇌ CO2(g) + H2(g) it is found that the equilibrium concentrations at a particular temperature are [H2] = 1.4 M, [CO2] = 1.3 M, [CO] = 0.71 M, and [H2O] = 0.66 M. Calcu...

Q: For the reaction N2(g) + 3H2(g

For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) K = 1.3 * 10-2 at a given temperature. If the system at equilibrium is analyzed and the concentrations of both N2 and H2 are found to be 0.10 M, what is the...

Q: Calculate the percent by mass of solute in each of the following

Calculate the percent by mass of solute in each of the following solutions. a. 6.11 mg of calcium chloride dissolved in 5.25 g of water b. 6.11 mg of calcium chloride dissolved in 52.5 g of water c...

Q: The equilibrium constant for the reaction 2NOCl(g) ⇌

The equilibrium constant for the reaction 2NOCl(g) ⇌ 2NO(g) + Cl2(g) has the value 9.2 * 10-6 at a particular temperature. The system is analyzed at equilibrium, and it is found that the concentrati...

Q: As you learned in Chapter 7, most metal hydroxides are sparingly

As you learned in Chapter 7, most metal hydroxides are sparingly soluble in water. Write balanced chemical equations describing the dissolving of the following metal hydroxides in water. Write the exp...

Q: Approximately 9.0 * 10-4 g of silver chloride

Approximately 9.0 * 10-4 g of silver chloride, AgCl(s), dissolves per liter of water at 10 °C. Calculate Ksp for AgCl(s) at this temperature.

Q: Mercuric sulfide, HgS, is one of the least soluble salts

Mercuric sulfide, HgS, is one of the least soluble salts known, with Ksp = 1.6 * 10-54 at 25 °C. Calculate the solubility of HgS in moles per liter and in grams per liter.

Q: For the reaction N2( g) + 3H2( g)

For the reaction N2( g) + 3H2( g) 2NH3( g), list the types of bonds that must be broken and the type of bonds that must form for the chemical reaction to take place.

Q: What does the activation energy for a reaction represent? How is

What does the activation energy for a reaction represent? How is the activation energy related to whether a collision between molecules is successful?

Q: What are the catalysts in living cells called? Why are these

What are the catalysts in living cells called? Why are these biological catalysts necessary?

Q: When a reaction system has reached chemical equilibrium, the concentrations of

When a reaction system has reached chemical equilibrium, the concentrations of the reactants and products no longer change with time. Why does the amount of product no longer increase, even though lar...

Q: Ammonia, a very important industrial chemical, is produced by the

Ammonia, a very important industrial chemical, is produced by the direct combination of the elements under carefully controlled conditions. N2(g) + 3H2(g) ⇌ 2NH3(g) Suppose, in an experiment, that th...

Q: For the reaction 2CO2( g) ⇌ 2CO( g

For the reaction 2CO2( g) ⇌ 2CO( g) + O2( g) an analysis of an equilibrium mixture is performed. At a particular temperature, it is found that [CO] = 0.11 M, [O2] = 0.055 M, and [CO2] = 1.4 M. Calcul...

Q: What does it mean to say that an acid is strong in

What does it mean to say that an acid is strong in aqueous solution? What does this reveal about the ability of the acid’s anion to attract protons?

Q: At a particular temperature, a 3.50-L flask

At a particular temperature, a 3.50-L flask contains 1.16 moles of NH3, 2.40 moles of H2, and 1.14 moles of N2 in equilibrium. Calculate the value of K for the reaction 3H2(g) + N2(g) ⇌ 2NH3(g)

Q: Suppose that for a hypothetical reaction: A2(g)

Suppose that for a hypothetical reaction: A2(g) + 2B(g) ⇌ 2AB(g) It is determined that at a certain temperature the equilibrium concentrations are: [A2] = 0.0090, [B] = 0.940, and [AB] = 5.3 * 10-4....

Q: For the reaction: 3O2(g) ⇌ 2O3(

For the reaction: 3O2(g) ⇌ 2O3(g) K = 1.8 * 10-7 at a certain temperature. If at equilibrium [O2] = 0.062 M, calculate the equilibrium O3 concentration.

Q: The reaction H2(g) + I2(g)

The reaction H2(g) + I2(g) ⇌ 2HI(g) has Kp = 45.9 at 763 K. A particular equilibrium mixture at 763 K contains HI at a pressure of 4.94 atm and H2 at a pressure of 0.628 atm. Calculate the equilibrium...

Q: For the reaction: H2(g) + F2(

For the reaction: H2(g) + F2(g) ⇌ 2HF(g) K = 2.1 * 10-3 at a certain temperature. At equilibrium, [H2] = [F2] = 0.083 M. What is the concentration of HF under these conditions?

Q: For the following endothermic reaction at equilibrium: 2SO3(g

For the following endothermic reaction at equilibrium: 2SO3(g) ⇌ 2SO2(g) + O2(g) which of the following changes will increase the value of K? a. increasing the temperature b. decreasing the temp...

Q: Consider the following exothermic reaction at equilibrium: N2(g

Consider the following exothermic reaction at equilibrium: N2(g)+ 3H2(g) ⇌ 2NH3(g) Predict how the following changes affect the number of moles of each component of the system aft...

Q: Write the equilibrium expression for each of the following reactions.

Write the equilibrium expression for each of the following reactions. a. C2H6( g) + Cl2( g) ⇌ C2H5Cl(s) + HCl( g) b. 4NH3( g) + 5O2( g) ⇌ 4NO( g) + 6H2O( g) c. PCl5( g) ⇌ PCl3( g) + Cl2( g)

Q: Write the equilibrium expression for each of the following reactions.

Write the equilibrium expression for each of the following reactions. a. N2( g) + 3Cl2( g) ⇌ 2NCl3( g) b. H2( g) + I2( g) ⇌ 2HI( g) c. N2( g) + 2H2( g) ⇌ N2H4( g)

Q: Write the equilibrium expression for each of the following reactions.

Write the equilibrium expression for each of the following reactions. a. NO2( g) + ClNO( g) ⇌ ClNO2( g) + NO( g) b. Br2( g) + 5F2( g) ⇌ 2BrF5( g) c. 4NH3( g) + 6NO( g) ⇌ 5N2( g) + 6H2O( g)

Q: Calculate how many grams of solute and solvent are needed to prepare

Calculate how many grams of solute and solvent are needed to prepare the following solutions. a. 525 g of 3.91% iron(III) chloride solution b. 225 g of 11.9% sucrose solution c. 1.45 kg of 12.5% sod...

Q: Write the equilibrium expression for each of the following reactions.

Write the equilibrium expression for each of the following reactions. a. CO( g) + 2H2( g) ⇌ CH3OH( g) b. 2NO2( g) ⇌ 2NO( g) + O2( g) c. P4( g) + 6Br2( g) ⇌ 4PBr3( g)

Q: Suppose that for the reaction PCl5( g) ⇌ PCl3

Suppose that for the reaction PCl5( g) ⇌ PCl3( g) + Cl2( g) it is determined, at a particular temperature, that the equilibrium concentrations are [PCl5( g)] = 0.0711 M, [PCl3( g)] = 0.0302 M, and [C...

Q: For the simple reaction 2H2(g) + O2(

For the simple reaction 2H2(g) + O2(g) 2H2O(l) list the types of bonds that must be broken and the types of bonds that must form for the chemical reaction to take place.

Q: Ammonia, a very important industrial chemical, is produced by the

Ammonia, a very important industrial chemical, is produced by the direct combination of the following elements under carefully controlled conditions: N2(g) + 3H2(g) ⇌ 2NH3(g) Suppose, in an experimen...

Q: At high temperatures, elemental nitrogen and oxygen react with each other

At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide. N2(g) + O2(g) ⇌ 2NO(g) Suppose the system is analyzed at a particular temperature, and the equilib...

Q: Suppose that for the reaction 2N2O( g) + O2

Suppose that for the reaction 2N2O( g) + O2( g) ⇌ 4NO( g) it is determined, at a particular temperature, that the equilibrium concentrations are [NO( g)] = 0.00341 M, [N2O( g)] = 0.0293 M, and [O2( g...

Q: Write the equilibrium expression for each of the following heterogeneous equilibria.

Write the equilibrium expression for each of the following heterogeneous equilibria. a. P4(s) + 6F2( g) ⇌4PF3( g) b. Xe( g) + 2F2( g) ⇌XeF4(s) c. 2SiO(s) + 4Cl2( g) ⇌2SiCl4( l ) + O2( g)

Q: Write the equilibrium expression for each of the following heterogeneous equilibria.

Write the equilibrium expression for each of the following heterogeneous equilibria. a. 2LiHCO3(s) ⇌ Li2CO3(s) + H2O( g) + CO2( g) b. PbCO3(s) ⇌ PbO(s) + CO2( g) c. 4Al(s) + 3O2( g) ⇌ 2Al2O3(s)

Q: Write the equilibrium expression for each of the following heterogeneous equilibria.

Write the equilibrium expression for each of the following heterogeneous equilibria. a. C(s) + H2O( g) ⇌ H2( g) + CO( g) b. H2O( l ) ⇌ H2O( g) c. 4B(s) + 3O2( g) ⇌ 2B2O3(s)

Q: Indicate whether the stated equilibrium expression is correct for each of the

Indicate whether the stated equilibrium expression is correct for each of the following heterogeneous equilibria. For those expressions that are not correct, provide the correct expression along with...

Q: How is the strength of an acid related to the fact that

How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?

Q: In your own words, describe what Le Châtelier’s principle tells us

In your own words, describe what Le Châtelier’s principle tells us about how we can change the position of a reaction system at equilibrium.

Q: For an equilibrium involving gaseous substances, what effect, in general

For an equilibrium involving gaseous substances, what effect, in general terms, is realized when the volume of the system is decreased?

Q: For the reaction system C(s) + H2O(

For the reaction system C(s) + H2O( g) ⇌ H2( g) + CO( g) which has already reached a state of equilibrium, predict the effect that each of the following changes will have on the position of the equi...

Q: For the reaction system P4(s) + 6F2(

For the reaction system P4(s) + 6F2( g) ⇌ 4PF3( g) which has already reached a state of equilibrium, predict the effect that each of the following changes will have on the position of the equilibriu...

Q: Suppose the reaction system CH4(g) + 2O2(

Suppose the reaction system CH4(g) + 2O2(g) ⇌ CO2(g) + 2H2O(l) has already reached equilibrium. Predict the effect of each of the following changes on the position of the equilibrium. Tell whether th...

Q: Consider the general reaction 2A( g) + B(

Consider the general reaction 2A( g) + B(s) ⇌ C( g) + 3D( g) ∆H = 1115 kJ/mol which has already come to equilibrium. Predict whether the equilibrium will shift to the left, will shift to the right,...

Q: Hydrogen gas and chlorine gas in the presence of light react explosively

Hydrogen gas and chlorine gas in the presence of light react explosively to form hydrogen chloride H2( g) + Cl2( g) ⇌ 2HCl( g) The reaction is strongly exothermic. Would an increase in temperature fo...

Q: Hydrogen gas, oxygen gas, and water vapor are in equilibrium

Hydrogen gas, oxygen gas, and water vapor are in equilibrium in a closed container. Hydrogen gas is injected into the container, and the system is allowed to return to equilibrium. Which of the follow...

Q: The reaction C2H2(g) + 2Br2(g)

The reaction C2H2(g) + 2Br2(g) ⇌ C2H2Br4(g) is exothermic in the forward direction. Will an increase in temperature shift the position of the equilibrium toward reactants or products?

Q: When molecules collide, a certain minimum energy called the is needed

When molecules collide, a certain minimum energy called the is needed for the reaction to occur.

Q: How do the properties of a nonhomogeneous (heterogeneous) mixture differ

How do the properties of a nonhomogeneous (heterogeneous) mixture differ from those of a solution? Give two examples of nonhomogeneous mixtures.

Q: A strong acid has a weak conjugate base, whereas a weak

A strong acid has a weak conjugate base, whereas a weak acid has a relatively strong conjugate base. Explain.

Q: Old fashioned “smelling salts” consist of ammonium carbonate, (

Old fashioned “smelling salts” consist of ammonium carbonate, (NH4)2CO3. The reaction for the decomposition of ammonium carbonate (NH4)2CO3(s) ⇌ 2NH3(g) + CO2(g) + H2O(g) is endothermic. What would b...

Q: Plants synthesize the sugar dextrose according to the following reaction by absorbing

Plants synthesize the sugar dextrose according to the following reaction by absorbing radiant energy from the sun (photosynthesis). 6CO2(g) + 6H2O(g) ⇌ C6H12O6(s) + 6O2(g) Will an increase in...

Q: Suppose a reaction has the equilibrium constant K 5 1.7

Suppose a reaction has the equilibrium constant K 5 1.7 * 10-8 at a particular temperature. Will there be a large or small amount of unreacted starting material present when this reaction reaches equi...

Q: For the reaction Br2( g) + 5F2( g

For the reaction Br2( g) + 5F2( g) ⇌ 2BrF5( g) the system at equilibrium at a particular temperature is analyzed, and the following concentrations are found: [BrF5( g)] = 1.01 * 10-9 M, [Br2( g)] = 2...

Q: Consider the reaction SO2( g) + NO2( g

Consider the reaction SO2( g) + NO2( g) ⇌ SO3( g) + NO( g) Suppose it is found at a particular temperature that the concentrations in the system at equilibrium are as follows: [SO3( g)] = 4.99 * 10-5...

Q: For the reaction 2CO(g) + O2(g

For the reaction 2CO(g) + O2(g) ⇌ 2CO2(g) it is found at equilibrium at a certain temperature that the concentrations are [CO( g)] = 2.7 * 10-4 M, [O2( g)] = 1.9 * 10-3 M, and [CO2( g)] = 1.1 * 10-1...

Q: For the reaction CO2( g) + H2( g

For the reaction CO2( g) + H2( g) ⇌ CO( g) + H2O( g) the equilibrium constant, K, has the value 5.21 * 10-3 at a particular temperature. If the system is analyzed at equilibrium at this temperature,...

Q: The equilibrium constant for the reaction H2(g) +

The equilibrium constant for the reaction H2(g) + F2(g) ⇌ 2HF(g) has the value 2.1 * 103 at a particular temperature. When the system is analyzed at equilibrium at this temperature, the concentration...

Q: How does a catalyst work to speed up a chemical reaction?

How does a catalyst work to speed up a chemical reaction?

Q: 2H2O(g) ⇌ 2H2(g) + O2(

2H2O(g) ⇌ 2H2(g) + O2(g) K = 2.4 * 10-3 at a given temperature. At equilibrium it is found that [H2O( g)] = 1.1 * 10-1 M and [H2( g)] = 1.9 * 10-2 M. What is the concentration of O2( g) under these co...

Q: An aqueous solution is to be prepared that will be 7.

An aqueous solution is to be prepared that will be 7.51% by mass ammonium nitrate. What mass of NH4NO3 and what mass of water will be needed to prepare 1.25 kg of the solution?

Q: For the reaction 3O2( g) ⇌ 2O3( g

For the reaction 3O2( g) ⇌ 2O3( g) The equilibrium constant, K, has the value 1.12 * 10-54 at a particular temperature. a. What does the very small equilibrium constant indicate about the e...

Q: For the reaction N2O4(g) ⇌ 2NO2(g

For the reaction N2O4(g) ⇌ 2NO2(g) the equilibrium constant K has the value 8.1 * 10-3 at a particular temperature. If the concentration of N2O4(g) is found to be 5.4 * 10-4 M in the equilibrium syst...

Q: What is the special name given to the equilibrium constant for the

What is the special name given to the equilibrium constant for the dissolving of an ionic solute in water?

Q: Which of the following will affect the total amount of solute that

Which of the following will affect the total amount of solute that can dissolve in a given amount of solvent? a. The solution is stirred. b. The solute is ground to fine particles before dissolving....

Q: Write the balanced chemical equation describing the dissolving of each of the

Write the balanced chemical equation describing the dissolving of each of the following sparingly soluble salts in water. Write the expression for Ksp for each process. a. AgIO3(s) b. Sn(OH)2(s) c....

Q: Write the balanced chemical equation describing the dissolving of each of the

Write the balanced chemical equation describing the dissolving of each of the following sparingly soluble salts in water. Write the expression for Ksp for each process. a. NiS(s) b. CuCO3(s) c. BaC...

Q: Why are enzymes important? For example, what is the importance

Why are enzymes important? For example, what is the importance of the enzyme carbonic anhydrase in the body?

Q: A saturated solution of nickel(II) sulfide contains approximately 3

A saturated solution of nickel(II) sulfide contains approximately 3.6 * 10-4 g of dissolved NiS per liter at 20 °C. Calculate the solubility product Ksp for NiS at 20 °C.