Question: A is some factor that

> The mass 1.66 * 10-24 g is equivalent to 1 .

> 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 transition metal, M? a. Th b. Ti c. Hg d. Ru e. Ag

> Calculate the number of grams of lithium that contain the same number of atoms as 1.00 kg of zirconium.

> 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 sodium nitrate e. 0.000357 mole of iron

> 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 following could be a molar mass of the compound? i. 13.01

> 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. The mass of the copper sample is more than twice as grea

> Given that the molar mass of carbon tetrachloride, CCl4, is 153.8 g, calculate the mass in grams of 1 molecule of CCl4.

> For the following chemical reactions, determine the precipitate produced when the two reactants listed below are mixed together. Indicate “none” if no precipitate will form. Formula of Precipitate Sr(NO3)2(aq) + К,

> For the following chemical reactions, determine the precipitate produced when the two reactants listed below are mixed together. Indicate “none” if no precipitate will form. Formula of Precipitate Na,SO4(aq) + Pb(

> 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 atoms in 12.01 g of carbon (5) 6.022 * 1023 molecules

> 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 using the correct formulas in your explanation.

> 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 in the presence of moisture. Write a balanced equation

> 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.

> 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 of moles of C3H8 (g)? What mole ratios enable you to c

> 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 of trichloroethane, C2H3Cl3 e. 0.167 mole of lithium

> 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.

> 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

> 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

> 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.

> 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?

> 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?

> Balance each of the following equations that describe decomposition reactions. a. NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g) b. NaClO3(s) NaCl(s) + O2(g) c. HgO(s) Hg(l) +

> 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) HCl(g) d. K(s) + S8(s)

> 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 chemical reaction occurs, then a net ionic equation cannot

> What are the molecular and empirical formulas for the following molecule? Explain your reasoning. H Н-С—ОН Н. HO OH H HO `H. С—С H OH

> 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 = 1⁄1000 mole) d. 1.31 * 10-3 moles of uranium e. 0.00104

> 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?

> For the reaction 16Fe(s) + 3S8(s) 8Fe2S3(s), show how electrons are gained and lost by the atoms.

> For the reaction 2Al(s) + 3I2(s) 2AlI3(s), show how electrons are gained and lost by the atoms. © Cengage Leaming

> 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 sulfate, Na2SO4

> Write the balanced molecular, complete ionic, and net ionic equations for the reaction of ammonium sulfide with iron(III) chloride.

> 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. CaCl2(aq) + Na3PO4(aq) Ca3(PO4)2(s) + Na

> 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, water). For each salt, write an equation showing the forma

> 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.

> 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) + BaCl2(aq) BaSO4 b

> 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 instructor takes samples of iron and sulfur and just mixes th

> 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 chloride d. 4.75 g of calcium sulfate e. 96.2 mg of nitro

> 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) b. H2SO4(aq) + Ba(OH)2(aq) c. HClO4(aq) + NaOH(aq)

> 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 reaction occurs, so indicate. a. iron(III) nitrate and

> 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+

> 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.

> 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) + P(s) Na3P(s) d. CH4(g) + Cl2(g)

> 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(s) + H2O(g) + CO2(g) d. C6H6(l) C(s)

> 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)

> 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) H3PO4(aq)

> 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 magnesium oxide was present. What is the student’s percent yi

> 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.

> 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 H2O2

> 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 not be 100%.

> 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 acid is added to water, the solution gets very hot. d

> What are the four “stages” of coal formation? How do the four types of coal differ?

> 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 tetroxide, N2O4 d. diphenyl ether, C12H10O, and phenol, C6H5O

> 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-butene, C4H6Cl2

> Explain to a friend who has not yet taken a chemistry course what is meant by the empirical formula of a compound.

> What experimental evidence about a new compound must be known before its formula can be determined?

> Why is the “quality” of energy decreasing in the universe?

> Why are petroleum products especially useful as sources of energy?

> 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 uranium e. 29.7 g of sodium acetate f. 1.03 g of sul

> 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?

> 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 stored in the gasoline be reused once it is dispersed to t

> 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.

> When a chemical system evolves energy, where does the energy go?

> 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 answer. a. Both CuSO4 and KI are equally limiting be

> 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 with the smallest coefficient in the balanced chemical

> If the amount of a sample doubles, what happens to the percent composition of each element in the compound?

> 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.

> In studying heat flows for chemical processes, what do we mean by the terms system and surroundings?

> 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 between moles of reactants and moles of products, we use mol

> 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. 5.04 g of aluminum sulfate e. 2.99 g of lead(II) chlor

> A is a device used to determine the heat associated with a chemical reaction.

> 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 chemical equation is SOCl2(l) + H2O(l)

> 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(s) + 11H2O(g) What mass of carbon is produced if 1.19

> represents the ability to do work or to produce heat.

> 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 will not result in the production of 2 g of H2O.

> 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 used in bombs and incendiary devices for warfare. P4(s)

> 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 following balanced equation: NH4Cl(s) + NaOH(s)

> 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) H2O(l) + SO2(g) If 4.25 g of sulfurous aci

> 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 the reaction by which wines are produced from grape j

> 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 is heated and placed in pure chlorine gas, the iron “

> 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

> Define the amu. What is one amu equivalent to in grams?

> 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 will remain if a 1.52-g sample of sodium hydrogen carbon

> 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 monofluoride must be used to produce 30.0 g of nitrogen tr

> 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 carbide is useful because it reacts readily with water

> “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. The strong odor of the ammonia usually restores conscio

> Describe in your own words how the molar mass of the compound below may be calculated. 1 CH4 molecule

> The of a substance is the mass (in grams) of 1 mole of the substance.

> 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 exactly 1 g of C will react with exactly 1 g of O2. True or

> 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, just as they can be changed to balance the charges when

> 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.

> 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 proportions in which these substances react on a macroscop

> 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

> What does it mean to say that the balanced chemical equation for a reaction describes the stoichiometry of the reaction?

> What quantity serves as the conversion factor between the mass of a sample and how many moles the sample contains?

> Which weighs less, 0.25 mole of xenon atoms or 2.0 moles of carbon atoms?

> Which has the smaller mass, 1 mole of He atoms or 4 moles of H atoms?

> 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?

> If an average sodium atom has a mass of 3.82 * 10-23 g, what is the mass of a magnesium atom in grams?

> What mass of cobalt contains the same number of atoms as 57.0 g of fluorine?

> What mass of hydrogen contains the same number of atoms as 7.00 g of nitrogen?