> Allcott Computer Services (ACS) provides computer training and repair services for schools and local businesses. Sales for year 1 totaled $1,350,000. Information regarding resources for the year includes the following:In addition, ACS spent $42,000 on 50
> Leidenheimer Corporation manufactures small airplane propellers. Sales for year 2 totaled $1,700,000. Information regarding resources for the month follows:In addition, Leidenheimer spent $50,000 on 50 engineering changes with a cost-driver rate of $1,00
> Refer to Exercise 10-38.Exercise 10-38Gunnison Supply provides the following information about resources:In addition, sales for the period totaled $150,000.Requireda. Prepare a traditional income statement like the one in Exhibit 10.10.b. Prepare an acti
> Chelsea Household Renovations (CHR) is a rapidly growing company that has not been profitable despite increases in sales. It has hired you as a consultant to find ways to improve profitability. You believe that the problem results from poor cost control
> A tornado struck the only manufacturing plant of Toledo Farm Implements (TFI) on June 1. All work-in-process inventory was destroyed, but a few records were salvaged from the wreckage and from the company’s headquarters. If acceptable documentation is pr
> The following transactions occurred in January at Dungan Cabinetry, a furniture maker that uses job costing:1. Purchased $53,700 in materials on account.2. Issued $1,500 in supplies from the materials inventory to the production department.3. Paid for th
> Amazon Beverages produces and bottles a line of soft drinks using exotic fruits from Latin America and Asia. The manufacturing process entails mixing and adding juices and coloring ingredients at the bottling plant, which is a part of Mixing Division. Th
> Panther Corporation appeared to be experiencing a good year. Sales in the first quarter were one-third ahead of last year, and the sales department predicted that this rate would continue throughout the entire year. The controller asked Janet Nomura, a s
> MTI makes three types of lawn tractors: M3100, M4100, and M6100. In the past, it allocated overhead to products using machine-hours. Last year, the company produced 10,000 units of M3100, 17,500 units of M4100, and 10,000 units of M6100 and had the follo
> Chander, Inc., manufactures cloth shopping bags. The controller is preparing a budget for the coming year and asks for your assistance. The following costs and other data apply to bag production:Direct materials per bag1.0 yard cotton at $3 per yard0.2 y
> Cameron Parts has the following data from year 1 operations, which are to be used for developing year 2 budget estimates:Sales revenue (12,500 units). . . . . . . . $ 1,119,000Manufacturing costsMaterials . . . . . . . . . . . . . . . . . . . . . . . . .
> Pharmaceutical firms, oil and gas companies, and other ventures inevitably incur costs on unsuccessful investments in new projects (e.g., new drugs or new wells). For oil and gas firms, a debate continues over whether those costs should be written off as
> House Station, Inc., is a nationwide hardware and furnishings chain. The manager of the House Station Store in Portland is evaluated using ROI. House Station headquarters requires an ROI of 10 percent of assets. For the coming year, the manager estimates
> Huron Furniture is considering updating its cost system to an activity-based costing system and is interested in understanding the effects. The company’s cost accountant has identified three overhead cost pools along with appropriate co
> Pickle Motorcycles, Inc. (PMI), manufactures three motorcycle models: a cruising bike (Route 66), a street bike (Main Street), and a starter model (Alley Cat). Because of the different materials used, production processes for each model differ significan
> The following information is available for year 1 for Dancer Components:Sales revenue (300,000 units) . . . . . . $5,700,000Manufacturing costsMaterials . . . . . . . . . . . . . . . . . . . . . . . . . $ 336,000Variable cash costs . . . . . . . . . . .
> Kitchen Supply, Inc. (KSI), manufactures three types of flatware: institutional, standard, and silver. It applies all indirect costs according to a predetermined rate based on direct labor-hours. A consultant recently suggested that the company switch to
> Clemson Company prepares its budgets on the basis of standard costs. A responsibility report is prepared monthly showing the differences between master budget and actual results. Variances are analyzed and reported separately. There are no materials inve
> Balance each of the following half-reactions. a. I-(aq) / I2(s) b. O2( g) / O2-(s) c. P4(s) / P3-(s) d. Cl2( g) / Cl-(aq)
> In each of the following reactions, identify which element is oxidized and which is reduced by assigning oxidation states. a. 2B2O3(s) + 6Cl2(g) / 4BCl3(l) + 3O2(g) b. GeH4(g) + O2(g) / Ge(s) + 2H2O(g) c. C2H4(g) + Cl2(g) / C2H4Cl2(l) d. O2(g) + 2F2(g)
> In each of the following reactions, identify which element is oxidized and which is reduced by assigning oxidation states. a. C(s) + O2( g) / CO2( g) b. 2CO( g) + O2( g) / 2CO2( g) c. CH4( g) + 2O2( g) / CO2( g) + 2H2O( g) d. C2
> Assign oxidation states to all of the atoms in each of the following: a. BiO+ b. PO43- c. NO2- d. Hg22+
> Assign oxidation states to all of the atoms in each of the following: a. CrCl3 b. K2CrO4 c. K2Cr2O7 d. Cr(C2H3O2)2
> Assign oxidation states to all of the atoms in each of the following: a. MnO2 b. BaCrO4 c. H2SO3 d. Ca3(PO4)2
> Assign oxidation states to all of the atoms in each of the following: a. PBr3 b. C3H8 c. KMnO4 d. CH3COOH
> Assign oxidation states to all of the atoms in each of the following: a. NH3 b. CO c. CO2 d. NF3
> For each of the following oxidation–reduction reactions of metals with nonmetals, identify which element is oxidized and which is reduced. a. 3Zn(s) + N2( g) Zn3N2(s) b. Co(s) + S(s) CoS(s) c. 4K(s) + O2( g) 2K2O(s) d.
> For each of the following oxidation–reduction reactions of metals with nonmetals, identify which element is oxidized and which is reduced. a. 4Na(s) + O2( g) 2Na2O(s) b. Fe(s) + H2SO4(aq) FeSO4(aq) + H2( g) c. 2Al2O3(s)
> Explain why, although it is not an ionic compound, we still assign oxygen an oxidation state of -2 in water, H2O. Give an example of a compound in which oxygen is not in the -2 oxidation state.
> Balance each of the following oxidation–reduction reactions, which take place in acidic solution. a. MnO4-(aq) + H2O2(aq) / Mn2+(aq) + O2( g) b. BrO3-(aq) + Cu+(aq) / Br-(aq) + Cu2+(aq) c. HNO2(aq) + I-(aq) / NO( g) + I2(aq)
> Balance each of the following oxidation–reduction reactions by inspection. a. C3H8( g) + O2( g) / CO2( g) + H2O( g) b. CO( g) + H2( g) / CH3OH( l ) c. SnO2(s) + C(s) / Sn(s) + CO( g) d. C2H5OH( l ) + O2( g) / CO2( g) + H2O( g)
> Carbon compounds containing double bonds (such compounds are called alkenes) react readily with many other reagents. In each of the following reactions, identify which atoms are oxidized and which are reduced, and specify the oxidizing and reducing agent
> In each of the following reactions, identify which species is the oxidizing agent. a. 2Al(s) + 6HCl(aq) ( 2AlCl3(aq) + 3H2(g) b. Cu(s) + H2SO4(aq) ( CuSO4(aq) + H2(g)
> In each of the following reactions, identify which element is oxidized and which is reduced. a. Zn(s) + 2HCl(aq) ZnCl2(aq) + H2( g) b. 2CuI(s) CuI2(s) + Cu(s) c. 6Fe2+(aq) + Cr2O72-(aq) + 14H+(aq) 6Fe3+
> For each of the following unbalanced oxidation–reduction chemical equations, balance the equation by inspection, and identify which species is the reducing agent. a. Fe(s) + O2(g) / Fe2O3(s) b. Al(s) + Cl2(g) / AlCl3(s) c. Mg(s) + P4(s)
> Although aluminum is a reactive metal, pure aluminum ordinarily does not corrode severely in air because a protective layer of builds up on the metal’s surface.
> Corrosion of a metal represents its by species present in the atmosphere.
> The common acid dry cell battery typically contains an inner casing made of metal, which functions as the anode.
> The process of involves forcing a current through a cell to produce a chemical change that would not otherwise occur. How is this process different than what occurs in a galvanic cell?
> Why must the sum of all the oxidation states of the atoms in a neutral molecule be zero?
> The “pressure” on electrons to flow from one electrode to the other in a battery is called the of the battery.
> In a(n) cell, electrons flow through a wire from the reducing agent to the oxidizing agent.
> What systematic ending is used to show that a molecule is a carboxylic acid? Give an example.
> Which process (oxidation/reduction) takes place at the anode of a galvanic cell?
> An electrochemical cell that produces a current from an oxidation–reduction reaction is often called a(n) cell.
> To obtain useful electrical energy from an oxidation–reduction process, we must set up the reaction in such a way that the oxidation half-reaction and the reduction half-reaction are physically one another.
> When we balance an oxidation–reduction equation, the number of electrons lost by the reducing agent must the number of electrons gained by the oxidizing agent.
> To function as a good reducing agent, a species must electrons easily.
> An oxidizing agent causes the (oxidation/reduction) of another species, and the oxidizing agent itself is (oxidized/reduced).
> let’s us keep track of electrons in oxidation– reduction reactions by assigning charges to the various atoms in a compound.
> Why is methanol sometimes called wood alcohol? Describe the modern synthesis of methanol. What are some uses of methanol?
> Although nuclear processes offer the potential for an abundant source of energy, no nuclear power plants have been built in the United States for some time. In addition to the fear of a malfunction in such a plant (as happened at the Three Mile Island nu
> How do the chemical properties of radioactive nuclei (as opposed to the nuclear decay they undergo) influence the degree of damage they do to an organism?
> Explain why, although gamma rays are far more penetrating than alpha particles, the latter are actually more likely to cause damage to an organism. Which radiation is more effective at causing ionization of biomolecules?
> Write the equation for the synthesis of ethanol from ethylene. What are some commercial uses of ethanol made by this process?
> The “Chemistry in Focus” segment Water-Powered Fireplace discusses a fireplace that uses the electrolysis of water to produce hydrogen gas. Write the balanced chemical equation for the electrolysis of water. Which element in water is oxidized? Which is r
> Although the energy transferred per event when a living creature is exposed to radiation is small, why is such exposure dangerous?
> What are some important uses of electrolysis?
> What type of “fuel” could be used in a nuclear fusion reactor, and why is this desirable?
> If a benzene ring contains several substituents, how are the relative locations of the substituents numbered in the systematic name given to the molecule?
> For each of the following oxidation–reduction reactions, identify which element is oxidized and which is reduced. a. Mg(s) + Br2( l ) MgBr2(s) b. 2Na(s) + S(s) Na2S(s) c. CO2( g) + H2( g) CO( g) + H2O( g)
> Benzene exhibits resonance. Explain this statement in terms of the different Lewis structures that can be drawn for benzene.
> Explain how some metals, notably aluminum, naturally resist complete oxidation by the atmosphere.
> What is a meltdown, and how can it occur? Most nuclear reactors use water as the cooling liquid. Is there any danger of a steam explosion if the reactor core becomes overheated?
> Can a nuclear explosion take place in a reactor? Is the concentration of fissionable material used in reactors large enough for this?
> Describe the purpose of each of the major components of a nuclear reactor (moderator, control rods, containment, cooling liquid, and so on).
> What does it mean to say that fissionable material possesses a critical mass? Can a chain reaction occur when a sample has less than the critical mass?
> The thyroid gland is interesting in that it is practically the only place in the body where the element iodine is used. How have radiotracers been used to study and treat illnesses of the thyroid gland?
> Why does an ancient wood or cloth artifact contain less 6 14
> In dating artifacts using carbon-14, an assumption is made about the amount of carbon-14 in the atmosphere. What is this assumption? Why is the assumption important?
> What is a salt bridge? Why is a salt bridge necessary in a galvanic cell? Can some other method be used in place of the salt bridge?
> For each of the following oxidation–reduction reactions, identify which element is being oxidized and which is being reduced. a. Ca(s) + 2H2O(l) Ca(OH)2(s, aq) + H2(g) b. H2(g) + F2(g) 2HF( g) c. 4Fe(s) + 3O2(g)
> Describe in general terms how an archaeological artifact is dated using carbon-14.
> The element krypton has several radioactive isotopes. Below are listed several of these isotopes along with their half-lives. Which of the isotopes is most stable? Which of the isotopes is “hottest”? If we were to begin a half-life experiment with separa
> Iodide ion, I-, is one of the most easily oxidized species. Balance each of the following oxidation–reduction reactions, which take place in acidic solution, by using the “half-reaction” method. a. IO3-(aq) + I-(aq) I2(aq) b. Cr2O72-(aq)
> Balance each of the following oxidation–reduction reactions, which take place in acidic solution, by using the “half-reaction” method. a. Al(s) + H+(aq) / Al3+(aq) + H2(g) b. S2–(aq) + NO3–(g) / S(s) + NO(g) c. I2(aq) + Cl2(aq) / IO3–(aq) + HCl(g) d.
> Balance each of the following oxidation–reduction reactions, which take place in acidic solution, by using the “half-reaction” method. a. Mg(s) + Hg2+(aq) / Mg2+(aq) + Hg22+(aq) b. NO3–(aq) + Br–(aq) / NO(g) + Br2(l) c. Ni(s) + NO3–(aq) / Ni2+(aq) + NO
> Balance each of the following half-reactions, which take place in acidic solution. a. O2(g) / H2O(l) b. SO42–(aq) / H2SO3(aq) c. H2O 2(aq) / H2O(l) d. NO2–(aq) / NO3–(aq)
> Balance each of the following half-reactions, which take place in acidic solution. a. HClO(aq) Cl-(aq) b. NO(aq) N2O( g) c. N2O(aq) N2( g) d. ClO3-(aq) HClO2(aq)
> Balance each of the following half-reactions. a. 3N2( g) + 2e- 2N3-(aq) b. O22-(aq) O2( g) c. Zn(s) Zn2+(aq) d. F2( g) F-(aq)
> Balance each of the following half-reactions. a. Cu / Cu2+ b. Fe3+ / Fe2+ c. Br– / Br2 d. Fe2+ / Fe
> Why must the number of electrons lost in the oxidation equal the number of electrons gained in the reduction? Is it possible to have “leftover” electrons in a reaction?
> For each of the following oxidation–reduction reactions, identify which element is oxidized and which is reduced. a. 6Na(s) + N2( g) 2Na3N(s) b. Mg(s) + Cl2( g) MgCl2(s) c. 2Al(s) + 3Br2( l ) 2AlBr3(s)
> What is a half-reaction? What does each of the two half- reactions that make up an overall process represent?
> Why is a systematic method for balancing oxidation–reduction reactions necessary? Why can’t these equations be balanced readily by inspection?
> In what two respects must oxidation–reduction reactions be balanced?
> Potassium iodide in solution reacts readily with many reagents. In the following reactions, identify the atoms that are being oxidized and reduced, and specify the oxidizing and reducing agents. a. Cl2( g) + KI(aq) KCl(aq) + I2(s) b. 2
> Complete the following table with the nuclear particle that is produced in each nuclear reaction. Initial Nuclide Product Nuclide Particle Produced 239Pu 94 235 김 Pb BI 214 214 83 Co NI 99- Ru 239 93 239 Pu
> Consider the oxidation–reduction reaction Mg(s) + Cu2+(aq) / Mg2+(aq) + Cu(s) Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reactio
> Consider a galvanic cell based on the following oxidation– reduction reaction: 2Al3+(aq) + 3Mg(s) ( 2Al(s) + 3Mg2+(aq) What will the electrode found in the cathode portion of the cell be made of? Explain your answer. a. air b. HCl c. Mg d. Al e. H2
> Each of the following nuclides is known to undergo radioactive decay by production of a ß particle, /. Write a balanced nuclear equation for each process. a. 53 136
> Write a nuclear equation showing the bombardment of beryllium-9 with alpha particles, resulting in production of carbon-12 and a neutron.
> Write a balanced nuclear equation for the bombardment of 7 14
> How many of the following statements regarding the decay of radioactive nuclides are true? a. During a given period of time, a radioactive nucleus with a short half-life is much more likely to decay than one with a long half-life. b. As a nuclide decay
> What do we mean when we say that one radioactive nucleus is “hotter” than another? Which element would have more decay events over a given period of time?
> Complete each of the following nuclear equations by supplying the missing particle. a. 88 226
> Aluminum exists in several isotopic forms, including /Al, /Al, and /Al. Indicate the number of protons and the number of neutrons in each of these isotopes.
> The element zinc in nature consists of five isotopes with higher than 0.5% natural abundances, with mass numbers 64, 66, 67, 68, and 70. Write the nuclear symbol for each of these isotopes. How many protons does each contain? How many neutrons does each
> Zirconium consists of five primary isotopes, of mass numbers and abundances shown below: Zr-90………...51.5% Zr-91………….11.2% Zr-92………...17.1% Zr-94……….17.4% Zr-96…………2.8% Write the nuclear symbol,
> Each of the following nuclides is known to undergo radioactive decay by production of a ß particle, /. Write a balanced nuclear equation for each process. a. / b. / c. /
