Question: Kitchen Supply, Inc. (KSI), manufactures three
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 an activity-based costing system and prepared the following cost estimates for year 2 for the recommended cost drivers.
In addition, management estimated 7,500 direct labor-hours for year 2.
Assume that the following cost driver volumes occurred in January year 2:
Required
a. Compute a predetermined overhead rate for year 2 for each cost driver using the estimated costs and estimated cost driver units prepared by the consultant. Also compute a predetermined rate for year 2 using direct labor-hours as the allocation base.
b. Compute the production costs for each product for January using direct labor-hours as the allocation base and the predetermined rate computed in requirement (a).
c. Compute the production costs for each product for January using the cost drivers recommended by the consultant and the predetermined rates computed in requirement (a). (Do not assume that total overhead applied to products in January will be the same for activity-based costing as it was for the labor-hour-based allocation.)
d. Management has seen your numbers and wants an explanation for the discrepancy between the product costs using direct labor-hours as the allocation base and the product costs using activity-based costing. Write a brief response to management.
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> 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)
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> 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+
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> 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.
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> 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.
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> 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).
> What structural feature distinguishes aldehydes from ketones?
> 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?
