Science
ChemistryChemistry: An Atoms First ApproachIt takes 15 kWh (kilowatt-hours) of electrical energy to produce 1.0 kg aluminum metal from aluminum oxide by the Hall-Heroult process. Compare this to the amount of energy necessary to melt 1.0 kg aluminum metal. Why is it economically feasible to recycle aluminum cans? [The enthalpy of fusion for aluminum metal is 10.7 kJ/mol (1 watt = 1 J/s).]

It takes 15 kWh (kilowatt-hours) of electrical energy to produce 1.0 kg aluminum metal from aluminum oxide by the Hall-Heroult process. Compare this to the amount of energy necessary to melt 1.0 kg aluminum metal. Why is it economically feasible to recycle aluminum cans? [The enthalpy of fusion for aluminum metal is 10.7 kJ/mol (1 watt = 1 J/s).]

BuyFind

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
BuyFind

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

Solutions

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Chapter 17, Problem 131AE
Textbook Problem

It takes 15 kWh (kilowatt-hours) of electrical energy to produce 1.0 kg aluminum metal from aluminum oxide by the Hall-Heroult process. Compare this to the amount of energy necessary to melt 1.0 kg aluminum metal. Why is it economically feasible to recycle aluminum cans? [The enthalpy of fusion for aluminum metal is 10.7 kJ/mol (1 watt = 1 J/s).]

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Chapter 17,
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Chapter 17 Solutions

Chemistry: An Atoms First Approach
Ch. 17 - What is a half-reaction? Why must the number of...Ch. 17 - Galvanic cells harness spontaneous...Ch. 17 - Table 17-1 lists common half-reactions along with...Ch. 17 - Consider the equation G = -nF. What are the four...Ch. 17 - The Nernst equation allows determination of the...Ch. 17 - What are concentration cells? What is in a...Ch. 17 - Batteries are galvanic cells. What happens to as a...Ch. 17 - Not all spontaneous redox reactions produce...Ch. 17 - What characterizes an electrolytic cell? What is...Ch. 17 - Sketch a galvanic cell, and explain how it works....
Ch. 17 - In making a specific galvanic cell, explain how...Ch. 17 - You want to plate out nickel metal from a nickel...Ch. 17 - A copper penny can be dissolved in nitric acid but...Ch. 17 - Sketch a cell that forms iron metal from iron(II)...Ch. 17 - Which of the following is the best reducing agent:...Ch. 17 - You are told that metal A is a better reducing...Ch. 17 - Explain the following relationships: G and w, cell...Ch. 17 - Explain why cell potentials are not multiplied by...Ch. 17 - What is the difference between and ? When is equal...Ch. 17 - Consider the following galvanic cell: What happens...Ch. 17 - Look up the reduction potential for Fe3+ to Fe2+....Ch. 17 - If the cell potential is proportional to work and...Ch. 17 - Is the following statement true or false?...Ch. 17 - Define oxidation and reduction in terms of both...Ch. 17 - Assign oxidation numbers to all the atoms in each...Ch. 17 - Specify which of the following equations represent...Ch. 17 - The Ostwald process for the commercial production...Ch. 17 - What is electrochemistry? What are redox...Ch. 17 - When balancing equations in Chapter 5, we did not...Ch. 17 - When magnesium metal is added to a beaker of...Ch. 17 - How can one construct a galvanic cell from two...Ch. 17 - The free energy change for a reaction, G, is an...Ch. 17 - What is wrong with the following statement: The...Ch. 17 - When jump-starting a car with a dead battery, the...Ch. 17 - In theory, most metals should easily corrode in...Ch. 17 - Consider the electrolysis of a molten salt of some...Ch. 17 - Consider the following electrochemical cell: a. If...Ch. 17 - Balance the following oxidationreduction reactions...Ch. 17 - Balance the following oxidationreduction reactions...Ch. 17 - Balance the following oxidation-reduction...Ch. 17 - Balance the following oxidationreduction reactions...Ch. 17 - Chlorine gas was first prepared in 1774 by C. W....Ch. 17 - Gold metal will not dissolve in either...Ch. 17 - Consider the following galvanic cell: Label the...Ch. 17 - Consider the following galvanic cell: a. Label the...Ch. 17 - Sketch the galvanic cells based on the following...Ch. 17 - Sketch the galvanic cells based on the following...Ch. 17 - Calculate values for the galvanic cells in...Ch. 17 - Calculate values for the galvanic cells in...Ch. 17 - Sketch the galvanic cells based on the following...Ch. 17 - Sketch the galvanic cells based on the following...Ch. 17 - Give the standard line notation for each cell in...Ch. 17 - Give the standard line notation for each cell in...Ch. 17 - Consider the following galvanic cells: For each...Ch. 17 - Give the balanced cell equation and determine for...Ch. 17 - Calculate values for the following g cells. Which...Ch. 17 - Calculate values for the following cells. Which...Ch. 17 - Chlorine dioxide (C1O2), which is produced by the...Ch. 17 - The amount of manganese in steel is determined by...Ch. 17 - Calculate the maximum amount of work that can be...Ch. 17 - Calculate the maximum amount of work that can be...Ch. 17 - Estimate for the half-reaction 2H2O+2eH2+2OH given...Ch. 17 - The equation G = nF also can be applied to...Ch. 17 - Glucose is the major fuel for most living cells....Ch. 17 - Direct methanol fuel cells (DMFCs) have shown some...Ch. 17 - Using data from Table 17-1, place the following in...Ch. 17 - Using data from Table 17-1, place the following in...Ch. 17 - Answer the following questions using data from...Ch. 17 - Answer the following questions using data from...Ch. 17 - Consider only the species (at standard conditions)...Ch. 17 - Consider only the species (at standard conditions)...Ch. 17 - Use the table of standard reduction potentials...Ch. 17 - Use the table of standard reduction potentials...Ch. 17 - Hydrazine is somewhat toxic. Use the...Ch. 17 - The compound with the formula TlI3 is a black...Ch. 17 - A galvanic cell is based on the following...Ch. 17 - Consider the concentration cell in Fig. 17-10. If...Ch. 17 - Consider the concentration cell shown below....Ch. 17 - Consider a concentration cell similar to the one...Ch. 17 - The overall reaction in the lead storage battery...Ch. 17 - Calculate the pH of the cathode compartment for...Ch. 17 - Consider the cell described below:...Ch. 17 - Consider the cell described below:...Ch. 17 - Calculate G and K at 25C for the reactions in...Ch. 17 - Calculate G and K at 25C for the reactions in...Ch. 17 - Consider the galvanic cell based on the following...Ch. 17 - Consider the galvanic cell based on the following...Ch. 17 - An electrochemical cell consists of a standard...Ch. 17 - An electrochemical cell consists of a nickel metal...Ch. 17 - An electrochemical cell consists of a standard...Ch. 17 - An electrochemical cell consists of a nickel metal...Ch. 17 - Consider a concentration cell that has both...Ch. 17 - You have a concentration cell in which the cathode...Ch. 17 - Under standard conditions, what reaction occurs,...Ch. 17 - A disproportionation reaction involves a substance...Ch. 17 - Consider the following galvanic cell at 25C:...Ch. 17 - An electrochemical cell consists of a silver metal...Ch. 17 - Calculate Ksp for iron(II) sulfide given the...Ch. 17 - For the following half-reaction, = 2.07 V:...Ch. 17 - Calculate for the following half-reaction:...Ch. 17 - The solubility product for CuI(s) is 1.1 102...Ch. 17 - How long will it take to plate out each of the...Ch. 17 - The electrolysis of BiO+ produces pure bismuth....Ch. 17 - What mass of each of the following substances can...Ch. 17 - Aluminum is produced commercially by the...Ch. 17 - An unknown metal M is electrolyzed. It took 74.1 s...Ch. 17 - Electrolysis of an alkaline earth metal chloride...Ch. 17 - What volume of F2 gas, at 25C and 1.00 atm, is...Ch. 17 - What volumes of H2(g) and O2(g) at STP are...Ch. 17 - A single HallHeroult cell (as shown in Fig. 17-22)...Ch. 17 - A factory wants to produce 1.00 103 kg barium...Ch. 17 - It took 2.30 min using a current of 2.00 A to...Ch. 17 - A solution containing Pt4+ is electrolyzed with a...Ch. 17 - A solution at 25C contains 1.0 M Cd2+, 1.0 M Ag+,...Ch. 17 - Consider the following half-reactions: A...Ch. 17 - In the electrolysis of an aqueous solution of...Ch. 17 - Copper can be plated onto a spoon by placing the...Ch. 17 - What reactions take place at the cathode and the...Ch. 17 - What reaction will take place at the Cathode and...Ch. 17 - What reactions take place at the cathode and the...Ch. 17 - What reaction will take place at the Cathode and...Ch. 17 - Gold is produced electrochemically from an aqueous...Ch. 17 - The blond alcohol (C2H5OH) level can be determined...Ch. 17 - The saturated calomel electrode. abbreviated SCE....Ch. 17 - Consider the following half-reactions: Explain why...Ch. 17 - Consider the standard galvanic cell based on the...Ch. 17 - A standard galvanic cell is constructed so that...Ch. 17 - The black silver sulfide discoloration of...Ch. 17 - In 1973 the wreckage of the Civil War ironclad USS...Ch. 17 - When aluminum foil is placed in hydrochloric acid,...Ch. 17 - Which of the following statements concerning...Ch. 17 - A fuel cell designed to react grain alcohol with...Ch. 17 - The overall reaction and equilibrium constant...Ch. 17 - What is the maximum work that can be obtained from...Ch. 17 - The overall reaction and standard cell potential...Ch. 17 - An experimental fuel cell has been designed that...Ch. 17 - The ultimate electron acceptor in the respiration...Ch. 17 - One of the few industrial-scale processes that...Ch. 17 - It took 150. s for a current of 1.25 A to plate...Ch. 17 - It takes 15 kWh (kilowatt-hours) of electrical...Ch. 17 - In the electrolysis of a sodium chloride solution,...Ch. 17 - An aqueous solution of an unknown salt of...Ch. 17 - Which of the following statement(s) is/are true?...Ch. 17 - Consider a galvanic cell based on the following...Ch. 17 - Consider a galvanic cell based on the following...Ch. 17 - Consider a galvanic cell based on the following...Ch. 17 - An electrochemical cell consists of a silver metal...Ch. 17 - An aqueous solution of PdCl2 is electrolyzed for...Ch. 17 - Balance the following equations by the...Ch. 17 - Combine the equations to derive an expression for...Ch. 17 - The overall reaction in the lead storage battery...Ch. 17 - Consider the following galvanic cell: Calculate...Ch. 17 - A zinc-copper battery is constructed at follows at...Ch. 17 - A galvanic cell is based on the following...Ch. 17 - Consider a cell based on the following...Ch. 17 - The measurement of pH using a glass electrode...Ch. 17 - You have a concentration cell with Cu electrodes...Ch. 17 - A galvanic cell is based on the following...Ch. 17 - Given the following two standard reduction...Ch. 17 - Consider the following galvanic cell: Calculate...Ch. 17 - A chemist wishes to determine the concentration of...Ch. 17 - Consider the following galvanic cell: A 15 0-mole...Ch. 17 - When copper reacts with nitric acid, a mixture of...Ch. 17 - The following standard reduction potentials have...Ch. 17 - An electrochemical cell is set up using the...Ch. 17 - Three electrochemical cells were connected in...Ch. 17 - A silver concentration cell is set up at 25C as...Ch. 17 - A galvanic cell is based on the following...Ch. 17 - The table below lists the cell potentials for the...

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