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A solution containing 0.100 M AuCl4 and 0.100 M CI is subjected to a continuous current of 6.00 A to deposit Au(s) in one electrode and Cl₂ gas on the other electrode. The reaction involved is : 3Cl¯ (aq) + AuCl4 (aq) →1.5 Cl2(g) + Au(s) + 4Cl¯( (aq). Given F= 96,500 C/mol e (or 96,500 J/V-mol e) and the standard reduction potential values: Cl₂ + 2e → 2Cl¯ AuCl₂ + 3e → Au +4Cl¯ a. Write the oxidation half reaction. b. Write the reduction half-reaction. Write the shorthand cell notation. Eᵒred_(V). 1.360 1.000 C. d. Calculate the standard cell potential involved. e. Calculate the mass, in grams, of Au (At. mass= 197) that is deposited in one of the electrodes after passing the 6.00 A current for 245 seconds.

A solution containing 0.100 M AuCl4 and 0.100 M CI is subjected to a continuous current of 6.00 A to deposit Au(s) in one electrode and Cl₂ gas on the other electrode. The reaction involved is : 3Cl¯ (aq) + AuCl4 (aq) →1.5 Cl2(g) + Au(s) + 4Cl¯( (aq). Given F= 96,500 C/mol e (or 96,500 J/V-mol e) and the standard reduction potential values: Cl₂ + 2e → 2Cl¯ AuCl₂ + 3e → Au +4Cl¯ a. Write the oxidation half reaction. b. Write the reduction half-reaction. Write the shorthand cell notation. Eᵒred_(V). 1.360 1.000 C. d. Calculate the standard cell potential involved. e. Calculate the mass, in grams, of Au (At. mass= 197) that is deposited in one of the electrodes after passing the 6.00 A current for 245 seconds.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A solution containing 0.100 M AuCl4 and 0.100 M CI is subjected to a continuous current of 6.00 A to deposit Au(s) in one electrode and Cl₂ gas on the other electrode. The reaction involved is : 3CI (aq) + AuCl4 (aq) →1.5 Cl2(g) + Au(s) + 4Cl¯(aq). Given F= 96,500 C/mol e (or 96,500 J/V-mol e) and the standard reduction potential values: Cl₂ + 2e2Cl¯ AuCl4 + 3e → Au + 4Cl¯ a. b. C. Write the oxidation half reaction. Write the reduction half-reaction. Write the shorthand cell notation. Eᵒred_(V) 1.360 1.000 d. Calculate the standard cell potential involved. e. Calculate the mass, in grams, of Au (At. mass= 197) that is deposited in one of the electrodes after passing the 6.00 A current for 245 seconds.
Transcribed Image Text:A solution containing 0.100 M AuCl4 and 0.100 M CI is subjected to a continuous current of 6.00 A to deposit Au(s) in one electrode and Cl₂ gas on the other electrode. The reaction involved is : 3CI (aq) + AuCl4 (aq) →1.5 Cl2(g) + Au(s) + 4Cl¯(aq). Given F= 96,500 C/mol e (or 96,500 J/V-mol e) and the standard reduction potential values: Cl₂ + 2e2Cl¯ AuCl4 + 3e → Au + 4Cl¯ a. b. C. Write the oxidation half reaction. Write the reduction half-reaction. Write the shorthand cell notation. Eᵒred_(V) 1.360 1.000 d. Calculate the standard cell potential involved. e. Calculate the mass, in grams, of Au (At. mass= 197) that is deposited in one of the electrodes after passing the 6.00 A current for 245 seconds.
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