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
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdbf5906e-cfef-4138-bd85-fe9745156c72%2Fe0149ad6-8ef7-4123-9c73-718a741e7462%2Fxsmwif7_processed.png&w=3840&q=75)
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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