26. Given the following electrode (reduction) potentials: Ag* + e --> Ag; E° = 0.80 V Zn2+ + 2e --> Zn; E° = -0.76 V For a Voltaic cell represented by the cell notation: Zn(s)|Zn2*(aq)||Ag*(aq)|Ag(s), what is the cell potential (Ecell) when the electrolyte concentrations are as follows: [Ag*] = 1.3 x 10-5 M, and [Zn2*] = 1.0 M ?
26. Given the following electrode (reduction) potentials: Ag* + e --> Ag; E° = 0.80 V Zn2+ + 2e --> Zn; E° = -0.76 V For a Voltaic cell represented by the cell notation: Zn(s)|Zn2*(aq)||Ag*(aq)|Ag(s), what is the cell potential (Ecell) when the electrolyte concentrations are as follows: [Ag*] = 1.3 x 10-5 M, and [Zn2*] = 1.0 M ?
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![26. Given the following electrode (reduction) potentials:
Ag* + e --> Ag;
E° = 0.80 V
Zn2+ + 2e --> Zn;
E° = -0.76 V
For a Voltaic cell represented by the cell notation: Zn(s)|Zn2*(aq)||Ag*(aq)|Ag(s),
what is the cell potential (Ecell) when the electrolyte concentrations are as follows: [Ag*] = 1.3 x
10-5 M, and [Zn2*) = 1.0 M ?
(A) 2.36 V
(B) 1.56 V
(C) 0.84 V
(D) 0.04 V](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F16f65cf9-d3bb-4ef1-8d11-46be7a9043fa%2Fbba59e83-0927-407d-8544-9bfe3b5441fd%2Ftpk0pjp_processed.png&w=3840&q=75)
Transcribed Image Text:26. Given the following electrode (reduction) potentials:
Ag* + e --> Ag;
E° = 0.80 V
Zn2+ + 2e --> Zn;
E° = -0.76 V
For a Voltaic cell represented by the cell notation: Zn(s)|Zn2*(aq)||Ag*(aq)|Ag(s),
what is the cell potential (Ecell) when the electrolyte concentrations are as follows: [Ag*] = 1.3 x
10-5 M, and [Zn2*) = 1.0 M ?
(A) 2.36 V
(B) 1.56 V
(C) 0.84 V
(D) 0.04 V
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