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 ?

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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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

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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

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