1) The standard reduction potentials of Cu2+ (aq) Cu(s) and Ag+ (aq) Ag(s) are +0.34 and +0.80 V, respectively. Determine the value of the actual cell potential, Ecell, (in V) for the following cell at 25.0 °C. Cu(s) Cu²+ (0.250 M)||Ag (0.0010 M)|Ag(s) Hint: First calculate Eº, then apply the solution concentrations of the galvanic cell using the Nernst equation. A) +0.30 V B) +0.39 V C) +0.14 V D) +0.78 V E) +0.62 V

1) The standard reduction potentials of Cu2+ (aq) Cu(s) and Ag+ (aq) Ag(s) are +0.34 and +0.80 V, respectively. Determine the value of the actual cell potential, Ecell, (in V) for the following cell at 25.0 °C. Cu(s) Cu²+ (0.250 M)||Ag (0.0010 M)|Ag(s) Hint: First calculate Eº, then apply the solution concentrations of the galvanic cell using the Nernst equation. A) +0.30 V B) +0.39 V C) +0.14 V D) +0.78 V E) +0.62 V

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

1) The standard reduction potentials of Cu²+ (aq) Cu(s) and Agt (aq) Ag(s) are +0.34 and +0.80 V,
respectively. Determine the value of the actual cell potential, Ecell, (in V) for the following cell at
25.0 °C.
Cu(s) Cu²+ (0.250 M)||Ag (0.0010 M)|Ag(s)
Hint: First calculate Eº, then apply the solution concentrations of the galvanic cell using the
Nernst equation.
payila
A) +0.30 V
B) +0.39 V
C) +0.14 V
D) +0.78 V
-E) +0.62 V

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