Use the equation E°cell = E°cathode E°anode to calculate the E°cell for the reaction: 2 Ag+1 + Cu - Cu*2 + 2 Ag , given the following potentials: Ag*1 + 1 e- Ag E° = +0.80 V. Cu+2 + 2e- Cu E° = +0.34 V. Enter the answer using two significant figures and not units

Use the equation E°cell = E°cathode E°anode to calculate the E°cell for the reaction: 2 Ag+1 + Cu - Cu2 + 2 Ag , given the following potentials: Ag1 + 1 e- Ag E° = +0.80 V. Cu+2 + 2e- Cu E° = +0.34 V. Enter the answer using two significant figures and not units

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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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.

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Use the equation E°cell = E°cathode E°anode to calculate the E°cell| for the reaction:
2 Ag+1 + Cu - Cu+2 + 2 Ag , given the following potentials:
Ag*1 + 1 e- → Ag
E° = +0.80 V.
Cu+2
Cut2 + 2e- → Cu
E° = +0.34 V.
Enter the answer using two significant figures and not units

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