Electrolysis of AgF(aq) in acidic solution leads to the formation of silver metal and oxygen gas. Ag* (aq) + e"--> Ag(s) E°red = +0.799V 02 (g) + 4H* (ag) + 4e --> 2H2O(1) E°red = +1.23V What is the minimum external applied voltage required to cause this process to occur under standard conditions?

Electrolysis of AgF(aq) in acidic solution leads to the formation of silver metal and oxygen gas. Ag* (aq) + e"--> Ag(s) E°red = +0.799V 02 (g) + 4H* (ag) + 4e --> 2H2O(1) E°red = +1.23V What is the minimum external applied voltage required to cause this process to occur under standard conditions?

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.

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Electrolysis of AgF(ag) in acidic solution leads to the formation of silver metal and oxygen gas.
Ag" (ag) + e-->
AB(s)
E°red = +0.799V
02 (g) + 4H* (ag) + 4e" -->
2H2O(1)
E°red = +1.23V
What is the minimum external applied voltage required to cause this process to occur under standard
conditions?

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