Suppose a metal electrode is being coated with silver according to the half-reaction, Ag+(aq) + e- -> Ag(s), If a current of 0.850 A flows through the cell for 20.00 min, how many moles of Ag(s) are deposited? Use 9.65 x 104 C/(mol e-) for the Faraday constant, F. moles Ag(s)

Suppose a metal electrode is being coated with silver according to the half-reaction, Ag+(aq) + e- -> Ag(s), If a current of 0.850 A flows through the cell for 20.00 min, how many moles of Ag(s) are deposited? Use 9.65 x 104 C/(mol e-) for the Faraday constant, F. moles Ag(s)

Chemistry

10th Edition

ISBN:9781305957404

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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.

Question

Suppose a metal electrode is being coated with silver according to the half-reaction, Ag*(aq) + e- -> Ag(s), If a current of
0.850 A flows through the cell for 20.0 min, how many moles of Ag(s) are deposited? Use 9.65 x 104 C/(mol e-) for the
Faraday constant, F.
moles Ag(s)

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