A current of 200 A flows for 22.0 hours at an anode where the reaction occurring is Mn2*(aq) + 2H20(1) → Mn02(s) + 4H*(aq) + 2e¯ What mass (in kg) of MnOz is deposited on this anode?

A current of 200 A flows for 22.0 hours at an anode where the reaction occurring is Mn2(aq) + 2H20(1) → Mn02(s) + 4H(aq) + 2e¯ What mass (in kg) of MnOz is deposited on this anode?

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 128AE: It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing...

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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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A current of 200 A flows for 22.0 hours at an anode where the reaction occurring is
Mn2+(aq) + 2H20(1) → Mn02(s) + 4H*(aq) + 2e-
What mass (in kg) of MnO, is deposited on this anode?

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