3. Write the equation for the oxidation of water, 4. Write the equation for the reduction of water. 5. Calculate the mass of zinc that will be deposited if a current of 0.40 Amps is applied for 25 minutes to a ZnSO4 solution.

3. Write the equation for the oxidation of water, 4. Write the equation for the reduction of water. 5. Calculate the mass of zinc that will be deposited if a current of 0.40 Amps is applied for 25 minutes to a ZnSO4 solution.

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 100E: A factory wants to produce 1.00 103 kg barium from the electrolysis of molten barium chloride. What...

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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

3. Write the equation for the oxidation of water,
4. Write the equation for the reduction of water.
5. Calculate the mass of zinc that will be deposited if a current of 0.40 Amps is applied for 25 minutes to a
ZnSO4 solution.

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Step 1: Define oxidation

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Step 2: Balance the number of O atoms in oxidation reaction of water

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Step 3: Balance the number of H atoms in oxidation reaction of water

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Step 4: Balance the charge

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