Answered: Cr203(s) + H2O2(aq) → CrO42-(aq) +…

Cr203(s) + H2O2(aq) → CrO42-(aq) + H2O(1) Reductant half-reaction: Oxidant half-reaction: Net ionic full reaction in acid: Net ionic full reaction in base:

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter13: Electrochemistry

Section: Chapter Questions

Problem 3CO: • write and balance half-reactions for simple redox processes.

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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

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Balance by the half-reaction method, both in acid and in base

Cr2O3(s) + H2O2(aq) → CrO42-(aq) + H2O(1)
Reductant half-reaction:
Oxidant half-reaction:
Net ionic full reaction in acid:
Net ionic full reaction in base:

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