For the following half-reactions, answer the following questions below E = +1.953 V Co*(aq) + e- Co*(aq) Fe*(aq) + e → • Fe²*(aq) E = +0.769 V 1(aq) + 2e" → 21~(aq) E = +0.534 V E° = -0.127 V E = -0.402 V Pb²*(aq) + 2e¯ Pb(s) > Cd?+(aq) + 2e" Cd(s) Mn** (aq) + 2е" Mn(s) E° = -1.182 V

For the following half-reactions, answer the following questions below E = +1.953 V Co(aq) + e- Co(aq) Fe(aq) + e → • Fe²(aq) E = +0.769 V 1(aq) + 2e" → 21~(aq) E = +0.534 V E° = -0.127 V E = -0.402 V Pb²*(aq) + 2e¯ Pb(s) > Cd?+(aq) + 2e" Cd(s) Mn** (aq) + 2е" Mn(s) E° = -1.182 V

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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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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g. Which ion/s can be reduced by Ph?
h. Which metal/s can be oxidized by Fe*?

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