d. When the Sn-/Sn half-cell is paired with Cd/Cd, a cell potential of 0.267 V is measured. In addition, tin metal is seen to precipitate out of solution. Calculate the reduction potential of Cd* (aq) + 2 e • Cd(s) under the Hg standard and from the SHE standard. 7 Cd* (aq) + 2 e • Cd(s) V (Hg Standard) Cd (aq) + 2 e e Cd(s) V (SHE Standard)

d. When the Sn-/Sn half-cell is paired with Cd/Cd, a cell potential of 0.267 V is measured. In addition, tin metal is seen to precipitate out of solution. Calculate the reduction potential of Cd* (aq) + 2 e • Cd(s) under the Hg standard and from the SHE standard. 7 Cd* (aq) + 2 e • Cd(s) V (Hg Standard) Cd (aq) + 2 e e Cd(s) V (SHE Standard)

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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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

d. When the Sn-2/Sn half-cell is paired with Cd/Cd, a cell potential of 0.267 V is measured. In
addition, tin metal is seen to precipitate out of solution.
Calculate the reduction potential of Cd (aq) + 2 e ® Cd(s) under the Hg standard and from
the SHE standard.
7
Cd-2 (aq) + 2 e ® cd(s)
V (Hg Standard)
Cd (aq) + 2 e
Cd(s)
V (SHE Standard)

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