The reaction in the Daniell cell is Cu2+ + Zn → Cu + Zn2+. (a) Given the following standard electrode potentials: Eo298K (Zn | Zn2+) = − 0.763 V; Eo298K (Cu | Cu2+) = + 0.337 V, calculate ΔGo for the cell reaction at 298 K. [−212.3] (b) If for the temperature coefficient of the cell potential, (?Eo / ?T)P is −1.08 x 10−4 V K−1, calculate ΔSo and ΔHo for the cell reaction at 298 K. [−212.3; −20.8; −218.5] The answers are in the bracket, I would like to know how they were obtained. Thank you!
The reaction in the Daniell cell is Cu2+ + Zn → Cu + Zn2+. (a) Given the following standard electrode potentials: Eo298K (Zn | Zn2+) = − 0.763 V; Eo298K (Cu | Cu2+) = + 0.337 V, calculate ΔGo for the cell reaction at 298 K. [−212.3] (b) If for the temperature coefficient of the cell potential, (?Eo / ?T)P is −1.08 x 10−4 V K−1, calculate ΔSo and ΔHo for the cell reaction at 298 K. [−212.3; −20.8; −218.5] The answers are in the bracket, I would like to know how they were obtained. Thank you!
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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The reaction in the Daniell cell is Cu2+ + Zn → Cu + Zn2+.
(a) Given the following standard electrode potentials:
Eo298K (Zn | Zn2+) = − 0.763 V;
Eo298K (Cu | Cu2+) = + 0.337 V,
calculate ΔGo for the cell reaction at 298 K. [−212.3]
(b) If for the temperature coefficient of the cell potential, (?Eo / ?T)P is −1.08 x 10−4 V K−1,
calculate ΔSo and ΔHo for the cell reaction at 298 K.
[−212.3; −20.8; −218.5]
The answers are in the bracket, I would like to know how they were obtained. Thank you!
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