Consider the electrochemical cell, Zn (s) | ZnBr2 (0.235 mol kg - 1) | Br2 (1) | C (s), for which the reaction is Br2 (1) + Zn (s) → 2 Br - (aq) + Zn 2+ (aq). Since Eo (Zn2 +, Zn) = -0.763 V, Eo (Br -, Br2) = +1.09 V a. Determine the standard potential, b. Determine the average ionic activity coefficient of ZnBr2 from the Debye-Hückel limit law. c. Determine the potential of the electrochemical cell for the given conditions at 298 K.

Consider the electrochemical cell, Zn (s) | ZnBr2 (0.235 mol kg - 1) | Br2 (1) | C (s), for which the reaction is Br2 (1) + Zn (s) → 2 Br - (aq) + Zn 2+ (aq). Since Eo (Zn2 +, Zn) = -0.763 V, Eo (Br -, Br2) = +1.09 V a. Determine the standard potential, b. Determine the average ionic activity coefficient of ZnBr2 from the Debye-Hückel limit law. c. Determine the potential of the electrochemical cell for the given conditions at 298 K.

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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Question

Consider the electrochemical cell, Zn (s) | ZNBR2 (0.235 mol kg – 1) | Br2 (1) | C (s), for which the reaction is Br2 (1) + Zn (s) → 2 Br - (aq) +
Zn 2+ (aq). Since Eo (Zn2 +, Zn) = -0.763 V, Eo (Br -, Br2) = +1.09 V
a. Determine the standard potential,
b. Determine the average ionic activity coefficient of ZnBr2 from the Debye-Hückel limit law.
c. Determine the potential of the electrochemical cell for the given conditions at 298 K.
d. ArG, ArGo, and K for the reaction,
e. Given that (ƏE / ƏT) p = 8.45 × 10–5 V K –- 1. Calculate AS and
ΔΗ.

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