2. Refer to Table 10.1, calculate the cell voltage involving: a. Fe (s)/ Fe²+ (0.300M)// Sn²+ (0.150 M)/ Sn (s) b. Mn (s)/ Mn²+ (0.400M)// Ag+ (0.150 M)/ Ag (s) Let me show you an example for a. The cell involves the oxidation of Fe(s) and the reduction of Sn²+, the cell reaction being Fe (s) + Sn²+ → Fe²+ + Sn (s) Excell = Ecathode - Eanode = -0.136-(-0.440) = 0.304 V [Fe²+] log- = 0.304 - [Sn²+] Ecell = E cell 0.0592 2 0.0592 0.300 2 0.500 -log = 0.311 V

2. Refer to Table 10.1, calculate the cell voltage involving: a. Fe (s)/ Fe²+ (0.300M)// Sn²+ (0.150 M)/ Sn (s) b. Mn (s)/ Mn²+ (0.400M)// Ag+ (0.150 M)/ Ag (s) Let me show you an example for a. The cell involves the oxidation of Fe(s) and the reduction of Sn²+, the cell reaction being Fe (s) + Sn²+ → Fe²+ + Sn (s) Excell = Ecathode - Eanode = -0.136-(-0.440) = 0.304 V [Fe²+] log- = 0.304 - [Sn²+] Ecell = E cell 0.0592 2 0.0592 0.300 2 0.500 -log = 0.311 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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