20.51 Given the following reduction half-reactions: Fe (aq) + e Fe2 (aq) Eed = +0.77 V S,02 (aq) + 4H (aq) + 2e 2 H,SO,(aq) Eed= +0.60 V N20(g) +2H (aq) + 2e N2(8) + H2O(1) Eed=-1.77 V %3D VOo (aq) +2 H (aq) + e VO2 + H,O(I) Eed +1.00 V (a) Write balanced chemical equations for the oxidation of Fe2 (aq) by S,0 (aq), by N20(aq), and by VO2(aq). (b) Calculate AG for each reaction at 298 K. (c) Calculate the equilibrium constant K for each reaction at 298 K.
20.51 Given the following reduction half-reactions: Fe (aq) + e Fe2 (aq) Eed = +0.77 V S,02 (aq) + 4H (aq) + 2e 2 H,SO,(aq) Eed= +0.60 V N20(g) +2H (aq) + 2e N2(8) + H2O(1) Eed=-1.77 V %3D VOo (aq) +2 H (aq) + e VO2 + H,O(I) Eed +1.00 V (a) Write balanced chemical equations for the oxidation of Fe2 (aq) by S,0 (aq), by N20(aq), and by VO2(aq). (b) Calculate AG for each reaction at 298 K. (c) Calculate the equilibrium constant K for each reaction 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
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 88E: For the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1,...
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Transcribed Image Text:20.51 Given the following reduction half-reactions:
Fe (aq) + e
Fe (aq) Eed = +0.77 V
S,02 (aq) +4H (aq) + 2e 2 H,SO,(aq) Eed= +0.60 V
N20(g) +2H (ag) + 2e N2(8) + H2O(1) Eed
= -1.77 V
VO (aq) + 2 H"(aq) + e-
VO2+ H,O(I) Eed = +1.00 V
(a) Write balanced chemical equations for the oxidation
of Fe2 (aq) by S,0, (aq), by N20(aq), and by VO;(aq).
(b) Calculate AG for each reaction at 298 K. (c) Calculate
the equilibrium constant K for each reaction at 298 K.
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