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.
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Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.124QP: An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for...
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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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