Free Energy and Redox Reactions (Section)
Fe3+(aq) + e-→ Fe2+(aq) E°red = +0.77 V
S2O62- (aq) + 4 H+(aq) + 2 e-→ 2 H2SO3(aq) E°red = +0.60 V
N2O(g) + 2 H+(aq) + 2 e-→ N2(g) + H2O(l) E°red = -1.77 V
VO2+(aq) + 2 H+(aq) + e-.VO2+ + H2O(l) E°red = +1.00 V
(a) Write balanced chemical equations for the oxidation of Fe2+(aq) by S2O62-(aq), by N2O(aq), and by VO2+(aq). (b) Calculate ΔG° for each reaction at 298 K. (c) Calculate the equilibrium constant K for each reaction at 298 K.
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