Given the following reduction half reactions (a) Write balanced chemical equations for the oxidation of Fe2 (aq) by S2O62 (aq), by N2O(aq), and by VO2 (aq) (b) Calculate Icirc G deg for each reaction at 298 K (c) Calculate the equilibrium constant K for each reaction at 298 K 3 Fe2 ( e Ered 0 77 V Ered 0 60 V Ered 1 77 V Ered 1 00 V N20(g 2 H (a) 2eN2g) H,00) VO2 (aq) 2H (aq) e VO2 H20(1)

Question: Given the following reduction half-reactions: (a) Write balanced chemical equations for the oxidation of Fe2+(aq) by S2O62- (aq), by N2O(aq), and by VO2+(aq). (b) Calculate

Given the following reduction half-reactions:

(a) Write balanced chemical equations for the oxidation of Fe2+(aq) by S2O62- (aq), by N2O(aq), and by VO2+(aq).
(b) Calculate Î”G° for each reaction at 298 K.
(c) Calculate the equilibrium constant K for each reaction at 298 K.

3+ Fe2+ ( e Ered = +0.77 V Ered = +0.60 V Ered =-1.77 V Ered = +1.00 V N20(g 2 H (a) 2eN2g) +H,00) VO2+ (aq) + 2H+ (aq) + e- VO2+ + H20(1)

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