Given the following reduction half-reactions: Fe*(ag) + e → Fe2* (aq) Eed = +0.77 V S202- (ag) + 4 H*(aq) + 2 e → 2 H2SO3(aq) Ered = +0.60 V N20(8) + 2H*(aq) + 2 e¯ → N2(8) + H;0(I) Eed –1.77 V voj(aq) + 2H*(aq) + e- → VO2+ + H,0(I) Ered = +1.00V (a) Write balanced chemical equations for the oxidation of Fe2"(aq) by S20? (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.

Given the following reduction half-reactions: Fe(ag) + e → Fe2 (aq) Eed = +0.77 V S202- (ag) + 4 H(aq) + 2 e → 2 H2SO3(aq) Ered = +0.60 V N20(8) + 2H(aq) + 2 e¯ → N2(8) + H;0(I) Eed –1.77 V voj(aq) + 2H(aq) + e- → VO2+ + H,0(I) Ered = +1.00V (a) Write balanced chemical equations for the oxidation of Fe2"(aq) by S20? (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.

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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