please i need short and simple answer Given the following reduction half-reactions:Fe³+ (aq) + eS₂062 (aq) + 4H+ (aq) + 2 e¯-N₂O(g) + 2 H+ (aq) + 2 eVO₂ (aq) + 2 H+ (aq) + e-Fe2+ (aq) Ered= +0.77 V2 H₂SO3(aq) Ered = +0.60 VN2(g) + H₂O(1) Ered = -1.77 VVO2+ + H₂O(1) Ered = +1.00 V(a) Write balanced chemical equations for the oxidationof Fe2+ (aq) by S₂0 (aq), by N₂O(aq), and by VO₂ (aq).(b) Calculate AG for each reaction at 298 K. (c) Calculatethe equilibrium constant K for each reaction at 298 K.---Y

Balanced equations for oxidation of .

Given the following reduction half-reactions: Fe³+ (aq) + e- Fe2+ (aq) Ered S₂0 (aq) + 4H*(aq) + 2 e N₂O(g) + 2 H+ (aq) + 2 e 2 H₂SO3(aq) Ered = +0.60 V N2(8) + H₂O(1) Ered=-1.77 V VO2+ + H₂O(1) Ered = +1.00 V VO₂ (aq) + 2 H+ (aq) + e- (a) Write balanced chemical equations for the oxidation of Fe2+ (aq) by S₂0 (aq), by N₂O(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. - - = +0.77 V 1

Given the following reduction half-reactions: Fe³+ (aq) + e- Fe2+ (aq) Ered S₂0 (aq) + 4H*(aq) + 2 e N₂O(g) + 2 H+ (aq) + 2 e 2 H₂SO3(aq) Ered = +0.60 V N2(8) + H₂O(1) Ered=-1.77 V VO2+ + H₂O(1) Ered = +1.00 V VO₂ (aq) + 2 H+ (aq) + e- (a) Write balanced chemical equations for the oxidation of Fe2+ (aq) by S₂0 (aq), by N₂O(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. - - = +0.77 V 1

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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