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Given the following reduction half-reactions: Fe+ (aq) + e": S2O6² (aq) + 4H* (aq) + 2e¯ → 2 H2SO3 (aq) N¿O (g) + 2H* (aq) + 2e → N2 (9) + H2O (1) VO2* (aq) + 2H+ (aq) + e¯ → VO²+ (aq) + H2O (1) Fe2+ (aq) E°red = +0.77V E°red = +0.60 V E°red = -1.77 V E°red = +1.00 V %3D %3D Write balanced equations for the oxidation of Fe2*(aq) by: a. S20² (aq) b. N2O (g) c. VO2* (aq)

Given the following reduction half-reactions: Fe+ (aq) + e": S2O6² (aq) + 4H* (aq) + 2e¯ → 2 H2SO3 (aq) N¿O (g) + 2H* (aq) + 2e → N2 (9) + H2O (1) VO2* (aq) + 2H+ (aq) + e¯ → VO²+ (aq) + H2O (1) Fe2+ (aq) E°red = +0.77V E°red = +0.60 V E°red = -1.77 V E°red = +1.00 V %3D %3D Write balanced equations for the oxidation of Fe2*(aq) by: a. S20² (aq) b. N2O (g) c. VO2* (aq)

Chemistry
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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Given the following reduction half-reactions: Fe+ (aq) + e° → Fe2+ (aq) E°red = +0.77 V S2062- (aq) + 4H* (aq) + 2e¯ → 2 H;SO3 (aq) N2O (g) + 2H* (aq) + 2e VO2* (aq) + 2H* (aq) + e¯ → VO²+ (aq) + H2O (1) E°red = +0.60 V E°red = -1.77 V E°red = +1.00 V N2 (9) + H2O (1) Write balanced equations for the oxidation of Fe2*(aq) by: a. S206 (aq) b. N2O (g) c. VO2* (aq)
Transcribed Image Text:Given the following reduction half-reactions: Fe+ (aq) + e° → Fe2+ (aq) E°red = +0.77 V S2062- (aq) + 4H* (aq) + 2e¯ → 2 H;SO3 (aq) N2O (g) + 2H* (aq) + 2e VO2* (aq) + 2H* (aq) + e¯ → VO²+ (aq) + H2O (1) E°red = +0.60 V E°red = -1.77 V E°red = +1.00 V N2 (9) + H2O (1) Write balanced equations for the oxidation of Fe2*(aq) by: a. S206 (aq) b. N2O (g) c. VO2* (aq)
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