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Write the overall chemical reaction and calculate E° for the following reduction and oxidation half-reactions. 2H (aq) + 2e→ H2(g) E° = 0.00 V red Fe(s) → Fe2"(aq) + 2e E° +0.44 V %3D O Fe2 (aq) + H2(g) →Fe(s) + 2H*(aq) E° =+0.44 V O Fe(s) +2H"(ag) →F22*(aq) + H2(g) E° = -0.44 V O Fe2"(aq) + H2(g) →Fe(s) + 2H*(aq) E° = -0.44 V O Fe(s) +2H (aq) →FE2*(aq) + H2(g) E° =+0.44 V %3D

Write the overall chemical reaction and calculate E° for the following reduction and oxidation half-reactions. 2H (aq) + 2e→ H2(g) E° = 0.00 V red Fe(s) → Fe2"(aq) + 2e E° +0.44 V %3D O Fe2 (aq) + H2(g) →Fe(s) + 2H*(aq) E° =+0.44 V O Fe(s) +2H"(ag) →F22*(aq) + H2(g) E° = -0.44 V O Fe2"(aq) + H2(g) →Fe(s) + 2H*(aq) E° = -0.44 V O Fe(s) +2H (aq) →FE2*(aq) + H2(g) E° =+0.44 V %3D

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.95QE
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Write the overall chemical reaction and calculate E° for the following reduction and oxidation half-reactions. 2H (aq) + 2e H2(g) E° red = 0.00 V Fe(s) → Fe2"(aq) + 2e E° =+0.44 V OFF2 (aq) + H2(g) →Fe(s) + 2H"(aq) E° = +0.44 V O Fe(s) + 2H"(aq)→FE2*(aq) + H2(g) E° = -0.44 V OFE2"(ag) + H2(g)→Fe(s) + 2H*(aq) E° = -0.44 V O Fe(s) +2H"(aq)→FE2"(aq) + H2(g) E° =+0.44 V
Transcribed Image Text:Write the overall chemical reaction and calculate E° for the following reduction and oxidation half-reactions. 2H (aq) + 2e H2(g) E° red = 0.00 V Fe(s) → Fe2"(aq) + 2e E° =+0.44 V OFF2 (aq) + H2(g) →Fe(s) + 2H"(aq) E° = +0.44 V O Fe(s) + 2H"(aq)→FE2*(aq) + H2(g) E° = -0.44 V OFE2"(ag) + H2(g)→Fe(s) + 2H*(aq) E° = -0.44 V O Fe(s) +2H"(aq)→FE2"(aq) + H2(g) E° =+0.44 V
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