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MnO, (aq) + 2H,0 + 3e MnO,(s) + 40H'(aq) a MnO4 + 5Fe2+ Mn2+ + 5F (acidic solution) 3+ E° cell V AG° = kJ/mol

MnO, (aq) + 2H,0 + 3e MnO,(s) + 40H'(aq) a MnO4 + 5Fe2+ Mn2+ + 5F (acidic solution) 3+ E° cell V AG° = kJ/mol

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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Calculate E° cell from the tabulated standard reduction potentials for each of the following reactions in aqueous solution. Then calculate AG° and K at 25°C from E° cell 4. F = 9.65 x 10 J/V•mol e R = 8.314 J/mol•K Acidic solution Standard reduction potential, E° (Volts) Cu2" (aq) + e Cu (aq) Cu'(aq) + e- MnO, (aq) 8H (aq) + 5e Mn2 (aq) + 4H,O Fe" (aq) + e Fe"(aq) 0.153 Cu(s) 0.521 1.507 0.771 Basic solution -1.22 Zn(OH),(s) + 2e Zn(s) + 40H(aq) MnO, (aq) + 2H,O + 3e MnO,(s) + 40H (aq) 0.588 a MnO4 + 5Fe-t Mn2 + 5Fe (acidic solution) E° cell V AG° = kJ/mol K = Previous Next
Transcribed Image Text:Calculate E° cell from the tabulated standard reduction potentials for each of the following reactions in aqueous solution. Then calculate AG° and K at 25°C from E° cell 4. F = 9.65 x 10 J/V•mol e R = 8.314 J/mol•K Acidic solution Standard reduction potential, E° (Volts) Cu2" (aq) + e Cu (aq) Cu'(aq) + e- MnO, (aq) 8H (aq) + 5e Mn2 (aq) + 4H,O Fe" (aq) + e Fe"(aq) 0.153 Cu(s) 0.521 1.507 0.771 Basic solution -1.22 Zn(OH),(s) + 2e Zn(s) + 40H(aq) MnO, (aq) + 2H,O + 3e MnO,(s) + 40H (aq) 0.588 a MnO4 + 5Fe-t Mn2 + 5Fe (acidic solution) E° cell V AG° = kJ/mol K = Previous Next
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