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TABLE OF ELECTRODE POTENTIALS Eº Reduction (EºAg+,Ag = Electrode Reaction in 0.00 V) Reduction Eº Reduction (EºH¹,H2 = 0.00 V)

TABLE OF ELECTRODE POTENTIALS Eº Reduction (EºAg+,Ag = Electrode Reaction in 0.00 V) Reduction Eº Reduction (EºH¹,H2 = 0.00 V)

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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Please fill in the columns in table 2, given the answers in table 1. Please point out any errors in table 1

Givens: Potential for any half reaction involving silver is 0.00 V

CELL POTENTIAL Electrode system used in cell Zn (s) | Zn²+ (aq) || Cu²+ (aq) | Cu (s) Zn (s) | Zn²+ (aq) || Fe³+ (aq)| Fe2+ (s) | graphite Cu (s) | Cu²+ (aq) || Ag+ (aq) | Ag (s) Zn (s) | Zn²+ (aq) || Ag+ (aq) | Ag (s) Zn (s) | Zn²+ (aq) || 12 (s) | 1- (aq) | graphite Fe2+ (s) | Fe3+ (aq) || Br₂ (1) | Br- (aq) | graphite CI- (aq) | Cl₂ (g, 1 atm) || | Br2 (1) | Br- (aq) | graphite Cell Negative Potential (V) Electrode 0.825 Zn 0.407 Zn 0.413 Cu 1.250 Zn 1.025 Zn 0.408 Fe 0.103 CI TABLE OF ELECTRODE POTENTIALS Eo Reduction (EºAg+,Ag = 0.00 V) Electrode Reaction in Reduction Oxidation Reaction Zn (s)-> Zn²+ + 2e Zn (s)-> Zn²+ + 2e Cu (s)-> Cu²+ (aq) + 2e Zn (s)-> Zn²+ + 2e Zn (s)-> Zn²+ + 2e Fe2+ (s)-> Fe³+ + e CI- (aq) -> Cl₂ (g, 1 atm) Reduction Eº Eº Oxida Reaction Reduction tion (M) M 1.25 Cu²+ (aq) + 2e -> Cu (s) 1.25 Fe³+ (aq) -> Fe²+ (s) 0.413 Ag+ (aq) + e > Ag (s) 1.25 Ag+ (aq) + e -> Ag (s) 1.25 12 (s) + e 0.843 Br2 (1) + e -> Br- (aq) 0.538 -> 1- (aq) Eº Reduction (EºH¹,H₂ = 0.00 V) Br2 (1) -> Br- (aq) + e -0.425 -0.843 0.00 0.00 -0.225 -0.435 -0.435
Transcribed Image Text:CELL POTENTIAL Electrode system used in cell Zn (s) | Zn²+ (aq) || Cu²+ (aq) | Cu (s) Zn (s) | Zn²+ (aq) || Fe³+ (aq)| Fe2+ (s) | graphite Cu (s) | Cu²+ (aq) || Ag+ (aq) | Ag (s) Zn (s) | Zn²+ (aq) || Ag+ (aq) | Ag (s) Zn (s) | Zn²+ (aq) || 12 (s) | 1- (aq) | graphite Fe2+ (s) | Fe3+ (aq) || Br₂ (1) | Br- (aq) | graphite CI- (aq) | Cl₂ (g, 1 atm) || | Br2 (1) | Br- (aq) | graphite Cell Negative Potential (V) Electrode 0.825 Zn 0.407 Zn 0.413 Cu 1.250 Zn 1.025 Zn 0.408 Fe 0.103 CI TABLE OF ELECTRODE POTENTIALS Eo Reduction (EºAg+,Ag = 0.00 V) Electrode Reaction in Reduction Oxidation Reaction Zn (s)-> Zn²+ + 2e Zn (s)-> Zn²+ + 2e Cu (s)-> Cu²+ (aq) + 2e Zn (s)-> Zn²+ + 2e Zn (s)-> Zn²+ + 2e Fe2+ (s)-> Fe³+ + e CI- (aq) -> Cl₂ (g, 1 atm) Reduction Eº Eº Oxida Reaction Reduction tion (M) M 1.25 Cu²+ (aq) + 2e -> Cu (s) 1.25 Fe³+ (aq) -> Fe²+ (s) 0.413 Ag+ (aq) + e > Ag (s) 1.25 Ag+ (aq) + e -> Ag (s) 1.25 12 (s) + e 0.843 Br2 (1) + e -> Br- (aq) 0.538 -> 1- (aq) Eº Reduction (EºH¹,H₂ = 0.00 V) Br2 (1) -> Br- (aq) + e -0.425 -0.843 0.00 0.00 -0.225 -0.435 -0.435
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