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A.2. Table of Electrode Potentials In Table A.1, you should have a value for Eed or Exid for each of the electrode systems you have studied. Remembering that for any electrode system, Ed=-Exid, you can find the value for Ed for each system. List those potentials in the left column of the table below, in order of decreasing (more negative) value. EO reduction (Eº Ag+,Ag = 0.00 V) Electrode reaction in reduction (Eº E reduction H.H₂ = 0.00 V) The electrode potentials you have determined are based on setting E = 0.00 V. The usual convention in Agt.Ag electrochemistry is to set EH¹,H₂ = 0.00 volts, under which conditions E "Ag, Ag red = +0.80 V. Convert from one base to the other by adding 0.80 volts to each of the electrode potentials in the first column, and enter these values in the third column of the table. Why are the values of Ed on the two bases related to each other in such a simple way?

A.2. Table of Electrode Potentials In Table A.1, you should have a value for Eed or Exid for each of the electrode systems you have studied. Remembering that for any electrode system, Ed=-Exid, you can find the value for Ed for each system. List those potentials in the left column of the table below, in order of decreasing (more negative) value. EO reduction (Eº Ag+,Ag = 0.00 V) Electrode reaction in reduction (Eº E reduction H.H₂ = 0.00 V) The electrode potentials you have determined are based on setting E = 0.00 V. The usual convention in Agt.Ag electrochemistry is to set EH¹,H₂ = 0.00 volts, under which conditions E "Ag, Ag red = +0.80 V. Convert from one base to the other by adding 0.80 volts to each of the electrode potentials in the first column, and enter these values in the third column of the table. Why are the values of Ed on the two bases related to each other in such a simple way?

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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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 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 Cl- (aq) -> Cl₂ (g, 1 atm) Eº Reduction Eº Oxida Reaction tion (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 0.538 -> 1- (aq) 0.843 Br2 (1) + e -> Br- (aq) Br2 (1) –> Br- (aq) + e Reduction (M) -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 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 Cl- (aq) -> Cl₂ (g, 1 atm) Eº Reduction Eº Oxida Reaction tion (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 0.538 -> 1- (aq) 0.843 Br2 (1) + e -> Br- (aq) Br2 (1) –> Br- (aq) + e Reduction (M) -0.425 -0.843 0.00 0.00 -0.225 -0.435 -0.435
264 Experiment 32 Voltaic Cell Measurements A.2. Table of Electrode Potentials In Table A.1, you should have a value for Ed or Exid for each of the electrode systems you have studied. Remembering that for any electrode system, Ered =-E0 Eoxid, you can find the value for Ered for each system. List those potentials in the left column of the table below, in order of decreasing (more negative) value. Ereduction Ag+,Ag = 0.00 V) Electrode reaction in reduction (Eº = Ereduction H+,H₂ = 0.00 V) The electrode potentials you have determined are based on setting Egt.Ag 0.00 V. The usual convention in electrochemistry is to set EH¹,H₂ = 0.00 volts, under which conditions E Ag+,Ag red = +0.80 V. Convert from one base to the other by adding 0.80 volts to each of the electrode potentials in the first column, and enter these values in the third column of the table. Why are the values of Ed on the two bases related to each other in such a simple way?
Transcribed Image Text:264 Experiment 32 Voltaic Cell Measurements A.2. Table of Electrode Potentials In Table A.1, you should have a value for Ed or Exid for each of the electrode systems you have studied. Remembering that for any electrode system, Ered =-E0 Eoxid, you can find the value for Ered for each system. List those potentials in the left column of the table below, in order of decreasing (more negative) value. Ereduction Ag+,Ag = 0.00 V) Electrode reaction in reduction (Eº = Ereduction H+,H₂ = 0.00 V) The electrode potentials you have determined are based on setting Egt.Ag 0.00 V. The usual convention in electrochemistry is to set EH¹,H₂ = 0.00 volts, under which conditions E Ag+,Ag red = +0.80 V. Convert from one base to the other by adding 0.80 volts to each of the electrode potentials in the first column, and enter these values in the third column of the table. Why are the values of Ed on the two bases related to each other in such a simple way?
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