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2 a) Write the half-reaction for a hydrogen electrode in acidic solution when it is serving as the cathode of a voltaic cell. Define what is meant by the standard hydrogen electrode. What role does platinum play? b) For the half cells: Fe3+ + e-> Fe2+ E° = 0.77 V Cu2+ + 2e-> Cu E = 0.34 V Write the equation describing the reaction of an electrochemical cell comprised of the two half cells and calculate AG° for the cell. c)The standard reduction potentials for the following reactions are: 0.80 V Ag*(aq) + e- > Ag(s)

2 a) Write the half-reaction for a hydrogen electrode in acidic solution when it is serving as the cathode of a voltaic cell. Define what is meant by the standard hydrogen electrode. What role does platinum play? b) For the half cells: Fe3+ + e-> Fe2+ E° = 0.77 V Cu2+ + 2e-> Cu E = 0.34 V Write the equation describing the reaction of an electrochemical cell comprised of the two half cells and calculate AG° for the cell. c)The standard reduction potentials for the following reactions are: 0.80 V Ag*(aq) + e- > Ag(s)

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
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ka) Write the half-reaction for a hydrogen electrode in acidic solution when it is serving as the cathode of a voltaic cell. Define what is meant by the standard hydrogen electrode. What role does platinum play? b) For the half cells: Fe3+ + e-> Fe2+ E° = 0.77 V Cu2+ + 2e-→ Cu E = 0.34 V Write the equation describing the reaction of an electrochemical cell comprised of the two half cells and calculate AG° for the cell. c)The standard reduction potentials for the following reactions are: Ag*(aq) + e- > Ag(s) Cu2"(aq) + 2e- > Cu(s) Ni*(ag) + 2e- > Ni(s) Zn*(ag) + 2e- > Zn(s) 0.80 V 0.34 V - 0.28 V - 0.76 V Which combinations of these half-cell reactions yield the cells with the highest and lowest cell potentials?
Transcribed Image Text:ka) Write the half-reaction for a hydrogen electrode in acidic solution when it is serving as the cathode of a voltaic cell. Define what is meant by the standard hydrogen electrode. What role does platinum play? b) For the half cells: Fe3+ + e-> Fe2+ E° = 0.77 V Cu2+ + 2e-→ Cu E = 0.34 V Write the equation describing the reaction of an electrochemical cell comprised of the two half cells and calculate AG° for the cell. c)The standard reduction potentials for the following reactions are: Ag*(aq) + e- > Ag(s) Cu2"(aq) + 2e- > Cu(s) Ni*(ag) + 2e- > Ni(s) Zn*(ag) + 2e- > Zn(s) 0.80 V 0.34 V - 0.28 V - 0.76 V Which combinations of these half-cell reactions yield the cells with the highest and lowest cell potentials?
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