Which of the following is true for the voltaic cell utilizing, Ni(s), Ni²*(aq), Ag(s), and Ag+(aq). Ag*(aq) + e-Ag(s) EO = 0.7996 V Ni2*(au) + 2e= Ni(s) EO = -0.257 V %3D If the [Ni2] used is less than 1.0 M the nonstandard cell potential would be less than the standard value. The Ecell value at 35°C for this cell when [Ag*] = 3.5x10-3M and [Ni2+] = 8.6x10-4 %3D M would be 1.04 V. The AGO at 25°C would be -198 kJ. The anode half-reaction would convert Ag" ions to Ag(s). A Moving to another question will save this response. MooRook Pro

Which of the following is true for the voltaic cell utilizing, Ni(s), Ni²(aq), Ag(s), and Ag+(aq). Ag(aq) + e-Ag(s) EO = 0.7996 V Ni2(au) + 2e= Ni(s) EO = -0.257 V %3D If the [Ni2] used is less than 1.0 M the nonstandard cell potential would be less than the standard value. The Ecell value at 35°C for this cell when [Ag] = 3.5x10-3M and [Ni2+] = 8.6x10-4 %3D M would be 1.04 V. The AGO at 25°C would be -198 kJ. The anode half-reaction would convert Ag" ions to Ag(s). A Moving to another question will save this response. MooRook Pro

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

Problem 77AP

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Question

Which of the following is true for the voltaic cell utilizing, Ni(s), Ni<*(aq), Ag(s), and Ag+(aq).
Ag (aq) + e-Ag(s) EO = 0.7996 V
Ni2*(aq) + 2e= Ni(s) EO = -0.257 V
If the [Ni] used is less than 1.0 M the nonstandard cell potential would be less than the standard value.
The Ecell value at 35°C for this cell when [Ag*] = 3.5x10-3M and [Ni2+] = 8.6x10-4
M would be 1.04 V.
The AGO at 25°C would be -198 kJ.
The anode half-reaction would convert Ag" ions to Ag(s).
Moving to another question will save this response.
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