The cell potential for the standard galvanic cell shown above is +1.56V. If AgNO3(aq)|Ag(s) is replaced with 1M Pb(NO3)2(aq) solution and a Pb electrode, which of the following describes what happens to the operation of the cell, and why? A. Nothing changes because galvanic cells that have a Zn(s) electrode have a constant cell potential, E°cell, of +1.56V. B. The cell stops generating a voltage because the standard reduction potentials of Pb2+ and Zn2+ are both negative. C. The cell potential decreases because the reduction of Pb2+ is less thermodynamically favorable than the reduction of Ag+. D. The cell potential increases because twice as many electrons are transferred between Pb2+ and Zn than between Ag+ and Zn.
The cell potential for the standard galvanic cell shown above is +1.56V. If AgNO3(aq)|Ag(s) is replaced with 1M Pb(NO3)2(aq) solution and a Pb electrode, which of the following describes what happens to the operation of the cell, and why? A. Nothing changes because galvanic cells that have a Zn(s) electrode have a constant cell potential, E°cell, of +1.56V. B. The cell stops generating a voltage because the standard reduction potentials of Pb2+ and Zn2+ are both negative. C. The cell potential decreases because the reduction of Pb2+ is less thermodynamically favorable than the reduction of Ag+. D. The cell potential increases because twice as many electrons are transferred between Pb2+ and Zn than between Ag+ and Zn.
Principles of Instrumental Analysis
7th Edition
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Chapter22: An Introduction To Electroanalytical Chemistry
Section: Chapter Questions
Problem 22.1QAP: Calculate the electrode potentials of the following half-cells. (a) Ag+(0.0436 M)|Ag (b) Fe3+ (5.34 ...
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The cell potential for the standard galvanic cell shown above is +1.56V. If AgNO3(aq)|Ag(s) is replaced with 1M Pb(NO3)2(aq) solution and a Pb electrode, which of the following describes what happens to the operation of the cell, and why?
A. Nothing changes because galvanic cells that have a Zn(s) electrode have a constant cell potential, E°cell, of +1.56V.
B. The cell stops generating a voltage because the standard reduction potentials of Pb2+ and Zn2+ are both negative.
C. The cell potential decreases because the reduction of Pb2+ is less thermodynamically favorable than the reduction of Ag+.
D. The cell potential increases because twice as many electrons are transferred between Pb2+ and Zn than between Ag+ and Zn.
Transcribed Image Text:Voltmeter
Wire
+1.56 V
Ag
Zn
Salt Bridge
1 M Zn(NO3)2
1 M AgNO3
Half-Reaction
Standard Reduction Potential, E" (V)
Ag" (aq) +e Ag(s)
Ph* (ag) + 2e - Pb(s)
+0.80
-0.13
Zn" (ag) + 2 e→
Zn(s)
-0.76
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