Half-Reaction Standard Reduction Potential , E°(V) Ag+(aq)+e−→Ag(s) +0.80 Pb2+(aq)+2e−→Pb(s) −0.13 Zn2+(aq)+2e−→Zn(s) −0.76 The cell potential for the standard galvanic cell shown above is +1.56V . If AgNO3(aq)|Ag(s) is replaced with 1MPb(NO3)2(aq) solution and a Pb electrode, which of the following describes what happens to the operation of the cell, and why? a) The cell potential increases because twice as many
Half-Reaction Standard Reduction Potential , E°(V)
Ag+(aq)+e−→Ag(s) +0.80
Pb2+(aq)+2e−→Pb(s) −0.13
Zn2+(aq)+2e−→Zn(s) −0.76
The cell potential for the standard galvanic cell shown above is +1.56V . If AgNO3(aq)|Ag(s) is replaced with 1MPb(NO3)2(aq) solution and a Pb electrode, which of the following describes what happens to the operation of the cell, and why?
a) The cell potential increases because twice as many electrons are transferred between Pb2+ and Zn than between Ag+ and Zn .
b) Nothing changes because galvanic cells that have a Zn(s) electrode have a constant cell potential, E°cell , of +1.56V .
c) The cell potential decreases because the reduction of Pb2+ is less
d) The cell stops generating a voltage because the standard reduction potentials of Pb2+ and Zn2+ are both negative.
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