The standard reduction potentials of Zn2+|Zn and Cu2+|Cu are -0.76V and +0.34V respectively. What is the cell EMF of the following cell?
Zn|Zn2+(0.05M)||Cu2+(0.005M)|Cu
[RTF=0.059]
A
1.1295 V
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B
1.0705 V
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C
1.1000 V
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D
1.0412 V
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Solution
The correct option is B 1.0705 V The standard EMF of the given cell is: E0cell=E0Cu2+|Cu−E0Zn2+|Zn=0.34V−(−0.76V)=1.1V. The EMF of cell is: Ecell=E0cell−0.059nlog[Zn2+][Cu2+]. Ecell=1.1V−0.0592log0.050.005=1.1V−0.0295V=1.0705V.