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Question

Consider the following E0 values:E0Fe3+/Fe2+=+0.77V
E0Sn2+/Sn=0.14V
Under standard conditions the potential for the reaction
Sn(s) +2Fe3+(aq)2Fe2+(aq)+Sn2+(aq) is:

A
1.68 V
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B
1.40 V
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C
0.91 V
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D
0.63 V
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Solution

The correct option is A 0.91 V
For the redox system:
Sn(s)+2Fe3+(aq)2Fe2+(aq)+Sn2+(aq)
Reaction at cathode:
2Fe3+(aq)+2e2Fe2+(aq)
Reaction at anode:
Sn2+(aq)+2eSn(s)
EFe3+/Fe2+=+0.77V
E0Sn2+/Sn=0.14V
Under standard conditions the potential for the reaction
Ecell=EcathodeEanode
Ecathode=+0.77 V
Eanode=0.14 V
Ecell=+0.77(0.14)
=+0.91 V
C is correct

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