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Question

Given below are the half-cell reactions:
Mn2++2eMn;E0=1.18V
2(Mn3++eMn2+);E0=+1.51V.

The E0 for 3Mn2+Mn+2Mn3+ will be:

A
0.33V; the reaction will not occur
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B
0.33V; the reaction will occur
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C
2.69V; the reaction will not occur
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D
2.69V; the reaction will occur
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Solution

The correct option is D 2.69V; the reaction will not occur
Adding equation 2 from 1 gives 3Mn2+Mn+2Mn3+

Hence, E0 for this reaction =(1.18)(+1.51) V
=2.69 V.

The reaction will not occur as E0cell is negative value as for spontaneous reaction value should be positive.

Option C is correct.

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