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Question

Given below are the half - cell reactions
Mn2++2eMn;E=1.18eV
2(Mn3++eMn2+);E0=+1.51eV
The Efor 3Mn2+Mn+2Mn3+ will be

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

The correct option is A -2.69 V; the reaction will not occur
Standard electrode potential of reaction [E] can be calculated as
Ecell=EREP
Where, ER=SRP of reactant, EP=SRP of product
If Ecell=+ve, then reaction is spontaneous otherwise non - spontaneous.
Mn3+E1=1.51 V−−−−−Mn2+Mn2+E21.18 V−−−−Mn
For Mn2+ disproportionation,
E=1.51V1.18V=2.69V<0
Thus, all reactions will not occur.

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