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Question

Given below are the half-cell reaction:
Mn2++2eMn; E=1.18V
2(Mn3++eMn2+; E=+1.51V

The E for 3Mn2+Mn+2Mn3+ will be:
(IIT-JEE 2014)


A

(a) -0.33 V; the reaction will not occur

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B

(b) -0.33 V; the reaction will occur

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C

(c) -2.69 V; the reaction will not occur

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D

(d) -2.69 V; the reaction will occur

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Solution

The correct option is C

(c) -2.69 V; the reaction will not occur


Mn2++2eMn; E=1.18V
2Mn2++2Mn3++2e; E=1.51V
______________________________________________________________________
3Mn2+Mn+2Mn3+
______________________________________________________________________

Ecell=Ered+Eoxid
= -1.18 + (-1.51) = -2.69 V

Negative EMF reflects non-spontaneous cell reaction.


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