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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)
  1. (b) -0.33 V; the reaction will occur
  2. (c) -2.69 V; the reaction will not occur
  3. (a) -0.33 V; the reaction will not occur
  4. (d) -2.69 V; the reaction will occur


Solution

The correct option is B (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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