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The standard e.m.f of a cell, involving ...

The standard e.m.f of a cell, involving one electron change is found to be 0.591 V at `25^(@) C`. The equilibrium constant of the reaction is : `(F=96,500C mol^(-1)`: R=8.314 `Jk^(-1)mol^(-1)`

A

`1.0xx10^(10)`

B

`1.0xx10^(5)`

C

`1.0xx10^(1)`

D

`1.0xx10^(30)`

Text Solution

Verified by Experts

The correct Answer is:
A
`E_(cell)=E_(cell)^(o)-(0.0591)/(n)logK_(C)`
At 298K `E_(cell)=0,0=0.591-(0.591)/(n)logK_(C)`
`logK_(C)=(0.591xx1)/(0.0591)=10,K_(c)="anti log 10"=1xx10^(10)`
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