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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

`1.0 xx 10^(10)`

B

`1.0 xx 10^(5)`

C

`1.0 xx 10^(1)`

D

`1.0 xx 10^(30)`

Text Solution

Verified by Experts

The correct Answer is:
A
`E_(cell) = E_(cell)^(@) - (0.0591)/(n) logQ`
At equilibrium
`E_(cell) = 0, Q = K`
`0 = 0.591 - (0.0591)/(1) log K`
`log K = 10`
`K = 10^(10)`
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