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The cell in which the following reaction...

The cell in which the following reaction occurs
`2Fe^(3+)(aq)+2I^(-)(aq)to2Fe^(2+)(aq)++I_(2)(s)` has `E_(cell)^(0)=0.236V` at 298 K.
Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

Text Solution

Verified by Experts

`n=2`
`DeltaG^(@)=-nFE_("cell")^(@)=-2xx96500xx0.236J=-45.55kJ//mol`
`DeltaG^(@)=-2.303"RT log K"_(c)`
`logK_(c)=(DeltaG^(@))/(-2.303RT)=(45.55xx10^(3))/(2.303xx8.314xx298)=7.983`
`K_(c)="antilog (7.982)"=9.616xx10^(7)`
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