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

Answer

`DeltaG^(@)=-45.548" kJ mol"^(-1)`

Explanation

The redox reaction in the cell is :
`2Fe^(3+)(aq)+2e^(-) to 2Fe^(-)(aq)`
`2Fe^(3+)(aq)+2e^(-) to 2Fe^(2+)(aq)`
`2l^(-)(aq) to l_(2)(s)+2e^(-)`
`DeltaG^(@)=-nFE_(cell)^(@)`
`=-2xx(96500" C mol"^(-1))xx(0.236" V")=45,548" CV "mol^(-1)`
`=-45.548" J mol"^(-1)=-45.548" kJ mol"^(-1)`