The cell in which the following reaction occurs `2Fe^(3+)(aq)+2I^(-)(aq)to2Fe^(2+)(aq)+I_(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.

The cell in which the following reaction occurs `2Fe^(3+)(aq)+2I^(-)(a

1.	The cell in which the following reaction occurs `2Fe^(3+)(aq)+2I^(-)(aq)to2Fe^(2+)(aq)+I_(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.
Answer» `2Fe^(3+)(aq)+2I^(-)(aq)to2Fe^(2+)(aq)+I_(2)(s)` For the given cell `n=2` `Delta_(r)G^(@)=-nFE_(cell)^(@)` `=-2xx96500xx0.236` `=-45.55kJ" "mol^(-1)` also, `Delta_(r)G^(@)=-2.303RT" "log" "K_(C)` `implieslogK_(C)=(-Delta_(r)G^(@))/(2.303RT)` `=(-45.55)/(2.303xx8.314xx10^(-3)xx298)` `=7.983` `impliesK_(C)="antilog"(7.983)` `=9.616xx10^(7)`

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The cell in which the following reaction occurs `2Fe^(3+)(aq)+2I^(-)(aq)to2Fe^(2+)(aq)+I_(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.

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