The cell in which the following reactions occurs : 2Fe_((aq))^(3+)+2l_((aq))^(-) to 2Fe_((aq))^(2+)+I_(2(S)) has E_(cell)^(Theta)=0.236V at 298 K. calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

The cell in which the following reactions occurs : 2Fe_((aq))^(3+)+2l_

1.	The cell in which the following reactions occurs : 2Fe_((aq))^(3+)+2l_((aq))^(-) to 2Fe_((aq))^(2+)+I_(2(S)) has E_(cell)^(Theta)=0.236V at 298 K. calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.
Answer» Solution :(a) Cell reaction and calculation of `Delta_(R)G^(Theta)`: Where, n=2 MOL, `F=96487" C "mol^(-1)`, `E_(cell)^(Theta)=0.236V` `THEREFORE Delta_(r)G^(Theta)=-nFE_(cell)^(Theta)` `=-(2mol)(96487" C "mol^(-1))(0.236V)` `=-45542(V)` `=-45542J` =-45.542 kJ `~~-45.54kJ` (b) Calculation of equilibrium constant `K_(c)`: `therefore Delta_(r)G^(Theta)=-2.303RT" log "K_(c)` `therefore -45542=-2.303xx8.314xx298xxlog" "K_(c)` `therefore log" "K_(c)=(-45542)/(-2.303xx8.314xx298)` `therefore log" "K_(c)=+7.9816` `thereforeK_(c)="Antilog"(7.9816)` `=9.586xx10^(7)` `~~9.6xx10^(7)`