Equilibrium constant is related to `E_("cell")^(@)` but not `E_("cell")-` Explain why?

Explanation

The standard Gibbs free energy change `(DeltaG^(@))` is related to the equilibrium constant (K) as `DeltaG^(@)-RT ln K` and to the `E_("cell")^(@)` as `DeltaG^(@)=-nFE^(@)`. Thus, the equilibrium contant is related to `E^(@)` as `E^(@)=(RT ln K)/(nF)`. The free energy change under non- standard condition `(DeltaG)` is related to `E_("cell)` as `DeltaG=-nFE_("cell").`
but like the relation `DeltaG^(@)-RT ln K`, there is not relation between `DeltaG` and K. This is why K is not related to `E_("cell")`.