Give the relation between equilibrium constant of the reaction and standard potential of the cell.

Explanation

`E_("cell")-(2.303RT)/(nF)log K_(c). `E_("cell")^(0) to ` Standard potential fo the cell.
`R to" Gas constant (8.314 JK^(-1)"mol"^(-1). T to ` "Absolute temperature".`
`n to ` No. of electrons involved `F to" Faraday constant (96500C" mol^(-1))`
`K_(c) to ` Equilibrium constant
At 298 K or `25^(@)C`
`E_("cell")^(0)-(0.059)/(n)log K_(C)`