Answer
$[([C]^c\times [D]^d)\div([A]^a\times [B]^b] = K_{c} $
Work Step by Step
Consider a cell reaction involving n electrons
$ aA + bB → cC + dD $
The nernst equation for this cell reaction can be written as
$ E_{cell} =
E^{\circ}_{cell} –[ (R\times T)\div(n \times F)] \times ln[([C]^c\times [D]^d )\div([A]^a\times [B]^b]$
Or
$ E_{cell} =
E^{\circ}_{cell} –[ (R\times T)\div(n \times F)] \times lnK_{c} $
Where,
$ ([C]^c, [D]^d)$ = concentration of products raised to the power of stoichiometric constants.
$ ([A]^a, [B]^b)$ = concentration of reactants raised to the power of stoichiometric constants.
$[([C]^c\times [D]^d)\div([A]^a\times [B]^b] = K_{c} $
$K_{c}$ =Equilibrium Constant of cell reaction
$ E_{cell} =$ Cell potential at any concentrations.
$ E^{\circ}_{cell}$ = Cell potential at standard conditions.
R = Universal gas constant.
T = Absolute temparature.
n = number of electrons involved.
F = Faradays Constant.
