for the reaction . and at T = 298K the above equation can be written as = . V log K C = . V ( = .1V) log K C = ( .1V × ) .
. V K C = × at 298K. In general, = . RT nF log K C ( .
) Thus, Eq. ( . ) gives a relationship between equilibrium constant of the reaction and standard potential of the cell in which that reaction takes place. Thus, equilibrium constants of the reaction, difficult to measure otherwise, can be calculated from the corresponding E o value of the cell.
. . Equilibrium Constant from Nernst Equation