How can Nernst equation be applied in calculating the equilibrium constant for any cell reaction ?

Calculation Of Equilibrium Constant

The value of equilibrium constant for a feasible cell reaction is :

How is free energy change related to equilibrium constant for the reaction?

The EMF of a cell is related to the equilibrium constant of the cell reaction as

Equilibrium const and nernst equation

The driving force DeltaG diminishes to zero on the way to equilibrium, just as in any other spontaneous process. Both DeltaG and the corresponding cell potential (E=-(DeltaG)/(nF)) are zero when the redox reaction comes to equilibrium. The Nernst equation for the redox process of the cell may be given as : E=E^(@)-0.059/n log Q The key to the relationship is the standard cell potential E^(@) , derived from the standard free energy changes as : E^(@)=-(DeltaG^(@))/(nF) At equilibrium, the Nernst equation is given as : E^(@)=0.059/n log K The equilibrium constant K_(c) for the reaction : Cu(s)+2Ag^(+) (aq.)+2Ag(s)" "(E_(cell)^(@)=0.46 V) will be :

For a system in equilibrium, the rate constant for the forward reaction is represented by K_f and the rate constant for the reverse reaction is represented by K_r .Which equation represents the equilibrium constant for this reaction in the forward direction ?