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Equilibrium Constant and Free Energy Change
for an Electrochemical Cell

Two important important parameters that can be determined from a cell potential are the equilibrium constant for the cell reaction and the free energy change for the cell reaction.

Determining the Equilibrium Constant from Eocell

To calculate the equilibrium constant for an electrochemical cell we need to know:

The Nernst equation is used in calculating the equilibrium constant.

Nernst Equation

At equilibrium Q = K. Substituting in K for Q, and the values for R, T, and F, we get:

Nernst Equation

Example:  Find the value of the equilibrium constant at 25oC for the cell reaction for the following electrochemical cell:

Cu | Cu2+(1 M) || Ag+(1 M) | Ag.

2 Ag+(aq) + 2 e- --> 2 Ag(s) Eoreduction = + 0.799 V
Cu(s) --> Cu2+(aq) + 2 e- Eooxidation = - 0.518 V


2 Ag+(aq) + Al(s) --> 2 Ag(s) + Cu2+(aq) Eocell = + 0.281 V

n = 2 moles of electrons

Solving for K

Note:  values for the equilibrium constant for electrochemical cell reactions are sometimes very large.

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Determining the Standard State Free Energy Change from Eocell

To determine the standard state free energy change for a cell reaction

DGo = - nFEocell

        DGo = standard state free energy change (joules)
        n = number of moles of electrons transferred
        F = Faraday's constant (96,485 C/mol e-)
        Eocell = standard state cell potential (volts or joules/C)

Example:  Find the value of the equilibrium constant at 25oC for the cell reaction for the following electrochemical cell:

Cu | Cu2+(1 M) || Ag+(1 M) | Ag.

(The solution for the determination of the Eocell and the number of moles of electrons, n, are shown in the example in the previous section. Click HERE to see the solution.)

DGo = - (2 mol e-)(96,485 C/mol e-)(0.281 J/C)
DGo = - 54,200 J or - 54.2 kJ

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Determining the Non-Standard State Free Energy Change

To determine the non-standard state free energy change:

DG = - nFEcell

Example: Calculate the free energy change for the following electrochemical cell.

Zn(s) | Zn2+ (1.50 M) || Cu2+ (0.25 M) | Cu(s)

Calculation of Non-Standard Free Energy Change

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