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Relationship between free Energy and Equilibrium Constant

The free energy change of the reaction in any state, ΔG (when equilibrium has not been attained) is related to the standard free energy change of the reaction, ΔG0 (which is equal to the difference in free energies of formation of the products and reactants both in their standard states) according to the equation.

      ΔG = ΔGo + RT InQ

Where Q is the reaction quotient

When equilibrium is attained, there is no further free energy change i.e. ΔG = 0 and Q becomes equal to equilibrium constant. Hence the above equation becomes.

           ΔGo = –RT In K(eq) 

      or  ΔGo = –2.303 RT log K(eq)

In case of galvanic cells. Gibbs energy change ΔG is related to the electrical work done by the cell.

ΔG = -nFE(cell) where n = no. of moles of electrons involved

                        F = the Faraday constant

                        E = emf of the cell

If reactants and products are in their standard states ΔGo = –nFEocell

Solved example: Calculate ΔG0 for conversion of oxygen to ozone 3/2 O2 (g) ——> O3 (g) at 298 K, if Kp for this conversion is 2.47 ´ 10-29.

Solution: ΔGo = –2.303 RT log Kp

Where R = 8.314 J/K mol, Kp = 2.47 ´ 10-29, T = 298K

       ΔG0 = 16300 J/mol = 163 KJ/mol.

To read more, Buy study materials of Thermodynamics comprising study notes, revision notes, video lectures, previous year solved questions etc. Also browse for more study materials on Chemistry here.

 

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