Question

What is the relationship between the standard Gibbs energy change and the equillibrium constant of the reaction?

Answer 1

A non-spontaneous reaction has a positive delta G and a small K value. When delta G is equal to zero and K is around one, the reaction is at equilibrium. You have learned the relationship linking these two properties. This relationship allows us to relate the standard free energy change to the equilibrium constant.

Answer 2

Relationship between Gibbs 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)

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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

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