The relationship between the change in Gibbs free energy and the emf of an electrochemical cell is given by .

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The relationship between the change in Gibbs free energy and the emf of an electrochemical cell is given by the equation ΔG = - nFE, where ΔG is the change in Gibbs free energy, n is the number of moles of electrons transferred in the reaction, F is the Faraday constant (the charge of one mole of electrons), and E is the emf of the cell. This equation is derived from the definition of Gibbs free energy and the equation for the cell potential, Ecell = Eoxidation - Ereduction, where Eoxidation and Ereduction are the reduction potentials of the half-reactions involved in the cell reaction. The relationship between ΔG and Ecell is used to determine the feasibility and spontaneity of electrochemical reactions.

The Relationship Between the Change in Gibbs Free Energy and the Emf