The standard free energy change of a process, ΔG°, was defined in a previous chapter as the maximum work that could be performed by a system, wmax. In the case of a redox reaction taking place within a galvanic cell under standard state conditions, essentially all the work is associated with transferring the electrons from reductant-to-oxidant, welec:
$$ΔG°=w_{max}=w_{elec}$$
The work associated with transferring electrons is determined by the total amount of charge (coulombs) transferred and the cell potential:
$$ΔG°=w_{elec}=-nFE^°{cell}$$ $$ΔG°=-nFE^°{cell}$$
where n is the number of moles of electrons transferred, F is Faraday’s constant, and E°cell is the standard cell potential. The relation between free energy change and standard cell potential confirms the sign conventions and spontaneity criteria previously discussed for both of these properties: spontaneous redox reactions exhibit positive potentials and negative free energy changes.