The amount of useful work other than the expansion work that a reaction can produce is given by the ΔG°rxn of the process. So the value for the maximum electrical work that can be done in a reaction can be obtained from ΔG°rxn. And if both ΔH° and ΔS° are known it can be calculated using ΔG°rxn = ΔH° rxn – TΔS° rxn. What is the maximum amount of electrical work (per mole of fuel) that the same reactions can perform when carried out at 298K for C6H6(l) ?