For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction   C2H6(g)+H2(g)↽−−⇀2CH4(g)   the standard change in Gibbs free energy is Δ?°=−72.6 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are ?C2H6=0.200 atm, ?H2=0.150 atm, and ?CH4=0.750 atm?

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