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 ΔG°=−32.8 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are PC2H6=0.500 atm , PH2=0.100 atm , and PCH4=0.800 atm ?

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