Problem- 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 the standard change in Gibbs free energy is dekta G° = -69.0 kJ/mol. What is delta G for this reaction at 298 K when the partial pressures are PC2H6 0.100 atm, PH2 0.450 atm, and PCH4 0.085 atm. What is the delta G in kJ/mol?
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