For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species.
For the reaction
the standard change in Gibbs free energy is Δ?°=−69.0 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are ?C2H6=0.300 atm, ?H2=0.500 atm, and ?CH4=0.950 atm?
The equation for Gibbs Free Energy is
G = + RT lnQ
For a gas phase reaction
aA(g) + bB(g) cC(g) + dD(g)
For Given Reaction
where = -69.0kJ/mol ; T = 298K ; R = 8.314 J K-1 mol-1
PC2H6 = 0.300 atm ; PH2 = 0.500 atm ; PCH4 = 0.950 atm
= -69000 J mol-1 + ( 8.314 J K-1 mol-1 )(298 K)
= -69000 J mol-1 + 4446.086 J mol-1
= - 64553.914 J mol-1
= - 64.55 kJ mol-1
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