1. The problem statement, all variables and given/known data For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar for all species. For the reaction 2 NO(gas) + O2(gas) <---> 2 NO2(gas), the standard change in Gibbs free energy (ΔG°) = -72.6 kJ. What is the ΔG for this reaction at 298 K when the partial pressures are PNO = 0.500 bar, PO2 = 0.100 bar, PNO2 = 0.900 bar. 2. Relevant equations Q = (PNO2)2 / (PO2)(PNO)2 ΔG = ΔG° + RTln(Q) 3. The attempt at a solution Q = (PNO2)2 / (PO2)(PNO)2 Q = (0.900 bar)2 / (0.100)(0.500)2 Q = 32.4 ΔG = ΔG° + RTln(Q) ΔG = -72.6 kJ + (0.008314 kJ mol- K-)(298 K)(ln 32.4) ΔG = -72.6 + 8.6174 = -63.98 kJ I am not sure about my approach to this question. Can anyone confirm if I am on the right track? Thanks. All help Is very much appreciated.