1. Assume that one mole of H2O(g) condenses to H2O(l) at 1.00atm and 95 Celcius. Calculate q, w, ΔH, ΔS of the system, ΔS of surroundings. BUT I AM NOT ASKING HOW TO CALCULATE THESE VALUES, SEE LAST SENTENCE OF POST. 2. Relevant equations q = nCΔT ΔH = n(Cp)ΔT W = -PΔV ΔS = [q_reversible] / T Cp of H2O(l) = 75.3 J / K*mol Cp of H2O(g) = 36.4 J / K*mol ΔH-vaporization of H2O @ 100 = 40.7 kJ / K*mol 3. The attempt at a solution Basically, I have the solution but I don't understand why it's the case. When I asked my TA, he said that the condensation is actually occurring at 95 Celcius, which confused me right off the bat since I knew that at 1atm, the condensation point should be 100 degrees. Regardless, I thought that the step that was occurring should be simply: H2O (g) -> H2O (l) @ 95 degrees. Thus, I thought that since the system stays at the same temperature, then ΔE = 0 and that q = -w. However, this assumption is wrong. I am simply asking why this is wrong (and not to calculate the values).