q = -35.2 kJ
w = 0 kJ
ΔU = -35.2 kJ
ΔH = -35.2 kJ
ΔS = -44.1 J K−1 mol−1
ΔSsurr = 0 J K−1 mol−1
ΔSuniv = -44.1 J K−1 mol−1
What are the values of q, w, ΔU, ΔH, ΔS, ΔSsurr, and ΔSuniv for the following constant pressure process for a system containing 0.956 moles of CH3OH ?
CH3OH(g, 122.0 ºC, 1.00 atm) ⟶ CH3OH(l, 34.0 ºC, 1.00 atm)
Assume that CH3OH(g) behaves as an ideal gas and the volume of CH3OH(l) is much less than that of CH3OH(g). Also, assume that the temperature of the surroundings is 34.0 ºC.
Data:
Molar heat capacity for CH3OH(g), Cp,m = 44.1 J K−1 mol−1
Molar heat capacity for CH3OH(l), Cp,m = 81.1 J K−1 mol−1
Enthalpy of vaporization, ΔvapH = 35.2 kJ mol−1 at 64.7 ºC and 1.00 atm
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