Why is the vaporization enthalpy of the mixture greater than that of the pure substance?
Thread Content
At atmospheric pressure, the enthalpy of vaporization of C3H8 is 101.25 Kcal/hr, while that of N-C5H12 is 85.69 Kcal/hr. If C3H8 and N-C5H12 are mixed in a 1:1 (mol) ratio, Aspen calculates the vaporization enthalpy of the mixture at atmospheric pressure to be 112.224 Kcal/hr, which is higher than that of either C3H8 or N-C5H12 alone. How can this be explained theoretically?
Is it necessary to overcome the heat of solution? I’m just guessing since I don’t know