please help find answers a -d

All Sections (a) The pure toluene vapor pressure is 28.4 torr; and pure benzene vapor pressure is 98.4 torr at 25C. What can you conclude about the relative values of enthalpy of vaporization for these two compounds? which one might have larger enthalpy of vaporization? what is the potential reason behind this behavior? (b) Suppose now you mix toluene and benzene together, the mixed solution has 24% by mass for toluene. Show how you get the mole fraction of toluene in the solution phase. What is the mole fraction of benzene in the solution? (c) Further, calculate the partial vapor pressure of toluene above the mixed solution in (b). Also get the partial vapor pressure of benzene above the mixed solution. Add these two to get the total vapor pressure Ptot = P(tolunene) + P(benzene). (d) For the vapor phase above the mixed solution, it is a mixing of tolunene and benzene mixture. The mole fraction of tolunene in the vapor phase is given by P(toluenen)/Ptot (according to Dalton's law). Get the mole fraction of toluene in the gas phase and compare the mole fraction of tolunene in the solution phase (you got that in (b)). are the two numbers same or not same? Explain how the two mole fractions should relate to each other