From the data below, calculate the total heat (in J) needed to convert 0.333 mol of gaseous ethanol at 300 degrees celcius and 1 atm to liquid ethanol at 25.0 degrees celcius and 1 atm.
bp at 1 atm: 78.5 degrees celcius
c(gas) = 1.43 J/g*C
(delta)H^0vapor = 40.5 kJ/mol
c(liquid) = 2.45 J/g*C
I really just need someone to tell me how to solve this. I don't care if someone gives me the answer I just need to know the steps to solve it and the equations that are used.