Calculating the energy state changes of an organic compound?

Question

How much heat is required to raise the temperature of 210 g of

CH3OH(L) from 22.0 to 30.0 degrees C and than vaporize it at 30.0 degrees C?

The molar heat capacity of CH3OH(L) is 81.1 J /mol x K

The heat of vaporization of CH3OH at 298K is 38.0 kJ/Mol

Answer 1

30.0C - 22.0C = 8degC difference

Atomic weights: C=12  H=1  O=16  CH4O=32

First raise the temperature of the liquid:

210gCH3OH x 1molCH3OH/32gCH3OH x 8.0degC x 81.1J/1molCH3OH = 4257.75 J

Next boil the liquid:

210gCH3OH x 1molCH3OH/32gCH3OH x 38.0J/1molCH3OH = 249.38 J

Finally, addem up:

4257.75 + 249.38 = 4510 J to three significant figures