How much heat (in J) is required to produce 2.0L of N2(g) at 77.36 K and 1.0 atm? The only thing that is given is: 

The enthalpy of vaporization for $N_2(l)$ is 5.56 kJ/mol.

There aren't any examples similar to this problem in the textbook. I only know how to get energy using:

$q=mcΔT$ and $w=PΔV$

No clue what to do with the enthalpy of vaporization value.

UPDATE: Solved it by first getting number of moles ($n$) via $PV=nRT$ then multiplying moles by 5.56 kJ/mol. Moles cancel out, leaving only kJ, 1.75kJ to be precise.
Since nitrogen's boiling point is 77.36 K , it appears that the question is asking how much heat is required to boil nitrogen to produce 2.0 L at 1 atm.