This problem is quite involved, but it is extremely instructive for understanding phase transitions in particular and chemical equilibrium in general.

Find the temperature at which N2 boils at a pressure of 1 bar. Use the van der Waals constants given below:

Constants for N2,

1.3661 a/dm6*bar*mol-2, 1.3483 a/dm6*atm*mol-2, 0.038577b/dm3*mol-1

Compare this temperature with the true boiling point of N2. The boiling temperature is the temperature at which the areas under the two van der Waals loops are equal. In order to solve the problem, you will need to graph the van der Waals equation for N2 for various values of the temperature and compute the areas under the loops. The loops you obtain will not be symmetric.