Chapter 17, Problem 77P

At high gas densities, the van der Waals equation modifies the ideal-gas law to account for nonzero molecular volume and for the van der Waals force that we discussed in Section 17.1. The van der Waals equation is

$\left(p\text{}\text{ + }\frac{n^{2}a}{V^2}\right)(V-nb)=nRT$

where a and b are constants that depend on the particular gas. For nitrogen (N₂), a = 0.14 Pa m⁶/mol² and b = 3.91 × 10⁻⁵ m³/mol. For 1.000 mol of N₂ at 10.00 atm pressure, confined to a volume of 2.000 L. find the temperatures predicted (a) by the ideal-gas law and (b) by the van der Waals equation.