We’re being asked to calculate the pressure exerted by a Ne in a box using the Van der Waal’s equation.

The **Van der Waals equation** is shown below:

$\overline{)\left(\mathbf{P}\mathbf{+}\mathbf{a}\frac{{\mathbf{n}}^{\mathbf{2}}}{{\mathbf{V}}^{\mathbf{2}}}\right)\left(\mathbf{V}\mathbf{-}\mathbf{n}\mathbf{b}\right){\mathbf{=}}{\mathbf{n}}{\mathbf{R}}{\mathbf{T}}}$

▪ **P** = pressure, atm

▪ **V** = volume, L

▪ **n** = # of moles, mol

▪ **R** = gas constant = 0.08206 (L∙atm)/(mol∙K)

▪ **T** = temperature, K

▪ **a** = polarity coefficient

▪ **b **= size coefficient

Let’s first isolate the pressure in the **Van der Waals Equation**:

Calculate the pressure exerted by 1.00 mol of Ne in a box that is 0.300 L and 298 K. For Ne, a = 0.211 L^{2} atm/mol^{2} and b = 0.0171 L/mol.