The Van der Waals equation is shown below:

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

Rearranging:

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

Calculate the pressure exerted by 1.00 mol of H_{2} in a box that is 0.300 L and 298 K. For H_{2}, a = 0.244 L^{2} atm/mol^{2} and b = 0.0266 L/mol.

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