The ideal gas law treats the molecules of a gas as point particles with perfectly elastic collisions. This works well for dilute gases in many experimental circumstances. But gas molecules are not point masses, and there are circumstances where the properties of the molecules have an experimentally measurable effect. A modification of the ideal gas law was proposed by Johannes D. van der Waals in 1873 to take into account molecular size and molecular interaction forces. It is usually referred to as the van der Waals equation of state.

Symbol
$p_{\mathrm{VdW}}$
Unit
Pa
Formulae
$\frac{R_{\mathrm{gas}} T_{\mathrm{gas}}}{V_{\mathrm{m}} - b_{\mathrm{VdW}}} - \frac{a_{\mathrm{VdW}}}{V_{\mathrm{m}}^{2}}$
Related
$a_{\mathrm{VdW}}$
Van der Walls constant a [bar.L²/mol²]
$b_{\mathrm{VdW}}$
$R_{\mathrm{gas}}$
$T_{\mathrm{gas}}$
$V_{\mathrm{m}}$
Molar volume [m³/mol]