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Van der Waals equation is an equation of state for a non-ideal gas that takes account of intermolecular forces and the volume occupied by the molecules of the gas.
The van der Waals equation is based on plausible reasons that real gases do not follow the ideal gas law. The ideal gas law treats gas molecules as point particles that do not interact with each other but only with their containers. In other words, they do not take up any space, and are not attracted or repelled by other gas molecules and thus never lose kinetic energy during collisions. The ideal gas law states that volume (V) occupied by n moles of any gas has a pressure (P) at temperature (T) in kelvins. The relationship for these variables is
PV = nRT
Where R is known as the gas constant, is called the ideal gas law or equation of state.
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