The Van der Waals law

The law

The →   ideal gas law considers the molecules or atoms of a gas as point particles that exert a pressure by striking the wall of the container that contains them. In fact, Van der Waals found it necessary to introduce corrections due to the fact - that the particles of a gas do not only hit the walls, but also suffer collisions between them. - that these particles are not punctual but have a specific volume These two corrections are translated by both →         Van der Waals parameters (constants) $a$ and $b$ which differ from one gas to another:

$(P\; +\;\frac{n^2\cdot a}{V^2})(V- n\cdot b)$$=$$n\;R\;T$

with: $a$ Parameter (takes into account interactions) $b$ Parameter (takes into account the reduction of the total volume because of the particulate volumes of the particles) $P$ Pressure $V$ Volume $n$ Number of moles $T$ Kelvin temperature $R$ Ideal gas constant = $0,08205 \frac{L\;atm}{mole\;K}$