Explore: Real Gases

Real gases are non-ideal gases whose molecules occupy space and have interactions; consequently, they do not adhere to the ideal gas law. To understand

gas like neon), or molecules (e.g. oxygen (O2) or carbon dioxide). Pure gases can also be mixed together such as in the air. What distinguishes gases

gases, such as many refrigerants, and for gases with strong intermolecular forces, notably water vapor. At high pressures, the volume of a real gas is

{nR}{V}})-({\frac {nRT}{V}})=0} Real gases have non-zero internal pressures because their internal energy changes as the gases expand isothermally - it can

Unlike ideal gases, the temperature of a real gas will change during a Joule expansion. At temperatures below their inversion temperature gases will cool

which is 99% diatomic). Also γ is typically 1.6 for mono atomic gases like the noble gases helium (He), and argon (Ar). In internal combustion engines γ

another. The kinetic theory of gases applies to the classical ideal gas, which is an idealization of real gases. In real gases, there are various effects

off each other during molecular collisions. In other words, real gases behave like ideal gases at low pressures and high temperatures. At moderately high

gas models which satisfy this theorem, such as the van der Waals model, the Dieterici model, and so on, that can be found on the page on real gases.

distinct liquid and gas phases of a given fluid do not exist. The pressure-volume-temperature (PVT) data for real gases varies from one pure gas to another. However