This page relates to the physical properties of real gases.   The webpage Gas Properties includes some general physical properties of selected gases.  Thermodynamic and heat transfer relationships for fluids can be found on page Thermodynamics /Heat Transfer

The laws and rules for ideal gases are only reasonable accurate for gases at low pressures and moderately high temperatures...At pressures around 1 bara or less the ideal gases are generally reasonably accurate for real gases.

The main reasons for the divergence from the ideal gas laws are that molecules actually attract each other and that molecules have real volumes.  The ideal gas laws assume that the volume of a gas molecule can be discounted and that molecules do not attract each other.  It is also apparent that as molecules approach very close, the attraction changes to repulsion.. In 1873 van der Waals devised a crude simple equation to adapt the ideal gas laws to the behaviour or real gases

Considering a molecule in a container.  The molecule will be attracted to all other molecules when located in away from the container wall.  When local to the container wall there will be greater attraction towards the molecules within the centre of the container and its momentum will be reduced.  The higher the pressure greater the inward attract and the more significant is this effect.   The correction for pressure will depend on the number of molecules at the surface and the number within the body of the gas.  Both of these factors vary inversely with the volume V.  Van der Walls proposed that a compensatory factor a/V² be added to the true pressure.

It is also true that the volume containing a gas within which the molecules are moving is reduced by the effective volume of the molecules.  This reduction is greater if the pressure is increased..Van der Walls proposed a factor b to allow for this reduction this factor is greater at higher pressures.
The Gas law as modified by Van der Waals for real gases is as follows >

The critical temperature for a matter is the maximum temperature that a gas can be liquified is called the critical temperature for the gas.   The liquid state cannot exist above this temperature.  

The pressure to cause liquifaction at this temperature is called the critical pressure. A vapor is really a gaseous state of a substance when its temperature is below the critical temperature.  A vapour can therefore by condensed to a liquid by increasing the pressure.