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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 the behaviour of real gases, the following must be taken into account: compressibility effects; variable specific heat capacity; van der Waals forces; non-equilibrium thermodynamic effects;
For an ideal gas, fugacity and pressure are equal, and so φ = 1. Taken at the same temperature and pressure, the difference between the molar Gibbs free energies of a real gas and the corresponding ideal gas is equal to RT ln φ. The fugacity is closely related to the thermodynamic activity. For a gas, the activity is simply the fugacity ...
In thermodynamics, the compressibility factor (Z), also known as the compression factor or the gas deviation factor, describes the deviation of a real gas from ideal gas behaviour. It is simply defined as the ratio of the molar volume of a gas to the molar volume of an ideal gas at the same temperature and pressure .
In thermodynamics, the Joule–Thomson effect (also known as the Joule–Kelvin effect or Kelvin–Joule effect) describes the temperature change of a real gas or liquid (as differentiated from an ideal gas) when it is expanding; typically caused by the pressure loss from flow through a valve or porous plug while keeping it insulated so that no heat is exchanged with the environment.
Although ideal gases, for which = (), do not change temperature in such a process, real gases do, and it is important in applications to know whether they heat up or cool down. [ 76 ] This coefficient can be found in terms of the previously derived α {\displaystyle \alpha } and c p {\displaystyle c_{p}} as [ 77 ] μ J T = v ( α T − 1 ) c p ...
At low temperatures, the pressure of a real gas is often considerably less than that of an ideal gas. At some point of low temperature and high pressure, real gases undergo a phase transition, such as to a liquid or a solid. The model of an ideal gas, however, does not describe or allow phase transitions.
Real gases are characterized by their compressibility (z) in the equation PV = zn 0 RT. When the pressure P is set as a function of the volume V where the series is determined by set temperatures T, P, and V began to take hyperbolic relationships that are exhibited by ideal gases as the temperatures start to get very high. A critical point is ...
This is the virial equation of state and describes a real gas. Since higher order virial coefficients are generally much smaller than the second coefficient, the gas tends to behave as an ideal gas over a wider range of pressures when the temperature reaches the Boyle temperature (or when c = 1 V m {\textstyle c={\frac {1}{V_{m}}}} or P ...