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  2. Real gas - Wikipedia

    en.wikipedia.org/wiki/Real_gas

    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;

  3. Van der Waals equation - Wikipedia

    en.wikipedia.org/wiki/Van_der_Waals_equation

    The van der Waals equation is a mathematical formula that describes the behavior of real gases. It is named after Dutch physicist Johannes Diderik van der Waals . It is an equation of state that relates the pressure , temperature , and molar volume in a fluid .

  4. Gas - Wikipedia

    en.wikipedia.org/wiki/Gas

    The van der Waals interactions between gas molecules, is the reason why modeling a "real gas" is more mathematically difficult than an "ideal gas". Ignoring these proximity-dependent forces allows a real gas to be treated like an ideal gas, which greatly simplifies calculation. Isothermal curves depicting the non-ideality of a real gas.

  5. Ideal gas - Wikipedia

    en.wikipedia.org/wiki/Ideal_gas

    At high pressures, the volume of a real gas is often considerably larger than that of an ideal gas. 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 ...

  6. Fugacity - Wikipedia

    en.wikipedia.org/wiki/Fugacity

    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 ...

  7. Joule–Thomson effect - Wikipedia

    en.wikipedia.org/wiki/Joule–Thomson_effect

    For such an ideal gas, this theoretical result implies that: The internal energy of a fixed mass of an ideal gas depends only on its temperature (not pressure or volume). This rule was originally found by Joule experimentally for real gases and is known as Joule's second law. More refined experiments found important deviations from it. [27] [28 ...

  8. Boyle temperature - Wikipedia

    en.wikipedia.org/wiki/Boyle_temperature

    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 ...

  9. Amagat's law - Wikipedia

    en.wikipedia.org/wiki/Amagat's_law

    However, for real (non-ideal) gases, the results differ. [3] Dalton's law of partial pressures assumes that the gases in the mixture are non-interacting (with each other) and each gas independently applies its own pressure , the sum of which is the total pressure.