Above the Boyle temperature, the compressibility factor is always greater than unity and increases slowly but steadily as pressure increases.
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Deviations of the compressibility factor, " Z ", from unity are due to attractive and repulsive Intermolecular forces.
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For non-ideal gasses ( most gasses ) a compressibility factor " Z " is introduced to allow for non-ideality.
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The ratio of the value of PV to that expected for an ideal gas at the same temperature is called the compressibility factor, Z.
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A few Approved articles, such as Compressibility factor ( gases ), come close to the citation density of a typical Wikipedia Featured Article.
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The Redlich Kwong equation can also be represented as an equation for the compressibility factor of a gas, as a function of temperature and pressure:
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There are more detailed generalized compressibility factor graphs based on as many as 25 or more different pure gases, such as the Nelson-Obert graphs.
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Where \ omega is the acentric factor of the species, R is the universal gas constant and Z = PV / ( RT ) is compressibility factor.
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For a gas, this is typically less than unity at low temperature and greater than unity at high temperature ( see the discussion in compressibility factor ).
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However, when the compressibility factors of various single-component gases are graphed versus pressure along with temperature isotherms many of the graphs exhibit similar isotherm shapes.
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