General principle in thermodynamics regarding pVT systems in equilibrium
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"Gibbs rule" redirects here. Not to be confused with Antony Gibbs & Sons v La Societe Industrielle et Commerciale des Metaux.
In thermodynamics, the phase rule is a general principle governing "pVT" systems, whose thermodynamic states are completely described by the variables pressure (p), volume (V) and temperature (T), in thermodynamic equilibrium. If F is the number of degrees of freedom, C is the number of components and P is the number of phases, then
[1][2]: 123–125
It was derived by American physicist Josiah Willard Gibbs in his landmark paper titled On the Equilibrium of Heterogeneous Substances, published in parts between 1875 and 1878.[3]
The rule assumes the components do not react with each other.
The number of degrees of freedom is the number of independent intensive variables, i.e. the largest number of thermodynamic parameters such as temperature or pressure that can be varied simultaneously and arbitrarily without determining one another. An example of one-component system is a system involving one pure chemical, while two-component systems, such as mixtures of water and ethanol, have two chemically independent components, and so on. Typical phases are solids, liquids and gases.
^Ness, Hendrick C. Van; Abbott, Michael; Swihart, Mark; Smith, J. M. (March 20, 2017). Introduction to Chemical Engineering Thermodynamics. Dubuque, Iowa: McGraw Hill Education. p. 422. ISBN 9781259696527. OCLC 1001316575.
^Atkins, Peter William; Paula, Julio De; Keeler, James (2018). Atkins' Physical Chemistry (11th ed.). Oxford University Press. ISBN 9780198769866. OCLC 1013164457.
^Gibbs, Josiah W. (1906). Scientific Papers of J. Willard Gibbs. Longmans, Green and Co. OCLC 1136910263.
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