The state of equilibrium is a common feature of all branches of physical science. It plays an important role when either chemical, mechanical or electromagnetic phenomena are described. Three examples emphasizing chemical applications must suffice. Analytical and preparative chemists use equilibrium considerations to select the temperature and concentration ranges best suited for their work. Chemical and metallurgical processes are often designed on the basis of equilibrium calculations. Moreover, equilibrium models for distribution of species in natural waters are frequently applied by geochemists.
As originally demonstrated by Gibbs, the concept of equilibrium is described in an entirely general way by classical thermodynamics (Gibbs, 1875). Let us consider the contemporary treatment also based on the second law and using modern nomenclature given by McGlashan (1979):
If a spontaneous process occurs in an isolated system Σ consisting of one or more phases α β ..., the entropy S...
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Bibliography
Gibbs, J. W. (1875) On the equilibrium of heterogeneous substances, in The Collected Works of J. Willard Gibbs. volume I: Thermodynamics. New Haven: Yale University Press. Reprinted 1948, P. 56.
McGlashan, M. L. (1979) Chemical Thermodynamics. London: Academic Press, 345 pp.
Cross references
Activation energy, activation enthalpy, activation volume; Chemical kinetics; Chemical potential; Clapeyron's equation; Equilibrium constant; Enthalpy; Entropy; Fluid-rock interactions; Free energy; Fugacity; Geochemical thermodynamics; Gibbs-Duhem equation; Henry's law; Metamorphic environments; Partition coefficients; Phase equilibria
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Gamsjäger, H. (1998). Equilibrium . In: Geochemistry. Encyclopedia of Earth Science. Springer, Dordrecht. https://doi.org/10.1007/1-4020-4496-8_116
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DOI: https://doi.org/10.1007/1-4020-4496-8_116
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