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State function
In thermodynamics, a state function, function of state, state quantity, or state variable is a property of a system that depends only on the current, equilbrium state of the system. State functions thus do not depend on the path by which the system arrived at its present state. A state function describes the equilibrium state of a system. For example, internal energy, enthalpy, and entropy are ''state quantities'' because they describe quantitatively an equilibrium state of a thermodynamic system, irrespective of how the system arrived in that state.
In contrast, mechanical work and heat are process quantities because their values depend on the specific ''transition'' (or path) between two equilibrium states.
==History==
It is likely that the term “functions of state” was used in a loose sense during the 1850s and 60s by those such as Rudolf Clausius, William Rankine, Peter Tait, William Thomson, and it is clear that by the 1870s the term had acquired a use of its own. In 1873, for example, Willard Gibbs, in his paper “Graphical Methods in the Thermodynamics of Fluids”, states: “The quantities V, B, T, U, and S are determined when the state of the body is given, and it may be permitted to call them ''functions of the state of the body''.”
抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』
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