Functions of state
{{ safesubst:#invoke:Unsubst$N=Unreferenced date=__DATE__ $B= {{#invoke:Message boxambox}} }} {{#invoke:Sidebar collapsible  bodyclass = plainlist  titlestyle = paddingbottom:0.3em;borderbottom:1px solid #aaa;  title = Thermodynamics  imagestyle = display:block;margin:0.3em 0 0.4em;  image =  caption = The classical Carnot heat engine  listtitlestyle = background:#ddf;textalign:center;  expanded = System properties
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State 

Processes 
Cycles 
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Functions of state 

Process functions 
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 Maxwell relations
 Onsager reciprocal relations
 Bridgman's equations
 Table of thermodynamic equations
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History 

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 Bernoulli
 Carnot
 Clapeyron
 Clausius
 Carathéodory
 Duhem
 Gibbs
 von Helmholtz
 Joule
 Maxwell
 von Mayer
 Onsager
 Rankine
 Smeaton
 Stahl
 Thompson
 Thomson
 Waterston
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}} 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 state of the system, not on the way in which the system acquired that state (independent of path). 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.
The opposite of a state function is a path function.
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.”
Overview
A thermodynamic system is described by a number of thermodynamic parameters (e.g. temperature, volume, pressure) which are not necessarily independent. The number of parameters needed to describe the system is the dimension of the state space of the system (). For example, a monatomic gas with a fixed number of particles is a simple case of a twodimensional system (). In this example, any system is uniquely specified by two parameters, such as pressure and volume, or perhaps pressure and temperature. These choices are equivalent. They are simply different coordinate systems in the twodimensional thermodynamic state space. An analogous statement holds for higher dimensional spaces, as described by the state postulate.
When a system changes state continuously, it traces out a "path" in the state space. The path can be specified by noting the values of the state parameters as the system traces out the path, perhaps as a function of time, or some other external variable. For example, we might have the pressure and the volume as functions of time from time to . This will specify a path in our two dimensional state space example. We can now form all sorts of functions of time which we may integrate over the path. For example if we wish to calculate the work done by the system from time to time we calculate
It is clear that in order to calculate the work W in the above integral, we will have to know the functions and at each time , over the entire path. A state function is a function of the parameters of the system which only depends upon the parameters' values at the endpoints of the path. For example, suppose we wish to calculate the work plus the integral of over the path. We would have:
It can be seen that the integrand can be expressed as the exact differential of the function and that therefore, the integral can be expressed as the difference in the value of at the end points of the integration. The product is therefore a state function of the system.
By way of notation, we will specify the use of d to denote an exact differential. In other words, the integral of will be equal to . The symbol δ will be reserved for an inexact differential, which cannot be integrated without full knowledge of the path. For example will be used to denote an infinitesimal increment of work.
It is best to think of state functions as quantities or properties of a thermodynamic system, while nonstate functions represent a process during which the state functions change. For example, the state function is proportional to the internal energy of an ideal gas, but the work is the amount of energy transferred as the system performs work. Internal energy is identifiable, it is a particular form of energy. Work is the amount of energy that has changed its form or location.
List of state functions
{{#invoke:see alsoseealso}} The following are considered to be state functions in thermodynamics:
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 Mass (m)
 Energy (E)
 Enthalpy (H)
 Internal energy (U)
 Gibbs free energy (G)
 Helmholtz free energy (A)
 Exergy
 Entropy (S)
 Pressure (p)
 Temperature (T)
 Volume (V)
 Chemical composition
 Specific volume (v) or its reciprocal Density (ρ)
 Fugacity
 Altitude
 Particle number (n_{i})
See also
ar:دالة حالة ca:Funció d'estat cs:Stavová veličina de:Zustandsgröße es:Función de estado eo:Statofunkcio fa:تابع حالت fr:Fonction d'état gl:Función de estado it:Funzione di stato hu:Állapotjelző nl:Toestandsfunctie ja:状態量 pl:Funkcja stanu pt:Função de estado ru:Термодинамическая функция состояния sk:Stavová veličina sv:Tillståndsstorhet tr:Hal fonksiyonu uk:Функція стану zh:态函数