| Thermodynamics | ||||||||||||
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Athermodynamic potential (or more accurately, athermodynamic potential energy)[1][2] is ascalar quantity used to represent thethermodynamic state of asystem. Just as inmechanics, wherepotential energy is defined as capacity to do work, similarly different potentials have different meanings. The concept of thermodynamic potentials was introduced byPierre Duhem in 1886.Josiah Willard Gibbs in his papers used the termfundamentalfunctions. Effects of changes in thermodynamic potentials can sometimes be measured directly, while their absolute magnitudes can only be assessed using computational chemistry or similar methods.[3]
One main thermodynamic potential that has a physical interpretation is theinternal energyU. It is the energy of configuration of a given system ofconservative forces (that is why it is called potential) and only has meaning with respect to a defined set of references (or data). Expressions for all other thermodynamic energy potentials are derivable viaLegendre transforms from an expression forU. In other words, each thermodynamic potential is equivalent to other thermodynamic potentials; each potential is a different expression of the others.
Inthermodynamics, external forces, such asgravity, are counted as contributing to total energy rather than to thermodynamic potentials. For example, theworking fluid in asteam engine sitting on top ofMount Everest has higher total energy due to gravity than it has at the bottom of theMariana Trench, but the same thermodynamic potentials. This is because thegravitational potential energy belongs to the total energy rather than to thermodynamic potentials such as internal energy.
Five common thermodynamic potentials are:[4]
| Name | Symbol | Formula | Natural variables |
|---|---|---|---|
| Internal energy | |||
| Helmholtz free energy | |||
| Enthalpy | |||
| Gibbs free energy | |||
| Landau potential, or grand potential | , |
whereT =temperature,S =entropy,p =pressure,V =volume.Ni is the number of particles of typei in the system andμi is thechemical potential for ani-type particle. The set of allNi are also included as natural variables but may be ignored when no chemical reactions are occurring which cause them to change. The Helmholtz free energy is in ISO/IEC standard called Helmholtz energy[1] or Helmholtz function. It is often denoted by the symbolF, but the use ofA is preferred byIUPAC,[5]ISO andIEC.[6]
These five common potentials are all potential energies, but there are alsoentropy potentials. Thethermodynamic square can be used as a tool to recall and derive some of the potentials.
Just as inmechanics, wherepotential energy is defined as capacity to do work, similarly different potentials have different meanings like the below:
From these meanings (which actually apply in specific conditions, e.g. constant pressure, temperature, etc.), for positive changes (e.g.,ΔU > 0), we can say thatΔU is the energy added to the system,ΔF is the total work done on it,ΔG is the non-mechanical work done on it, andΔH is the sum of non-mechanical work done on the system and the heat given to it.
Note that the sum of internal energy is conserved, but the sum of Gibbs energy, or Helmholtz energy, are not conserved, despite being named "energy". They can be better interpreted as the potential to perform "useful work", and the potential can be wasted.[7]
Thermodynamic potentials are very useful when calculating theequilibrium results of a chemical reaction, or when measuring the properties of materials in a chemical reaction. The chemical reactions usually take place under some constraints such as constant pressure and temperature, or constant entropy and volume, and when this is true, there is a corresponding thermodynamic potential that comes into play. Just as in mechanics, the system will tend towards a lower value of a potential and at equilibrium, under these constraints, the potential will take the unchanging minimum value. The thermodynamic potentials can also be used to estimate the total amount of energy available from a thermodynamic system under the appropriate constraint.
In particular: (seeprinciple of minimum energy for a derivation)[8]
For each thermodynamic potential, there are thermodynamic variables that need to be held constant to specify the potential value at a thermodynamical equilibrium state, such as independent variables for a mathematical function. These variables are termed thenatural variables of that potential.[9] The natural variables are important not only to specify the potential value at the equilibrium, but also because if a thermodynamic potential can be determined as a function of its natural variables, all of the thermodynamic properties of the system can be found by taking partial derivatives of that potential with respect to its natural variables and this is true for no other combination of variables. If a thermodynamic potential is not given as a function of its natural variables, it will not, in general, yield all of the thermodynamic properties of the system.
The set of natural variables for each of the above four thermodynamic potentials is formed from a combination of theT,S,p,V variables, excluding any pairs ofconjugate variables; there is no natural variable set for a potential including theT-S orp-V variables together as conjugate variables for energy. An exception for this rule is theNi −μi conjugate pairs as there is no reason to ignore these in the thermodynamic potentials, and in fact we may additionally define the four potentials for each species.[10] UsingIUPAC notation in which the brackets contain the natural variables (other than the main four), we have:
| Thermodynamic potential name | Formula | Natural variables |
|---|---|---|
| Internal energy | ||
| Helmholtz free energy | ||
| Enthalpy | ||
| Gibbs energy |
If there is only one species, then we are done. But, if there are, say, two species, then there will be additional potentials such as and so on. If there areD dimensions to the thermodynamic space, then there are2D unique thermodynamic potentials. For the most simple case, a single phase ideal gas, there will be three dimensions, yielding eight thermodynamic potentials.
The definitions of the thermodynamic potentials may be differentiated and, along with the first and second laws of thermodynamics, a set of differential equations known as thefundamental equations follow.[11] (Actually they are all expressions of the same fundamental thermodynamic relation, but are expressed in different variables.) By thefirst law of thermodynamics, any differential change in the internal energyU of a system can be written as the sum of heat flowing into the system subtracted by the work done by the system on the environment, along with any change due to the addition of new particles to the system:
whereδQ is theinfinitesimal heat flow into the system, andδW is the infinitesimal work done by the system,μi is thechemical potential of particle typei andNi is the number of the typei particles. (NeitherδQ norδW areexact differentials, i.e., they are thermodynamic process path-dependent. Small changes in these variables are, therefore, represented withδ rather thand.)
By thesecond law of thermodynamics, we can express the internal energy change in terms of state functions and their differentials. In case of reversible changes we have:
where
and the equality holds for reversible processes.
This leads to the standard differential form of the internal energy in case of a quasistatic reversible change:
SinceU,S andV are thermodynamic functions of state (also called state functions), the above relation also holds for arbitrary non-reversible changes. If the system has more external variables than just the volume that can change, the fundamental thermodynamic relation generalizes to:
Here theXi are thegeneralized forces corresponding to the external variablesxi.[12]
ApplyingLegendre transforms repeatedly, the following differential relations hold for the four potentials (fundamental thermodynamic equations or fundamental thermodynamic relation):
The infinitesimals on the right-hand side of each of the above equations are of the natural variables of the potential on the left-hand side. Similar equations can be developed for all of the other thermodynamic potentials of the system. There will be one fundamental equation for each thermodynamic potential, resulting in a total of2D fundamental equations.
The differences between the four thermodynamic potentials can be summarized as follows:
We can use the above equations to derive some differential definitions of some thermodynamic parameters. If we defineΦ to stand for any of the thermodynamic potentials, then the above equations are of the form:
wherexi andyi are conjugate pairs, and theyi are the natural variables of the potentialΦ. From thechain rule it follows that:
where{yi ≠ j} is the set of all natural variables ofΦ exceptyj that are held as constants. This yields expressions for various thermodynamic parameters in terms of the derivatives of the potentials with respect to their natural variables. These equations are known asequations of state since they specify parameters of thethermodynamic state.[13] If we restrict ourselves to the potentialsU (Internal energy),F (Helmholtz energy),H (Enthalpy) andG (Gibbs energy), then we have the following equations of state (subscripts showing natural variables that are held as constants):
where, in the last equation,ϕ is any of the thermodynamic potentials (U,F,H, orG), and are the set of natural variables for that potential, excludingNi. If we use all thermodynamic potentials, then we will have more equations of state such as
and so on. In all, if the thermodynamic space isD dimensions, then there will beD equations for each potential, resulting in a total ofD 2D equations of state because2D thermodynamic potentials exist. If theD equations of state for a particular potential are known, then the fundamental equation for that potential (i.e., theexact differential of the thermodynamic potential) can be determined. This means that all thermodynamic information about the system will be known because the fundamental equations for any other potential can be found via theLegendre transforms and the corresponding equations of state for each potential as partial derivatives of the potential can also be found.
The above equations of state suggest methods to experimentally measure changes in the thermodynamic potentials using physically measurable parameters. For example the free energy expressions
and
can be integrated at constant temperature and quantities to obtain:
which can be measured by monitoring the measurable variables of pressure, temperature and volume. Changes in the enthalpy and internal energy can be measured bycalorimetry (which measures the amount of heatΔQ released or absorbed by a system). The expressions
can be integrated:
Note that these measurements are made at constant {Nj } and are therefore not applicable to situations in which chemical reactions take place.
Again, definexi andyi to be conjugate pairs, and theyi to be the natural variables of some potentialΦ. We may take the "cross differentials" of the state equations, which obey the following relationship:
From these we get theMaxwell relations.[4][14] There will be(D − 1)/2 of them for each potential giving a total ofD(D − 1)/2 equations in all. If we restrict ourselves theU,F,H,G
Using the equations of state involving the chemical potential we get equations such as:
and using the other potentials we can get equations such as:
Again, definexi andyi to be conjugate pairs, and theyi to be the natural variables of the internal energy.Since all of the natural variables of the internal energyU areextensive quantities
it follows fromEuler's homogeneous function theorem that the internal energy can be written as:
From the equations of state, we then have:
This formula is known as anEuler relation, because Euler's theorem on homogeneous functions leads to it.[15][16] (It was not discovered byEuler in an investigation of thermodynamics, which did not exist in his day.).
Substituting into the expressions for the other main potentials we have:
As in the above sections, this process can be carried out on all of the other thermodynamic potentials. Thus, there is another Euler relation, based on the expression of entropy as a function of internal energy and other extensive variables. Yet other Euler relations hold for other fundamental equations for energy or entropy, as respective functions of other state variables including some intensive state variables.[17]
Deriving theGibbs–Duhem equation from basic thermodynamic state equations is straightforward.[11][18][19] Equating any thermodynamic potential definition with its Euler relation expression yields:
Differentiating, and using the second law:
yields:
Which is the Gibbs–Duhem relation. The Gibbs–Duhem is a relationship among the intensive parameters of the system. It follows that for a simple system withI components, there will beI + 1 independent parameters, or degrees of freedom. For example, a simple system with a single component will have two degrees of freedom, and may be specified by only two parameters, such as pressure and volume for example. The law is named afterJosiah Willard Gibbs andPierre Duhem.
As theinternal energy is aconvex function of entropy and volume, the stability condition requires that the second derivative ofinternal energy withentropy or volume to be positive. It is commonly expressed as. Since the maximum principle of entropy is equivalent to minimum principle of internal energy, the combined criteria for stability or thermodynamic equilibrium is expressed as and for parameters, entropy and volume. This is analogous to and condition for entropy at equilibrium.[20] The same concept can be applied to the various thermodynamic potentials by identifying if they areconvex orconcave of respective their variables.
and
Where Helmholtz energy is a concave function of temperature and convex function of volume.
and
Where enthalpy is a concave function of pressure and convex function of entropy.
and
Where Gibbs potential is a concave function of both pressure and temperature.
In general the thermodynamic potentials (theinternal energy and itsLegendre transforms), areconvex functions of theirextrinsic variables andconcave functions ofintrinsic variables. The stability conditions impose that isothermal compressibility is positive and that for non-negative temperature,.[21]
Changes in these quantities are useful for assessing the degree to which a chemical reaction will proceed. The relevant quantity depends on the reaction conditions, as shown in the following table.Δ denotes the change in the potential and at equilibrium the change will be zero.
| ConstantV | Constantp | |
|---|---|---|
| ConstantS | ΔU | ΔH |
| ConstantT | ΔF | ΔG |
Most commonly one considers reactions at constantp andT, so the Gibbs free energy is the most useful potential in studies of chemical reactions.
| Theory |  | |
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| Statistical thermodynamics | ||
| Models | ||
| Mathematical approaches | ||
| Critical phenomena | ||
| Entropy | ||
| Applications | ||
| International | |
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| National | |
| Other | |
