Conjugate variables (thermodynamics)

Just as a small increment of energy in a mechanical system is the product of a force times a small displacement, so an increment in the energy of a thermodynamic system can be expressed as the sum of the products of certain generalized "forces" which, when unbalanced, cause certain generalized "displacements" to occur, with their product being the energy transferred as a result. These forces and their associated displacements are called conjugate variables.[1] For example, consider the ${\displaystyle pV}$ conjugate pair. The pressure ${\displaystyle p}$ acts as a generalized force: Pressure differences force a change in volume ${\displaystyle \mathrm {d} V}$, and their product is the energy lost by the system due to work. Here, pressure is the driving force, volume is the associated displacement, and the two form a pair of conjugate variables. In a similar way, temperature differences drive changes in entropy, and their product is the energy transferred by heat transfer. The thermodynamic force is always an intensive variable and the displacement is always an extensive variable, yielding an extensive energy. The intensive (force) variable is the derivative of the (extensive) internal energy with respect to the extensive (displacement) variable, with all other extensive variables held constant.

The theory of thermodynamic potentials is not complete until one considers the number of particles in a system as a variable on par with the other extensive quantities such as volume and entropy. The number of particles is, like volume and entropy, the displacement variable in a conjugate pair. The generalized force component of this pair is the chemical potential. The chemical potential may be thought of as a force which, when imbalanced, pushes an exchange of particles, either with the surroundings, or between phases inside the system. In cases where there are a mixture of chemicals and phases, this is a useful concept. For example, if a container holds liquid water and water vapor, there will be a chemical potential (which is negative) for the liquid which pushes the water molecules into the vapor (evaporation) and a chemical potential for the vapor, pushing vapor molecules into the liquid (condensation). Only when these "forces" equilibrate, and the chemical potential of each phase is equal, is equilibrium obtained.

The most commonly considered conjugate thermodynamic variables are (with corresponding SI units):

Thermal parameters:

• Temperature: ${\displaystyle T}$  (K)
• Entropy: ${\displaystyle S}$  (J K⁻¹)

Mechanical parameters:

• Pressure: ${\displaystyle p}$  (Pa= J m⁻³)
• Volume: ${\displaystyle V}$  (m³ = J Pa⁻¹)

or, more generally,

• Stress: ${\displaystyle \sigma _{ij}\,}$ (Pa= J m⁻³)
• Volume × Strain: ${\displaystyle V\times \varepsilon _{ij}}$ (m³ = J Pa⁻¹)

Material parameters:

• chemical potential: ${\displaystyle \mu }$ (J)
• particle number: ${\displaystyle N}$   (particles or mole)

For a system with different types ${\displaystyle i}$ of particles, a small change in the internal energy is given by:

${\displaystyle \mathrm {d} U=T\,\mathrm {d} S-p\,\mathrm {d} V+\sum _{i}\mu _{i}\,\mathrm {d} N_{i}\,,}$

where ${\displaystyle U}$ is internal energy, ${\displaystyle T}$ is temperature, ${\displaystyle S}$ is entropy, ${\displaystyle p}$ is pressure, ${\displaystyle V}$ is volume, ${\displaystyle \mu _{i}}$ is the chemical potential of the ${\displaystyle i}$-th particle type, and ${\displaystyle N_{i}}$ is the number of ${\displaystyle i}$-type particles in the system.

Here, the temperature, pressure, and chemical potential are the generalized forces, which drive the generalized changes in entropy, volume, and particle number respectively. These parameters all affect the internal energy of a thermodynamic system. A small change ${\displaystyle \mathrm {d} U}$ in the internal energy of the system is given by the sum of the flow of energy across the boundaries of the system due to the corresponding conjugate pair. These concepts will be expanded upon in the following sections.

While dealing with processes in which systems exchange matter or energy, classical thermodynamics is not concerned with the rate at which such processes take place, termed kinetics. For this reason, the term thermodynamics is usually used synonymously with equilibrium thermodynamics. A central notion for this connection is that of quasistatic processes, namely idealized, "infinitely slow" processes. Time-dependent thermodynamic processes far away from equilibrium are studied by non-equilibrium thermodynamics. This can be done through linear or non-linear analysis of irreversible processes, allowing systems near and far away from equilibrium to be studied, respectively.

As an example, consider the ${\displaystyle pV}$ conjugate pair. The pressure acts as a generalized force – pressure differences force a change in volume, and their product is the energy lost by the system due to mechanical work. Pressure is the driving force, volume is the associated displacement, and the two form a pair of conjugate variables.

The above holds true only for non-viscous fluids. In the case of viscous fluids, plastic and elastic solids, the pressure force is generalized to the stress tensor, and changes in volume are generalized to the volume multiplied by the strain tensor.[2] These then form a conjugate pair. If ${\displaystyle \sigma _{ij}}$ is the ij component of the stress tensor, and ${\displaystyle \varepsilon _{ij}}$ is the ij component of the strain tensor, then the mechanical work done as the result of a stress-induced infinitesimal strain ${\displaystyle \mathrm {\varepsilon } _{ij}}$ is:

${\displaystyle \delta w=V\sum _{ij}\sigma _{ij}\,\mathrm {d} \varepsilon _{ij}}$

or, using Einstein notation for the tensors, in which repeated indices are assumed to be summed:

${\displaystyle \delta w=V\sigma _{ij}\,\mathrm {d} \varepsilon _{ij}}$

In the case of pure compression (i.e. no shearing forces), the stress tensor is simply the negative of the pressure times the unit tensor so that

${\displaystyle \delta w=V\,(-p\delta _{ij})\,\mathrm {d} \varepsilon _{ij}=-\sum _{k}pV\,\mathrm {d} \varepsilon _{kk}}$

The trace of the strain tensor (${\displaystyle \varepsilon _{kk}}$) is the fractional change in volume so that the above reduces to ${\displaystyle \delta w=-p\mathrm {d} V}$ as it should.

In a similar way, temperature differences drive changes in entropy, and their product is the energy transferred by heating. Temperature is the driving force, entropy is the associated displacement, and the two form a pair of conjugate variables. The temperature/entropy pair of conjugate variables is the only heat term; the other terms are essentially all various forms of work.

The chemical potential is like a force which pushes an increase in particle number. In cases where there are a mixture of chemicals and phases, this is a useful concept. For example, if a container holds water and water vapor, there will be a chemical potential (which is negative) for the liquid, pushing water molecules into the vapor (evaporation) and a chemical potential for the vapor, pushing vapor molecules into the liquid (condensation). Only when these "forces" equilibrate is equilibrium obtained.

• Generalized coordinate and generalized force: analogous conjugate variable pairs found in classical mechanics.
• Intensive and extensive properties
• Bond graph

• Lewis, Gilbert Newton; Randall, Merle (1961). Thermodynamics. Revised by Kenneth S. Pitzer and Leo Brewer (2nd ed.). New York City: McGraw-Hill Book. ISBN 9780071138093.
• Callen, Herbert B. (1998). Thermodynamics and an Introduction to Thermostatistics (2nd ed.). New York: John Wiley & Sons. ISBN 978-0-471-86256-7.