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Thermodynamic process

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Title: Thermodynamic process  
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Thermodynamic process

A thermodynamic process is a passage of a thermodynamic system from an initial state to a final state. In equilibrium thermodynamics, the initial and final states are states of internal thermodynamic equilibrium, each respectively fully specified by a suitable set of thermodynamic state variables, that depend only on the current state of the system, not the path taken to reach that state. In general, in a thermodynamic process, the system passes through physical states which are not describable as thermodynamic states, because they are far from internal thermodynamic equilibrium. It is possible, however, that a process may take place slowly or smoothly enough to allow its description to be usefully approximated by a continuous path of thermodynamic states. Then it may be approximately described by a process function that does depend on the path.


  • Overview 1
  • Conjugate variable processes 2
  • Thermodynamic potentials 3
  • Polytropic processes 4
  • Main classes of process 5
    • Natural process 5.1
    • Fictively reversible process 5.2
    • Unnatural process 5.3
    • Quasistatic process 5.4
  • See also 6
  • References 7
  • Further reading 8


An example of a series of thermodynamic processes which make up the Stirling cycle

A thermodynamic process can be visualized by graphically plotting the changes to the system's state variables. In the example, four processes are shown. Each process has a well-defined start and end point in the pressure-volume state space. In this particular example, processes 1 and 3 are isothermal, whereas processes 2 and 4 are isochoric. The PV diagram is a particularly useful visualization of a process, because the area under the curve of a process is the amount of work done by the system during that process. Thus work is considered to be a process variable, as its exact value depends on the particular path taken between the start and end points of the process. Similarly, heat may be transferred during a process, and it too is a process variable. In contrast, pressure and volume (as well as numerous other properties) are considered state variables because their values depend only on the position of the start and end points, not the particular path between them.

Conjugate variable processes

It is often useful to group processes into pairs, in which each variable held constant is one member of a conjugate pair.

Pressure - volume

The pressure-volume conjugate pair is concerned with the transfer of mechanical or dynamic energy as the result of work.

  • An isobaric process occurs at constant pressure. An example would be to have a movable piston in a cylinder, so that the pressure inside the cylinder is always at atmospheric pressure, although it is isolated from the atmosphere. In other words, the system is dynamically connected, by a movable boundary, to a constant-pressure reservoir.
  • An isochoric process is one in which the volume is held constant, meaning that the work done by the system will be zero. It follows that, for the simple system of two dimensions, any heat energy transferred to the system externally will be absorbed as internal energy. An isochoric process is also known as an isometric process or an isovolumetric process. An example would be to place a closed tin can containing only air into a fire. To a first approximation, the can will not expand, and the only change will be that the gas gains internal energy, as evidenced by its increase in temperature and pressure. Mathematically, \delta Q=dU. The system is dynamically insulated, by a rigid boundary, from the environment.

Temperature - entropy

The temperature-entropy conjugate pair is concerned with the transfer of thermal energy as the result of heating.

  • An isothermal process occurs at a constant temperature. An example would be to have a system immersed in a large constant-temperature bath. Any work energy performed by the system will be lost to the bath, but its temperature will remain constant. In other words, the system is thermally connected, by a thermally conductive boundary to a constant-temperature reservoir.
  • An adiabatic process is a process in which there is no energy added or subtracted from the system by heating or cooling. For a reversible process, this is identical to an isentropic process. The system is thermally insulated from its environment and that its boundary is a thermal insulator. If a system has an entropy which has not yet reached its maximum equilibrium value, the entropy will increase even though the system is thermally insulated. Under certain conditions two states of a system may be considered adiabatically accessible.
  • An isentropic process occurs at a constant entropy. For a reversible process this is identical to an adiabatic process. If a system has an entropy which has not yet reached its maximum equilibrium value, a process of cooling may be required to maintain that value of entropy.

Chemical potential - particle number

The processes above have all implicitly assumed that the boundaries are also impermeable to particles. We may assume boundaries that are rigid, but are permeable to one or more types of particle. Similar considerations then hold for the chemical potentialparticle number conjugate pair, which is concerned with the transfer of energy via this transfer of particles.

  • In a constant chemical potential process the system is particle-transfer connected, by a particle-permeable boundary, to a constant-µ reservoir.
  • In a constant particle number process there is no energy added or subtracted from the system by particle transfer. The system is particle-transfer-insulated from its environment by a boundary that is impermeable to particles, but permissive of transfers of energy as work or heat. These processes are the ones by which thermodynamic work and heat are defined, and for them, the system is said to be closed.

Thermodynamic potentials

Any of the thermodynamic potentials may be held constant during a process. For example:

Polytropic processes

A polytropic process is a thermodynamic process that obeys the relation:

P V^{\,n} = C,

where P is the pressure, V is volume, n is any real number (the "polytropic index"), and C is a constant. This equation can be used to accurately characterize processes of certain systems, notably the compression or expansion of a gas, but in some cases, liquids and solids.

Main classes of process

According to Planck, one may think of three main classes of thermodynamic process: natural, fictively reversible, and impossible or unnatural.[1][2]

Natural process

Only natural processes occur in nature. For thermodynamics, a natural process is a transfer between systems that increases the sum of their entropies, and is irreversible.[1] Natural processes may occur spontaneously, or may be triggered in a metastable or unstable system, as for example in the condensation of a supersaturated vapour.[3]

Fictively reversible process

To describe the geometry of graphical surfaces that illustrate equilibrium relations between thermodynamic functions of state, one can fictively think of so-called "reversible processes". They are convenient theoretical objects that trace paths across graphical surfaces. They are called "processes" but do not describe natural processes, which are always irreversible. Because the points on the paths are points of thermodynamic equilibrium, it is customary to think of the "processes" described by the paths as fictively "reversible"..[1]

Unnatural process

Unnatural processes are logically conceivable but do not occur in nature. They would decrease the sum of the entropies if they occurred.[1]

Quasistatic process

A quasistatic process is an idealized or fictive model of a thermodynamic "process" considered in theoretical studies. It does not occur in physical reality. It may be imagined as happening infinitely slowly so that the system passes through a continuum of states that are infinitesimally close to equilibrium. The fictive "process" can be regarded as reversible.

See also


  1. ^ a b c d Guggenheim, E.A. (1949/1967). Thermodynamics. An Advanced Treatment for Chemists and Physicists, fifth revised edition, North-Holland, Amsterdam, p. 12.
  2. ^ Tisza, L. (1966). Generalized Thermodynamics, M.I.T. Press, Cambridge MA, p. 32.
  3. ^ Planck, M.(1897/1903). , translated by A. Ogg, Longmans, Green & Co., LondonTreatise on Thermodynamics, p. 82.

Further reading

  • Physics for Scientists and Engineers - with Modern Physics (6th Edition), P. A. Tipler, G. Mosca, Freeman, 2008, ISBN 0-7167-8964-7
  • Encyclopaedia of Physics (2nd Edition), R.G. Lerner, G.L. Trigg, VHC publishers, 1991, ISBN 3-527-26954-1 (Verlagsgesellschaft), ISBN 0-89573-752-3 (VHC Inc.)
  • McGraw Hill Encyclopaedia of Physics (2nd Edition), C.B. Parker, 1994, ISBN 0-07-051400-3
  • Physics with Modern Applications, L.H. Greenberg, Holt-Saunders International W.B. Saunders and Co, 1978, ISBN 0-7216-4247-0
  • Essential Principles of Physics, P.M. Whelan, M.J. Hodgeson, 2nd Edition, 1978, John Murray, ISBN 0-7195-3382-1
  • Thermodynamics, From Concepts to Applications (2nd Edition), A. Shavit, C. Gutfinger, CRC Press (Taylor and Francis Group, USA), 2009, ISBN 9781420073683
  • Chemical Thermodynamics, D.J.G. Ives, University Chemistry, Macdonald Technical and Scientific, 1971, ISBN 0-356-03736-3
  • Elements of Statistical Thermodynamics (2nd Edition), L.K. Nash, Principles of Chemistry, Addison-Wesley, 1974, ISBN 0-201-05229-6
  • Statistical Physics (2nd Edition), F. Mandl, Manchester Physics, John Wiley & Sons, 2008, ISBN 9780471915331
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