# Work (thermodynamics)

### 2007 Schools Wikipedia Selection. Related subjects: General Physics

Thermodynamic potentials | |
---|---|

Internal energy | U(S,V) |

Helmholtz free energy | A(T,V) = U − TS |

Enthalpy | H(S,P) = U + PV |

Gibbs free energy | G(T,P) = U + PV − TS |

In thermodynamics, **thermodynamic work** is the quantity of energy transferred from one system to another. It is a generalization of the concept of mechanical work in mechanics. In the SI system of measurement, work is measured in joules (symbol: J). The rate at which work is performed is power.

## History

### 1824

The modern-day definition of work, i.e. "weight *lifted* through a height", was originally defined in 1824 by thermodynamicist Sadi Carnot in his famous paper *Reflections on the Motive Power of Fire*. Specifically, according to Carnot:

We use here motive power (work) to express the useful effect that a motor is capable of producing. This effect can always be likened to the elevation of a weight to a certain height. It has, as we know, as a measure, the product of the weight multiplied by the height to which it is raised. |

### 1845

In 1845, the English physicist James Joule read a paper *On the mechanical equivalent of heat* to the British Association meeting in Cambridge. In this work, he reported his best-known experiment, that in which the work released through the action of a "weight *falling* through a height" was used to turn a paddle-wheel in an insulated barrel of water.

In this experiment, the friction and agitation of action the paddle-wheel on the body of water caused heat to be generated which, in turn, increased the temperature of water. Both the temperature ∆T change of the water and the height of the fall ∆h of the weight mg were recorded. Using these values, Joule was able to determine the mechanical equivalent of heat. Joule estimated a mechanical equivalent of heat to be 819 ft•lbf/Btu (4.41 J/cal). The modern day definitions of heat, work, temperature, and energy all have connection to this experiment.

## Overview

According to the * First Law of Thermodynamics*, it is useful to separate changes to the internal energy of a thermodynamic system into two sorts of energy transfers. **Work** refers to forms of energy transfer, which can be accounted for in terms of changes in the *macroscopic* physical variables of the system, for example energy which goes into expanding the volume of a system against an external pressure, by say driving a piston-head out of a cylinder against an external force. This is in distinction to **heat** energy carried into or out of the system in the form of transfers in the *microscopic* thermal motions of particles.

The concept of thermodynamic work is a little more general than that of mechanical work, because it also includes other energy transfers, i.e. for example electrical work, the movement of charge against an external electrical field to charge up a battery say, which may or may not necessarily be thought of as strictly mechanical in nature.

## Mathematical definition

As stipulated to the First Law of Thermodynamics, any net increase in the internal energy *U* of a thermodynamic system must be fully accounted for, in terms of heat *δQ* entering the system less work *δW* done *by* the system:

The Roman letter *d* indicates that internal energy *U* is a property of the state of the system, so changes in the internal energy are exact differentials - they depend only on the original state and the final state, not the path taken. In contrast the Greek δs in this equation reflect the fact that the heat transfer and the work transfer are *not* properties of the final state of the system. Given only the initial state and the final state of the system, all one can say is what the total change in internal energy was, not how much of the energy went out as heat, and how much as work. This can be summarised by saying that heat and work are not state functions of the system.

## Pressure-volume work

Chemical thermodynamics studies *PV work*, which occurs when the volume of a fluid changes. PV work is represented by the following differential equation:

where:

*W*= work done on the system*P*= external pressure*V*= volume

Therefore, we have:

Like all work functions, PV work is path-dependent. (The path in question is a curve in the Euclidean space specified by the fluid's pressure and volume, and infinitely many such curves are possible.) From a thermodynamic perspective, this fact implies that *PV* work is not a state function. This means that the differential *d**W* is an inexact differential; to be more rigorous, it should be written đW (with a line through the d).

From a mathematical point of view, that is to say, *d**W* is not an exact one-form. This line through is merely a flag to warn us there is actually no function ( 0-form) *W* which is the potential of *d**W*. If there were, indeed, this function *W*, we should be able to just use Stokes Theorem, and evaluate this putative function, the potential of *d**W*, at the boundary of the path, that is, the initial and final points, and therefore the work would be a state function. This impossibility is consistent with the fact that it does not make sense to refer to *the work on a point*; work presupposes a path.

PV work is often measured in the (non-SI) units of litre-atmospheres, where 1 L·atm = 101.3 J.

## Free energy and exergy

The amount of useful work which *can* be extracted from a thermodynamic system is discussed in the article * Second Law of Thermodynamics*. Under many practical situations this can be represented by the thermodynamic Availability or Exergy function. Two important cases are thermodynamic systems where the temperature and volume are held constant in which the measure of "useful" work attainable reduces to the Helmholtz free energy function; and systems where the temperature and pressure are held constant in which the measure of "useful" work attainable reduces to the Gibbs free energy.