# Thermodynamics

zh-cn:热力学
**Thermodynamics** is the study of energy, its conversions between various forms, the ability of energy to do work, and the spontaneity of processes. It is closely related to statistical mechanics from which many thermodynamic relationships can be derived. It is not concerned with the concept of time, or that of rate of change (derivative in time). As a result, it has been suggested that this science should rather have been called *thermostatics*.

## The Laws of Thermodynamics

- Zeroth law: Considered to be more fundamental than the other three laws, it was not termed a law until after the others were already in use, hence the number 'zero'. There is some discussion about its status. Stated as:
- If each of two systems is in thermal equilibrium with a third system, all must be in equilibrium with each other.

- If each of two systems is in thermal equilibrium with a third system, all must be in equilibrium with each other.
- 1st Law: Is stated as follows:
- Energy can neither be created nor destroyed only changed.
- The heat flowing into a system equals the sum of change in internal energy plus the work done by the system.
- The work exchanged in an adiabatic process depends only on the initial and the final state and not on the details of the process.
- The sum of heat flowing into a system and work done by the system is zero.

- 2nd Law: A far reaching and powerful law, it can be stated many ways, the most popular of which is:
- It is impossible to obtain a process such that the unique effect is the subtraction of a positive heat from a reservoir and the production of a positive work.
- The entropy of a closed system never decreases (see Maxwell's demon)

- 3rd Law: This law explains why it is so hard to cool something to absolute zero:
- All processes cease as temperature approaches zero.
- As temperature approaches to 0, the entropy of a system approaches a constant.

## Basics

The following is a list of the major concepts in thermodynamics, together with the algebraic symbols used to represent them.

- Internal energy U
- Temperature T
- Entropy S
- Pressure P
- Volume V
- Density &rho
- Helmholtz free energy F
- Gibbs free energy G
- Enthalpy H
- Chemical potential &mu
- Particle number N
- Phase (matter)
- Particle number/density
- Intensive variable
- Extensive variable
- State function

### Substances describable by temperature alone

Blackbody radiation is an example. The reason why this is the case is because photon number isn't conserved. The state is completely described by its temperature except at phase transitions and perhaps spontaneous symmetry breaking in the ordered phase. given the internal energy as a function of temperature, we can define F=U-TS.### Substances describable by temperature and pressure alone

Most "pure" nonmagnetic substances fall into this category. This state is completely described by its temperature and pressure, except at phase transitions and perhaps spontaneous symmetry breaking in the ordered phase. Given U and V (or the density ρ) as a function of T and P, we can define the Helmholtz energy as before and the Gibbs energy as G=U-TS+PV and the enthalpy as H=U+PV.### Substances describable by temperature, pressure and chemical potential

If there are more than one kind of atom/molecule, a substance would fall into this category. This state is completely described by its temperature, pressure and chemical potentials, except at phase transitions and perhaps spontaneous symmetry breaking in the ordered phase.### Substances describable by temperature and magnetic field

If a substance is a ferromagnet or a superconductor, for example, it would fall into this category. It is completely described by its temperature and magnetic field, except at phase transitions and perhaps spontaneous symmetry breaking in the ordered phase.## Thermodynamic Systems

- Isolated systems are completely isolated from their surroundings. Neither heat nor matter can be exchanged between the system and the surroundings. An example of an isolated system would be an insulated container, such as an insulated gas cylinder. (In reality, a system can never be absolutely isolated from its environment, because there is always at least some slight coupling, even if only via minimal gravitational attraction).
- Closed systems are separated from the surroundings by an impermeable barrier. Heat can be exchanged between the system and the surroundings, but matter cannot. A greenhouse is an example of a closed system.
- Open systems can exchange both heat and matter with their surroundings. Portions of the boundary between the open system and its surroundings may be impermeable and/or adiabatic, however at least part of this boundary is subject to heat and mass exchange with the surroundings. The ocean would be an example of an open system.

## Thermodynamic State

A key concept in thermodynamics is the *state of a system*. When a system is at equilibrium under a given set of conditions, it is said to be in a definite *state*. For a given thermodynamic state, many of the system's properties have a specific value corresponding to that state. The values of these properties are a function of the state of the system and are independent of the path by which the system arrived at that state. The number of properties that must be specified to describe the state of a given system is given by Gibbs phase rule. Since the state can be described by specifying a small number of properties, while the values of many properties are determined by the state of the system, it is possible to develop relationships between the various state properties. One of the main goals of Thermodynamics is to understand these relationships between the various state properties of a system. Equations of state are examples of some of these relationships.

See also: thermodynamic properties

Thermodynamics also touches upon the fields of:

- Phase Equilibria
- Fluid dynamics
- Calorimetry
- Thermal Analysis
- Thermochemistry also known as chemical thermodynamics

- Partition function (statistical mechanics)
- list of thermodynamics topics