Thermodynamics

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Thermodynamics is the study of energy, its conversions between various forms such as heat, and the ability of energy to do work. It is closely related to statistical mechanics from which many themodynamic relationships can be derived.

It can be argued that thermodynamics was misnamed as it does not actually relate to rates of change as such and therefore would probably have been better called thermostatics as a field. Thermodynamics relates to whether certain chemical reactions are possible but not how quickly they occur.

The field covers a wide range of topics including, but not limited to: efficiency of heat engines and turbines, phase equilibria, PVT relationships. gas laws (both ideal and non ideal), energy balances, heats of reactions, and combustion reactions. It is governed by 4 basic laws (in brief):

Table of contents

1 The Laws of Thermodynamics 2 Basics 2.1 Substances describable by temperature alone 2.2 Substances describable by temperature and pressure alone 2.3 Substances describable by temperature, pressure and chemical potential 2.4 Substances describable by temperature and magnetic field 2.5 Links 3 Thermodynamic Systems 4 Thermodynamic State

The Laws of Thermodynamics

Alternative statements are given for each law. These statements are, for the most part, mathematically equivalent.

• Zeroth law: A fundamental concept within thermodynamics, however, it was not termed a law until after the first three laws were already widely in use, hence the zero numbering. 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.

• 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.
    • A system operating in contact with a thermal reservoir cannot produce positive work in its surroundings (Kelvin)
    • A system operating in a cycle cannot produce a positive heat flow from a colder body to a hotter body (Clausius)
  • 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 goes to 0, the entropy of a system approaches a constant

The three original laws have been humorously summarised as: (1) you can't win; (2) you can't break even; (3) you can't get out of the game.

Basics

This is a brief summary and collection of the major concepts in thermodynamics. To learn more about each, just click on the corresponding links:

U stands for the internal energy, T stands for temperature, S stands for entropy, P stands for pressure, V stands for volume, ρ stands for density, F stands for Helmholtz free energy, H stands for enthalpy, G stands for Gibbs free energy, μ stands for chemical potential and N stands for particle number.

The rest of this discussion is about systems in equilibrium only. For nonequilibrium thermodynamics, see ...

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.

Links

• Helmholtz free energy
• Gibbs free energy
• Entropy
• Enthalpy
• Internal energy
• Temperature
• Pressure
• Volume
• Density
• Phase (matter)
• Chemical potential
• Particle number/density
• Intensive variable
• Extensive variable

Thermodynamic Systems

A thermodynamic system is that part of the universe that is under consideration. A real or imaginary boundary separates the system from the rest of the universe, which is referred to as the surroundings. Often thermodynamic systems are characterized by the nature of this boundary as follows:

• 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 mechanics
• Calorimetry
• Thermal Analysis
• Thermochemistry also known as chemical thermodynamics

See also:

• Partition function (statistical mechanics)