![Table of thermodynamic equations Table of thermodynamic equations](/modules/owlapps_apps/img/nopic.jpg)
Common thermodynamic equations and quantities in thermodynamics, using mathematical notation, are as follows:
Many of the definitions below are also used in the thermodynamics of chemical reactions.
The equations in this article are classified by subject.
Below are useful results from the Maxwell–Boltzmann distribution for an ideal gas, and the implications of the Entropy quantity. The distribution is valid for atoms or molecules constituting ideal gases.
Corollaries of the non-relativistic Maxwell–Boltzmann distribution are below.
For quasi-static and reversible processes, the first law of thermodynamics is:
where δQ is the heat supplied to the system and δW is the work done by the system.
The following energies are called the thermodynamic potentials,
and the corresponding fundamental thermodynamic relations or "master equations" are:
The four most common Maxwell's relations are:
More relations include the following.
Other differential equations are:
where N is number of particles, h is Planck's constant, I is moment of inertia, and Z is the partition function, in various forms:
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