Table of thermodynamic equations
This article is a summary of common equations and quantities in thermodynamics (see thermodynamic equations for more elaboration). Definitions. Many of the definitions below are also used in the thermodynamics of chemical reactions. Equations. The equations in this article are classified by subject. Statistical physics. 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. Quasi-static and reversible processes. For quasi-static and reversible  processes, the first law of thermodynamics is: where δ"Q" is the heat supplied "to" the system and δ"W" is the work done "by" the system. Thermodynamic potentials. The following energies are called the thermodynamic potentials, and the corresponding fundamental thermodynamic relations or "master equations" are: Maxwell's relations. The four most common Maxwell's relations are: More relations include the following. Other differential equations are: Quantum properties. 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: