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The ideal gas law is a fundamental equation in thermodynamics that describes the behavior of ideal gases. It relates the pressure, volume, temperature, and amount of a gas to a constant value. The equation is typically expressed as PV = nRT, where P represents pressure, V represents volume, n is the number of moles of gas, R is the ideal gas constant, and T is the absolute temperature.

An ideal gas is a theoretical gas composed of many submicroscopic particles that move randomly according to Newton's laws of motion. The particles themselves are considered to have no volume and exert no intermolecular forces on each other, except for perfectly elastic collisions. While no real gas is truly ideal, the ideal gas law provides a good approximation for the behavior of many gases under conditions of low pressure and high temperature.

The ideal gas constant, R, has a value that depends on the units used for pressure, volume, and temperature. Common values include 8.314 joules per mole-kelvin or 0.0821 liters-atmospheres per mole-kelvin. The ideal gas law is derived from experimental observations and is a consolidation of Boyle's Law, Charles's Law, and Avogadro's Law. It is widely used in chemistry and physics to calculate unknown properties of gases and to understand chemical reactions involving gaseous substances. Deviations from ideal behavior in real gases become significant at high pressures or low temperatures where intermolecular forces and the finite volume of gas molecules become more important.