Gas laws

Gas laws are equations relating a gas’s pressure, volume, temperature, and amount. They describe how these properties change together under specified conditions.

Ideal gas law: An equation of state, PV = nRT, relating pressure, volume, temperature, and amount for an ideal gas. Combines the main gas variables in one equation of state.
Pressure: Pressure is force exerted per unit area by impacts or other stresses. Gas pressure arises from particles striking the container walls.
Standard temperature and pressure: A reference set of temperature and pressure conditions used to report and compare gas properties. Provides conventions for comparing gas volumes measured under different conditions.
Real gas: A gas whose particles have finite size and interact with one another. Real gases depart from ideal gas-law predictions at high pressures and low temperatures.
Boyle's law: At constant temperature and amount, a gas’s pressure varies inversely with its volume. Isolates the pressure–volume relationship when temperature is fixed.
Volume: Volume is the three-dimensional space occupied by a substance or region. Gas laws track how the space available to a gas changes.
Molar volume: The volume occupied by one mole of a substance under specified conditions. Gas laws let molar volume be calculated from pressure and temperature.
Van der Waals equation: An equation of state that adjusts the ideal gas law for molecular size and intermolecular attraction. Corrects two assumptions behind the ideal-gas approximation.
Charles's law: At constant pressure and amount, a gas’s volume is proportional to its absolute temperature. Shows how heating changes volume when pressure is held constant.
Temperature: Temperature measures a system’s thermal state and determines the direction of heat transfer. Gas-law proportionalities use absolute temperature, measured in kelvins.

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