Ideal gas

An ideal gas is a hypothetical gas whose particles have negligible volume and exert no intermolecular forces. Its pressure, volume, amount, and temperature obey the ideal gas law under all conditions.

Ideal gas law: The equation of state PV = nRT relates an ideal gas’s pressure, volume, amount, and absolute temperature. It summarizes the model’s measurable relationships in one equation.
Real gas: A gas whose particles have finite size and interact through intermolecular forces. It reveals the two simplifying assumptions that ideal gases omit.
Pressure: Force exerted per unit area by interactions with a surface. Gas pressure arises from particles colliding with the container walls.
Boyle's law: The inverse relationship between pressure and volume for a fixed amount of gas at constant temperature. It follows from the ideal gas law when temperature and amount are fixed.
Internal energy of an ideal gas: The energy of an ideal gas, determined by temperature and its molecular degrees of freedom. With no intermolecular potential energy, internal energy depends only on molecular motion.
Kinetic theory of gases: A particle model that explains gas properties through the motion and collisions of microscopic constituents. Its assumptions derive the ideal gas law from molecular motion.
van der Waals equation: An equation of state that corrects the ideal gas law for molecular size and attraction. Its correction terms model the departures expected in actual gases.
Volume: The three-dimensional space occupied by a substance or region. It is the container-scale quantity related to pressure and temperature.
Charles's law: The direct relationship between gas volume and absolute temperature at fixed pressure and amount. It is an ideal-gas prediction for heating a gas under constant pressure.
Heat capacity ratio: The ratio of a gas’s heat capacity at constant pressure to its heat capacity at constant volume. It shapes ideal-gas responses during adiabatic expansion and compression.

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