The laws of Boyle, Charles , and Gay

Boyle's Law: Pressure (P) of a gas is inversely proportional to its volume (V) at constant temperature: P ∝ 1/V. Reduced volume increases molecular collisions, raising pressure while temperature remains constant.

Charles's Law: Volume (V) of a gas is directly proportional to its absolute temperature (T) at constant pressure: V ∝ T. Increased temperature raises molecular motion, causing gas to expand.

Gay-Lussac's Law: Pressure (P) of a gas is directly proportional to its absolute temperature (T) at constant volume: P ∝ T. Higher temperature increases molecular motion, leading to more forceful collisions and increased pressure without volume change.

These laws describe the relationships between pressure, volume, and temperature of gases through kinetic theory.