The pressure of the gas increases.

The pressure of the gas increases (Boyle's Law).

The pressure of the gas increases.

The volume of the gas increases (Charles' Law).

It deviates significantly from ideal gas behavior due to increased intermolecular forces and non-negligible particle volume.

The Ideal Gas Law describes the relationship between pressure (P), volume (V), number of moles (n), ideal gas constant (R), and temperature (T) of an ideal gas: $$PV = nRT$$ or $$PV = Nk_BT$$

A theoretical gas that obeys the ideal gas law. Its particles have negligible volume, experience no intermolecular forces, and undergo perfectly elastic collisions.

Force exerted per unit area by gas particles colliding with the walls of a container. Usually measured in Pascals (Pa) or atmospheres (atm).

The amount of space occupied by the gas. Usually measured in cubic meters (m³) or liters (L).

The theoretical temperature at which an ideal gas would have zero pressure and minimal kinetic energy. It is 0 Kelvin or -273.15°C.

A physical constant that relates the energy scale to temperature scale, with a value of 8.314 J/mol·K.

A theoretical gas that perfectly obeys the ideal gas law, with particles having negligible volume, no intermolecular forces, and undergoing elastic collisions.

The force exerted per unit area by the gas on the walls of its container, usually measured in Pascals (Pa) or atmospheres (atm).

The amount of space occupied by the gas, typically measured in cubic meters (m³) or liters (L).

A measure of the average kinetic energy of the gas particles, always measured in Kelvin (K).

The theoretical temperature at which an ideal gas would have zero pressure and minimal kinetic energy; 0 Kelvin or -273.15°C.

A unit of measurement for the amount of substance, representing 6.022 x 10^23 particles (Avogadro's number).