liquid-vapour equilibrium

Liquid-vapor equilibrium describes the state where a substance exists in both liquid and gaseous phases simultaneously, with no net change occurring between them. This equilibrium is represented on a phase diagram by a line, specifically the vapor-pressure curve.1

The vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid or solid form. This pressure increases with temperature. The point where the vapor pressure of a liquid equals the surrounding pressure is known as its boiling point. At the critical point, the distinction between liquid and gas phases disappears, and they become indistinguishable. Vaporization, the process of a substance converting from liquid to gas, requires heat. Condensation is the reverse process, where heat is released. The Clausius-Clapeyron equation relates the change in vapor pressure to temperature changes, particularly useful for understanding boiling points at different pressures.23145