Vapor Pressure Vs Boiling Point

Vapor pressure is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases at a given temperature in a closed system. It reflects the tendency of particles to escape from the liquid or solid phase into the gas phase. The vapor pressure of a substance increases with temperature, as more molecules have sufficient energy to enter the vapor phase. This property is crucial in understanding processes like evaporation, boiling, and the behavior of substances under varying temperature and pressure conditions.

Boiling point is the temperature at which the vapor pressure of a liquid equals the external pressure surrounding the liquid, allowing it to change into a gas. At this point, the liquid begins to form vapor bubbles within its bulk, leading to a rapid transition from liquid to gas. The boiling point is influenced by external pressure; for instance, at higher altitudes where atmospheric pressure is lower, liquids boil at lower temperatures. Understanding boiling points is essential in various applications, including distillation, cooking, and chemical reactions.