Epsillon said:particles that are not neccessarly on surface are forming bubles and vaporizing
Vapour pressure is the measure of the pressure exerted by a substance's gas phase when it is in equilibrium with its liquid or solid phase at a given temperature.
The higher the vapour pressure, the lower the boiling point of a substance. This is because at higher vapour pressures, the molecules have enough energy to overcome the atmospheric pressure and escape into the gas phase, causing the substance to boil.
Vapour pressure is affected by temperature, intermolecular forces, and the nature of the substance. As temperature increases, so does the vapour pressure. Stronger intermolecular forces result in lower vapour pressures, while weaker forces result in higher vapour pressures.
Atmospheric pressure is the pressure exerted by the Earth's atmosphere. It affects boiling point because it is the pressure that must be overcome in order for a substance to boil. As atmospheric pressure decreases, the boiling point of a substance also decreases.
Atmospheric pressure decreases as altitude increases. This is because at higher altitudes, there is less air above to exert pressure. As a result, water and other liquids will boil at lower temperatures at higher altitudes due to the decreased atmospheric pressure.