evaporiatie

Evaporiatie, also known as evaporation, is the process by which a liquid becomes a vapor at the interface with its surroundings. It occurs when molecules at the liquid surface gain enough kinetic energy to overcome the cohesive forces of the liquid and escape into the gas phase. Evaporation can happen at any temperature, not only at the liquid’s boiling point, and proceeds until the rate of evaporation balances the rate of condensation in a given environment.

In terms of thermodynamics, the vapor pressure of a liquid increases with temperature. Evaporation continues even below the boiling point, and in a closed system the vapor accumulates until dynamic equilibrium is reached. If vapor is removed or the surroundings allow rapid diffusion away from the surface, evaporation can proceed more quickly.

Factors that influence evaporation include:

- Temperature difference between the liquid and its surroundings

- Surface area of the liquid exposed to air

- Air movement and convection above the liquid

- Humidity and partial pressure of the vapor in the surrounding air

- Ambient pressure

- Volatility of the liquid (its inherent tendency to evaporate)

Evaporation is distinct from boiling: boiling is a bulk phenomenon where vapor forms inside the liquid when its vapor pressure equals the surrounding pressure, typically at the liquid’s boiling point. Evaporation is surface-limited and can occur at temperatures well below boiling.

Applications and natural relevance include distillation, drying, desalination, and evaporative cooling. Evaporation also drives the Earth's water cycle, as water from oceans, rivers, and soils enters the atmosphere as vapor, influencing climate and weather patterns.