What conditions typically lead to evaporation of a liquid?

The conditions that lead to evaporation of a liquid are best captured by the combination of high heat, low humidity, and fast movement of surrounding air.

High heat provides the energy necessary for molecules in the liquid to overcome intermolecular forces and enter the vapor phase. When heat is applied, the kinetic energy of the molecules increases, making it easier for them to escape from the surface of the liquid.

Low humidity is crucial because it indicates that the air around the liquid has a lower concentration of water vapor. When humidity is low, the air can absorb more vapor from the liquid, facilitating a greater rate of evaporation. If the air is already saturated with moisture (high humidity), the rate of evaporation slows significantly since the air cannot hold much additional vapor.

Fast movement of surrounding air enhances evaporation by continuously removing water vapor that has already evaporated from the surface of the liquid. This movement reduces the local concentration of vapor above the liquid, allowing for more molecules to escape into the air. In contrast, stagnant air can lead to a buildup of vapor, which inhibits further evaporation.

These three factors - high heat, low humidity, and fast air movement - create optimal conditions for evaporation to occur efficiently.