How would you explain evaporation using kinetic molecular theory?

Hint: Evaporation is generally defined as a process by which a liquid or solid is transformed into vapour. The vapour contains particles which are in constant random motion. According to kinetic molecules the particles in gases are far apart and have less intermolecular forces of attraction between them.

Complete step by step answer:
The kinetic molecular theory states that the particles present in molecules are constantly moving. Due to which the particles in gases are far apart and have less intermolecular forces of attraction.
During the process of evaporation the liquid changes to water vapour when we increase the temperature.
The molecules present in liquid are in constant motion during there occurs collision between molecules and this causes molecules to be tightly bound with each other so the intermolecular forces of attraction are more.
This is occurring near the surface of the container where random motion of molecules is more and kinetic energy is also maximum.
This kinetic energy is enough to break the intermolecular force of attraction between molecules and the molecules escape the container and move apart with each other. In the form of vapour.
By this theory of kinetic energy evaporation takes place.

Note: The kinetic energy of a molecule is directly proportional to the temperature. With increase in temperature kinetic energy among molecules increases.
The kinetic molecular theory is based on four principles.
Space between gas molecules is much larger than the molecules themselves.
Gas molecules are in constant random motion.
The Average kinetic energy is determined solely by temperature.