6) Liquids may evaporate in open containers. The particles with large kinetic energies can escape to the gas phase by defeating these intermolecular forces. Because molecules collide too much, and their kinetic energies may exceed the average due to transmission.
Thus, if the molecule is close to the liquid surface, it can pass the gas phase by defeating the attraction power of the neighboring molecule. That is called evaporation.
Evaporation, if allowed, may continue until all the liquid in the container has evaporated and passes into the gas phase. Because when a liquid begins to evaporate from an open container, it takes heat from its surroundings to maintain its temperature, and this event is continuously renewed and continues until all the liquid has evaporated.
It also reduces the temperature around it due to the heat it receives from its surroundings. If the temperature of the liquid is increased, evaporation also increases.
Because when the temperature rises, the average kinetic energies of the molecules also increase, so that they have enough energy to move to the gas phase. If the temperature of the liquid is lowered, the number of energetic molecules is reduced and the evaporation rate decreases.
The pressure of the liquid vapor in equilibrium is called the balance vapor pressure at that temperature and depends on the following two factors:
a) The type of liquid:
Intermolecular attraction force is an important factor. Polarity degrees of molecules determine this force..
b) The temperature of the liquid:
Increase in temperature of molecules increases the kinetic energy and the number of molecules passing through the gas phase increases accordingly.
