Evaporation Causes Cooling

Evaporation is a cooling process because when a liquid turns to a gas, it requires more energy, which it must obtain from its surroundings. The energy is in the form of heat, and as the heat energy evaporates, the surroundings cool. Evaporation replenishes the humidity of the air, mostly from the seas and plants. It is a crucial aspect of the energy exchange in the Earth-atmosphere system that causes atmospheric motion and, as a result, weather and climate. When certain molecules in a water mass get enough kinetic energy to eject themselves from the water surface, they move water between the Earth’s surface and the atmosphere.

What is Evaporation?

Evaporation is the process by which a liquid turns into vapour before reaching its boiling point (or temperature). 

Liquid molecules are always in random motion and collide with one another, gaining kinetic energy from the collisions. Some of them are now so energised that they leave the liquid, transform into gas, and escape. As a result, we can see that the process of evaporation does not require a boiling point to occur. It can happen at temperatures much lower than the liquid’s boiling point.

How does Evaporation Cause Cooling?

Evaporation is responsible for natural cooling. The fundamental idea is that for matter to change state, it must either receive or lose energy. When matter molecules transition from liquid to gas, they need energy to overcome their potential energy via kinetic energy. As a result, energy from its surroundings is absorbed by the liquid.

When energy is transferred, the temperature of the material rises or falls depending on whether the energy is transferred from the substance to the surrounding environment or vice versa. During evaporation, the temperature of the material rises until the boiling point is reached, but no visible heat transfer occurs.

The material’s molecules constantly absorb heat energy from their surroundings, cooling them until they reach boiling point, at which point they begin to separate from the liquid and transform into vapour. Because there is no temperature difference until the evaporation process is complete, i.e. the entire liquid is transformed into vapour, the energy required for this phase change is referred to as the latent heat of evaporation, implying that this heat will not affect the temperature reading on a thermometer.

Evaporative Cooling Applications:

• When we wave our hands around with some spirit or petrol on the backs of our hands, the spirit quickly evaporates and our hands become extremely cold. This is because spirit requires latent vaporisation heat to transition from a liquid to a vaporised state. This dormant vaporising energy is yanked from our grasp by the spirit. The hand loses heat and begins to cool.

• During the hot summer months, water is frequently kept cool in a clay pot known as a picture or a Matka. Water is usually kept in an earthen pot known as a pitcher or Matka to keep cool on hot summer days. The earthen pot’s walls are riddled with a plethora of extremely small pores, or holes. Some water is constantly passing through these pores to the outside of the pot. This water constantly evaporates, absorbing the latent heat required for vaporisation from the clay pot and the remaining water. As a result, the remaining water loses heat and cools. This is also an example of evaporation-induced cooling.It should be noted that none of the water on the planet evaporates due to the high value of the latent heat of water evaporation.

• Many people, particularly in villages, sprinkle water on the ground in front of their homes during the hot summer evenings. This water evaporates by removing the ground’s and surrounding air’s high latent heat of evaporation. It becomes chilly and comfortable after the heat is removed from the area. The water that evaporates from the leaves of trees acts in the same way to cool the surrounding air.

• Perspiration, also known as sweating, is our bodies’ mechanism for maintaining a constant temperature. Our sweat glands release moisture or perspiration on our bodies when our body temperature rises too high on a hot day or after engaging in strenuous exercise. Our bodies absorb the vaporising latent heat as perspiration evaporates. This helps to keep our bodies cool.

• Because it works on the evaporation principle, a desert cooler keeps you cool on a hot and dry day. On a hot day, the higher the temperature, the slower the rate of water evaporation, and the lower the temperature, the faster the rate of water evaporation. A desert cooler cools better on a hot and dry day due to the higher rate of water evaporation.

• Humans can drink hot tea from a saucer faster than they can from a cup, which is a well-known fact. The phenomenon of evaporation-induced cooling explains this. The surface area of the saucer is quite large. Hot tea evaporates more quickly due to the large surface area of the saucer. This rapid evaporation cools the hot tea more quickly, making it more drinkable.

Conclusion

Evaporation replenishes the humidity of the air, mostly from the seas and plants. It is a crucial aspect of the energy exchange in the Earth-atmosphere system that causes atmospheric motion and, as a result, weather and climate. When energy is transferred, the temperature of the material rises or falls depending on whether the energy is transferred from the substance to the surrounding environment or vice versa. Because there is no temperature difference until the evaporation process is complete, i.e. the entire liquid is transformed into vapour, the energy required for this phase change is referred to as the latent heat of evaporation, implying that this heat will not affect the temperature reading on a thermometer.