Difference Between Boiling and Evaporation

Vaporization is a process of phase transition in which a substance, changes its state from liquid to vapour. It can take place in two ways, i.e. evaporation and boiling. The process of evaporation involves phase transition at a temperature below the boiling temperature. On the other hand, boiling of a substance takes place at boiling point, which may vary with the change in the environmental pressure.

Water boils at 100°C, and the temperature does not rise even if heat is continuously supplied to it. As against, the rate of evaporation depends on the surface area, in the sense that the larger the area, the faster would be the process. Let’s take a look at the article provided below which simplifies the difference between boiling and evaporation.

Content: Boiling Vs Evaporation

1. Comparison Chart
2. Definition
3. Key Differences
4. Conclusion

Comparison Chart

Basis for Comparison	Boiling	Evaporation
Meaning	Boiling implies a vaporization process that turns liquid into gas, when continuously heated.	Evaporation is a natural process, wherein the liquid changes its form to gas due to the increase in temperature or pressure.
Phenomenon	Bulk	Surface
Temperature required	Occurs only at boiling point.	Occurs at any temperature.
Bubbles	It forms bubbles	It does not forms bubbles.
Energy	Source of energy is required.	Energy is supplied by the surrounding.
Temperature of liquid	Remains constant	Reduces

Definition of Boiling

Boiling is a physical change and a type of rapid vaporization in which the liquid is converted to vapour when it is constantly heated at the such a temperature that the vapour pressure of the liquid is same as the external pressure, exerted by the surrounding.

The temperature at which boiling starts is known as the boiling point. It depends on the pressure exerted upon the liquid, i.e. the greater the pressure, the higher will be the boiling point. In the boiling process, when the molecules of the substance are so spread that it can change its state, the bubbles are formed and boiling starts.

In this process, as we heat the liquid, the vapour pressure rises, until it is equal to the atmospheric pressure. After that, the formation of bubbles will take place within the liquid and move to the surface and burst resulting in the release of gas. Even if we add more heat to the liquid, the boiling temperature will be same.

Definition of Evaporation

The process in which an element or compound is converted from liquid state to gaseous state, because of the rise in temperature and/or pressure is known as evaporation. The process can be used to separate the solid dissolved in the liquid, such as salt dissolved in water. It is a surface phenomenon, i.e. it happens from the surface of the liquid into vapour.

Heat energy is the basic requirement for evaporation to take place, i.e. to split the bonds that hold the molecules of water together. In this way, it helps water to evaporate slowly, at the freezing point.

Evaporation largely depends on the temperature and the amount of water present in the waterbody, i.e. the higher the temperature and the more the water is there, the higher will be the rate of evaporation. The process can take place in both natural and man-made environment.

Conclusion

To sum up, boiling is a faster process in comparison to the evaporation, as the molecules of the liquid, move faster in boiling than in the process of evaporation. While boiling produces heat and does not cause cooling of the liquid, evaporation leads to cooling of the liquid.