During a phase transition, energy is absorbed or released by the substance to change its state, but its temperature remains constant. For example, when ice melts, it absorbs energy from the surroundings but its temperature remains at 0°C until all the ice has melted. Similarly, when water boils, it absorbs energy and its temperature remains at 100°C until all the water has vaporized.
The energy required for a phase transition is called the latent heat. Latent heat is the amount of energy required to change the state of a substance without changing its temperature. The latent heat of fusion is the energy required to melt a solid, while the latent heat of vaporization is the energy required to vaporize a liquid.
Phase transitions are important in many natural processes, such as the melting of ice, the boiling of water, and the condensation of clouds. They are also used in industrial processes, such as the refining of metals and the production of plastics.
