For any substance, why does the temperature remain constant during the change of state?

The phenomenon of a steady temperature in the course of a change of state is known as a phase transition. At this point, the delivered heat power is utilized in breaking or forming intermolecular forces in preference to increasing the kinetic power (which determines temperature).

For instance:
1. Melting: When a strong substance melts into a liquid, strength is absorbed to break the sturdy intermolecular forces holding the strong together. This strength is utilized in converting the state of the substance instead of growing the common kinetic strength of the debris.

2. Boiling: Similarly, when a liquid transitions to a gas (boiling), power is absorbed to conquer the intermolecular forces in the liquid, permitting the liquid to exchange into a gaseous state. Again, this power goes into the phase change in preference to raising the temperature.

Conversely:
3. Freezing: During freezing, a liquid transforms right into a stable, and electricity is released because the molecules form ordered structures. This energy is launched with out converting the temperature till the complete substance has undergone the phase trade.

4. Condensation: When a gasoline condenses right into a liquid, energy is released because the fuel debris come collectively and shape a liquid. This released energy doesn’t have an effect on the temperature till the complete segment transition is whole.

This absorption or release of energy without a change in temperature is referred to as “latent heat.” The term “latent” indicates that this heat energy is hidden or stored within the substance during the phase change, not contributing to a change in temperature but rather to a change in the state of matter.