Which of the following processes is included in the enthalpy of phase changes?

The enthalpy of phase changes refers to the heat energy absorbed or released during a transition from one phase of matter to another, at a constant pressure. Vaporization, specifically, is the process where a substance changes from a liquid to a gas. This transition requires the absorption of energy, as the molecules must overcome intermolecular forces to enter the gaseous state.

During vaporization, the enthalpy of the system increases because energy is added to the liquid to break the bonds that hold the molecules together in the liquid phase. The energy change associated with this process is called the enthalpy of vaporization, which is a key concept in thermodynamics and is crucial for understanding how heat and temperature interact during phase transitions.

This principle also applies to other processes like condensation, freezing, and deposition, where energy interactions occur, but the focus is specifically on vaporization in this context, making it pivotal in discussions of enthalpy related to changes in phase.