Enthalpy change for a cyclic process is zero.

Explanation:
When we talk about a cyclic process, we are referring to a process in which a system undergoes a series of changes and eventually returns to its initial state. In other words, the system starts and ends at the same point.

Understanding Enthalpy:
Enthalpy is a thermodynamic property that describes the total energy of a system. It is denoted by the symbol 'H'. Enthalpy change, ΔH, represents the difference in enthalpy between the initial and final states of a system.

Key Point:
The enthalpy change for a cyclic process is zero because the system returns to its initial state, meaning the initial and final enthalpies are the same.

Explanation:
When a system undergoes a cyclic process, it goes through a series of changes that may involve energy transfer in the form of heat or work. However, since the system returns to its initial state, the overall change in enthalpy is zero.

Example:
Let's consider an example of a gas in a closed container that undergoes a cyclic process. Initially, the gas is at a certain temperature and pressure. It is then compressed, heated, and expanded back to its initial state.

During the compression and heating stages, the gas absorbs energy in the form of work and heat, respectively. However, during the expansion stage, the gas releases the same amount of energy that was absorbed earlier. As a result, the net change in energy is zero, and therefore, the enthalpy change is zero as well.

Conclusion:
In conclusion, the enthalpy change for a cyclic process is zero because the system returns to its initial state, and the initial and final enthalpies are the same.