The greatest value for a given substance will depend on the substance itself. However, in general, Option 2) the enthalpy of vaporization tends to be the largest among the given options for many substances.
The greatest value for a given substance will depend on the specific substance being considered. Let's discuss each of the options:
1. Enthalpy of Fusion: This is the amount of heat required to convert a solid substance into a liquid state at its melting point. The enthalpy of fusion is usually smaller than the enthalpy of vaporization for most substances. For example, the enthalpy of fusion of water is 6.01 kJ/mol.
2. Enthalpy of Vaporization: This is the amount of heat required to convert a liquid substance into a gaseous state at its boiling point. The enthalpy of vaporization is typically larger than the enthalpy of fusion. For example, the enthalpy of vaporization of water is 40.7 kJ/mol.
3. Enthalpy of Condensation: This is the amount of heat released when a gaseous substance condenses into a liquid state. The enthalpy of condensation is the same magnitude as the enthalpy of vaporization but with the opposite sign. For example, the enthalpy of condensation of water is -40.7 kJ/mol.
4. Enthalpy of Sublimation: This is the amount of heat required to convert a solid substance directly into a gaseous state without going through the liquid phase. The enthalpy of sublimation can vary depending on the substance. For example, the enthalpy of sublimation of dry ice (solid carbon dioxide) is 25.2 kJ/mol.