Prove that the slope of the sublimation curve of a pure substance at the triple point must be greater than that of the vaporization curve at the triple point.

Phase transitions are changes between different states of matter: solid, liquid, and gas. Common examples include melting (solid to liquid), freezing (liquid to solid), and boiling (liquid to gas). During a phase transition, the temperature of a substance remains constant while the change in state occurs. This phenomenon can be understood using the Clausius-Clapeyron equation, which relates temperature and pressure during phase transitions. For example, sublimation describes a solid turning directly into a gas, while vaporization refers to a liquid becoming a gas. Each phase transition has unique physical characteristics and plays a crucial role in a variety of natural processes.

Latent heat is the energy absorbed or released during a phase transition without changing the temperature. There are several types of latent heat:

• Latent heat of fusion: Energy required to melt a solid.
• Latent heat of vaporization: Energy needed to vaporize a liquid.
• Latent heat of sublimation: Energy for converting a solid into a gas.

For instance, water requires latent heat to transform from ice to liquid or from liquid to vapor. Latent heat helps in understanding phase transitions, as the amount of energy needed for these changes differs across substances and transitions. In our example, the latent heat of sublimation is generally higher than the latent heat of vaporization, explaining why different slopes are observed in phase transition curves.

The triple point of a substance is a unique combination of temperature and pressure at which three phases (solid, liquid, and gas) coexist in equilibrium. It is a vital concept in thermodynamics and helps determine the physical properties of substances. For example, the triple point of water is at 0.01°C and 611.657 Pa, where ice, liquid water, and water vapor meet. At the triple point, subtle differences in phase transition energies become noticeable. The slopes of the sublimation and vaporization curves can be compared using the Clausius-Clapeyron equation, revealing important insights into the latent heats for different transitions.

Sublimation is the process in which a solid changes directly into a gas without passing through the liquid phase. Common examples include dry ice (solid carbon dioxide) turning into carbon dioxide gas, and snow disappearing without melting. Sublimation requires energy input called the latent heat of sublimation, typically higher than the latent heat of vaporization. For instance, at the triple point, the slope of the sublimation curve can be steeper than the vaporization curve due to the higher energy involved. Exploring sublimation helps understand atmospheric processes and preserves materials that would otherwise melt under regular conditions.

Vaporization is the transformation of a liquid into a gas. This phase transition has two forms:

• Evaporation: Occurs at the surface of the liquid, typically at temperatures below boiling.
• Boiling: Happens throughout the entire liquid, at a specific temperature called the boiling point.

Vaporization involves the latent heat of vaporization, which is the energy needed to break intermolecular forces. For example, boiling water requires energy to transition from liquid to steam. Using the Clausius-Clapeyron equation, we see that the slope of the vaporization curve at the triple point depends primarily on this latent heat. Generally, the latent heat of vaporization is lower than the latent heat of sublimation, impacting the steepness of respective phase transition curves.