Final answer:
Raising the temperature increases saturation vapor pressure and specific melting rate while potentially decreasing the specific heat required for phase changes like sublimation and absorption. An example is the increased rate of water evaporation with higher temperatures. Additionally, in thermodynamics, a higher temperature can make a non-spontaneous process (with positive enthalpy and entropy changes) spontaneous due to a larger TΔS term.
Step-by-step explanation:
Raising the temperature impacts several thermodynamic properties, namely saturation vapor pressure (SVP), specific melting rate (SMR), specific sublimation heat (SSH), and specific absorption heat (SAH). When the temperature increases, SVP also increases because the higher kinetic energy of the molecules makes them more likely to escape the liquid and enter the vapor phase. Similarly, higher temperatures usually increase SMR because more energy is available to break the solid structure. SSH and SAH refer to the energy required for phase changes; higher temperatures can decrease these values because a higher ambient temperature means less heat needs to be absorbed for a phase change.
An example to illustrate the effect of temperature on these properties would be in the context of water. As water is heated, its saturation vapor pressure increases leading to a higher rate of evaporation.
Moreover, the relationship between temperature change and spontaneity of a process can be described by the equation ΔG = ΔH - TΔS, where ΔG is Gibbs free energy, ΔH is enthalpy change, and ΔS is entropy change. Case 3 conditions (ΔH > 0 and ΔS > 0) indicate that the process is less likely to be spontaneous at low temperatures but may become spontaneous as the temperature increases, because the term TΔS may become larger than ΔH.