Identify whether the enthalpy of the initial state is greater than, less than or equal to that of the final state in the following changes: solid`to`liquid, vopur`to`solid, liquid`to`vapour.

Explanation

Solid`to`Liquid: it is an endothermic process. In this process, `DeltaH gt0`, i.e.,, `H_("liquid") -H_("solid") gt 0` or, `H_("liquid") gt H_("solid")`.
Therefore, the enthalpy of the final state will be greater than that of the initial state.
Vapour`to`Solid: It is an exothermic process. so, iin this process, `DeltaH lt 0`. hence, `H_("solid") -H_("vapour")lt0`.
or, `H_("solid")ltH_("vapour")`. that is the enthalpy of the final state is less than that of the initial state.
Liquid`to`Vapour: it is an endothermic process. So, in this process, `DeltaH gt 0` or, `H_("vapour")-H_("liquid")`. therefore, the enthalpy of the final state is greater than that of the initial state.