For a process `DeltaH_(fusion)` = 2.4KCal/mol and `DeltaH_("vaporisation")` = 98.6Kcal/mol. then `DeltaH_("sublimation")`

Calculate Delta_(f)H^(Theta) ICI(g) from the data DeltaH dissociation CI_(2)(g) = 57.9 kcal mol^(-1) DeltaH dissociation I_(2)(g) = 36.1 kcal mol^(-1) DeltaH dissociation ICI(g) = 50.5 kcal mol^(-1) DeltaH sublimation I_(2)(g) = 15.0 kcal mol^(-1)

What is the melting point of benzene if DeltaH_("fusion")= 9.95kJ//mol and DeltaS_("fusion")= 35.7J//K-"mol"

White phosphorus is a tetra-atomic solid P_(4) (s)at room temperature. find bond enthalpy (P-P) in kJ//mol. Given : DeltaH_("sublimation") of P_(4) (s)= 61 kL//mol DeltaH_("atomisation") of P_(4) (s)= 1321 kJ//mol]