Solid iodine melts at 113 °C and boils at 184 °C under 1 atm pressure. The enthalpy of fusion at 113 °C is 15.5 kJ mol⁻¹, and the enthalpy of vaporization at 184 °C is 41.6 kJ mol⁻¹.
(1) Determine the molar enthalpy of sublimation of iodine at 1 atm, assuming that the temperature dependence of ΔH is negligible over the range considered. Show your calculation.
(2) Using your result from part (a), describe the physical significance of the enthalpy of sublimation in the context of the relative strengths of intermolecular forces in the solid and gaseous phases of iodine.