The liquid-solid-vapor triple point of a pure substance is Tt=283 K and Pt=0.05 bar. The molar densities of the liquid and solid phases are ?l=22 kmol/m3 and ?s=26 kmol/m3, respectively. The molar enthalpy change of sublimation of the solid at the triple point is ? ?H sv=6.22 kJ/mol and the molar enthalpy change of vaporization of the liquid at the triple point is ? ?H lv=5.65 kJ/mol. Calculate the melting temperature of the solid at a pressure of 10 bar, assuming that the ratio ? ?H sl=?? Vsl is temperature independent, where ? ?H sl is the molar enthalpy change of melting and where ?? Vsl is the molar volume change of melting.