Question

the liquid-solid-vapor triple point of a pure component is T triple = 10 C and P triple = 0.05 bar. The molar densities of the liquid and solid phases are pl = 22 kmol/m^3 and ps = 26 kmol/m^3, respectively. The enthalpy change of sublimation of the solid at the triple point is Hsv = 6.22 kJ/mol and the enthalpy change of vaporization of the liquid at the triple point is Hlv = 5.65 kJ/mol. You are asked to calculate the melting temperature of the solid at a pressure of P = 10 bar. Please state explicitly all assumptions on which your calculation is based