A compound has\ A molecular weight of 50 kg/kmol.\ 1I will post this in the slides folder on Google Drive.\ 1\ A normal melting point of 300 K.\ A normal boiling point of 350 K.\ A constant heat capacity in the solid phase of CP = 3000 J kg1 K1.\ A constant heat capacity in the liquid phase of CP = 3600 J kg1 K1.\ A constant density in the solid phase of \\\ ho = 640 kg/m3.\ A constant density in the liquid phase of \\\ ho = 480 kg/m3.\ An ideal gas heat capacity of CP = 4186.8 6.28T + 13.56 \\\\times 103T 2 J kg1 K1, with T representing the temperature in Kelvin.\ An enthalpy of fusion Hfus = 175 kJ/kg at atmospheric pressure.\ An enthalpy of vaporization Hvap = 300 kJ kg1 at atmospheric pressure.\ (a) Estimate the change in U when this compound melts at atmospheric pressure.\ (b) Estimate the change in U when this compound boils at atmospheric pressure.\ (c) Estimate the change in H when one kmol is heated at constant pressure P = 1 atm from 269 K to 366 K. How does this differ from U?\ (d) Suppose that the compound boils at 325 K if P = 0.5 bar. Describe how to estimate the enthalpy of vaporization for this compound using only the provided data.