Ethanol melts at -144°C and boils at 78°C. The enthalpy of fusion of ethanol is 5.02 kJ per mole and its enthalpy of vaporization is 38.56 kj/mol the specific heats of solid and liquid 0.97J/g•K and 2.3 J/ g•K. How much heat is required to convert 9.02 g of ethanol at - 141ﾟC to the vapor phase at 78ﾟC.

The enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.

Water at 0C was placed in a dish inside a vessel maintained at low pressure by a vacuum pump. After a quantity of water had evaporated, the remainder froze. If 9.31 g of ice at 0C was obtained, how much liquid water must have evaporated? The heat of fusion of water is 6.01 kJ/mol and its heat of vaporization is 44.9 kJ/mol at 0C.

Krypton, Kr, has a triple point at 169C and 133 mmHg and a critical point at 63C and 54 atm. The density of the solid is 2.8 g/cm3, and the density of the liquid is 2.4 g/cm3. Sketch a rough phase diagram of krypton. Circle the correct word in each of the following sentences (and explain your answers). a Solid krypton at 130 mmHg (melts, sublimes without melting) when the temperature is raised. b Solid krypton at 760 mmHg (melts, sublimes without melting) when the temperature is raised.