Question

1. Calculate the heat required to melt 9.43 g of benzene at its normal melting point. Heat of fusion (benzene) = 9.92 kJ/mol Heat = _______ kJ 2.Calculate the heat required to vaporize 9.43 g of benzene at its normal boiling point. Heat of vaporization (benzene) = 30.7 kJ/mol Heat = _______ kJ 3.What quantity of energy does it take to convert 0.800 kg ice at –20.°C to steam at 250.°C? Specific heat capacities: ice, 2.03 J/g·°C; liquid, 4.2 J/g·°C; steam, 2.0 J/g·°C; delta H vap = 40.7 kJ/mol; delta H fus = 6.02 kJ/mol. Energy = _______ kJ 4. A 23.2-g sample of ice at -12.1°C is mixed with 118.2 g of water at 80.0°C. Calculate the final temperature of the mixture, assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.03 and 4.18 J/g∙°C, respectively, and the enthalpy of fusion for ice is 6.02 kJ/mol. Final temperature = ______ C