The normal melting point of benzene is at 5.5°C, where its density changes from 0.891 g/mL to 0.879 g/mL when it transitions from solid to liquid. Its enthalpy of fusion is 10.59 kJ/mol. Estimate the melting point of benzene at 1000 atm. (1 L atm = 101.325 J)

Calculate the total energy (kJ) required to heat a 17.5 g sample of benzene (C6H6) from 0 °C to 97.2 °C molar mass: 78.11 g/mol cs,solid  = 1.51 J/g*°C cs,liquid  = 1.70 J/g*°C cs,gas  = 1.05 J/g*°C ΔHfus = 9.9 kJ/mol ΔHvap = 33.8 kJ/mol Tf = 5.6°C Tb = 80.08°C

Butane, C4H10, is vaporized at its boiling point. C4H10(1) → C4H10(g) AH° = 301.5 kJ/mol, ASº = 761.4 J/mol·K Calculate the boiling point temperature (in K) at standard conditions.

A soft drink (290 mL of mostly water) initially at 18.0 C is cooled by adding 197 g of ice cubes at 0 C. What mass of ice remains when the temperature of the drink reaches equilibrium (water and ice at 0 C)? The enthalpy of fusion of water (i.e., the heat required to melt ice) is 6.007 kJ/mol. The density of the water is 1.0 g/mL. Assume the specific heat capacity of water is constant and equal to 4.184 J/g/C.