Calculate the volume (mL) of acetone, C₃ H₆ O, (density = 0.786 g/mL) that can be vaporized at its normal boiling point with 345 kJ of heat. ΔH_vap for acetone is 29.1 kJ/mol.

In a typical heating curve for water, which arrows represent the phase transitions where heat energy is gained by the substance?

Which of the following statements correctly describes a heating or cooling curve for a pure substance?

Determine the vapor pressure (atm) of rubbing alcohol (isopropanol) at 20.0℃. The normal boiling point of isopropanol is 82.3℃ and the heat of vaporization (ΔH_vap) is 39.9 kJ/mol.

If 42.0 kJ of heat is added to a 32.0-g sample of liquid meth-ane under 1 atm of pressure at a temperature of -170°C, what are the final state and temperature of the methane once the system equilibrates? Assume no heat is lost to the surroundings. The normal boiling point of methane is -161.5 °C. The specific heats of liquid and gaseous methane are 3.48 and 2.22 J/g-K, respectively. [Section 11.3]

Consider a compound that has a melting point at 65 °C and a boiling point at 175 °C. Which of the following images represents a heating curve for the compound from 40 °C to 200 °C? (LO 11.5)

Why is the heat of sublimation, ΔHsubl, equal to the sum of ΔHvap and ΔHfusion at the same temperature?