In Heating and Cooling curves we have the representation of the amount of heat absorbed or released during phase changes.
Concept #1: If a solid substance absorbs enough thermal energy it can undergo the phase changes of fusion and vaporization.
Concept #2: If a gaseous substance evolves enough thermal energy it can undergo the phase changes of condensation and freezing.
Example #1: How much energy (kJ) is required to convert a 76.4 g acetone (molar mass = 58.08 g/mol) as a liquid at -30 oC to a solid at -115.0 oC?
Practice: If 53.2kJ of heat are added to a 15.5g ice cube at - 5.00 oC, what will be the resulting state and temperature of the substance?