Ch.8 Gases, Liquids and SolidsWorksheetSee all chapters
All Chapters
Ch.1 Matter and Measurements
Ch.2 Atoms and the Periodic Table
Ch.3 Ionic Compounds
Ch.4 Molecular Compounds
Ch.5 Classification & Balancing of Chemical Reactions
Ch.6 Chemical Reactions & Quantities
Ch.7 Energy, Rate and Equilibrium
Ch.8 Gases, Liquids and Solids
Ch.9 Solutions
Ch.10 Acids and Bases
Ch.11 Nuclear Chemistry

In Heating and Cooling curves we have the representation of the amount of heat absorbed or released during phase changes. 

Heating & Cooling Curves

Concept #1: If a solid substance absorbs enough thermal energy it can undergo the phase changes of fusion and vaporization. 

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Concept #2: If a gaseous substance evolves enough thermal energy it can undergo the phase changes of condensation and freezing. 

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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?

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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?


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