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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
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Pressure Units
Kinetic Molecular Theory
The Ideal Gas Law
The Ideal Gas Law Derivations
The Ideal Gas Law Applications
Chemistry Gas Laws
Chemistry Gas Laws: Combined Gas Law
Standard Temperature and Pressure
Dalton's Law: Partial Pressure (Simplified)
Gas Stoichiometry
Intermolecular Forces (Simplified)
Intermolecular Forces and Physical Properties
Atomic, Ionic and Molecular Solids
Heating and Cooling Curves

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. 

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?