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Ch.8 Gases, Liquids and SolidsWorksheetSee all chapters
All Chapters
Ch.1 Chemistry, Matter, and Measurement
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
Sections
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

Pressure is the force that is exerted within a given volume of space. 

Understanding Pressure

Concept #1: Pressure Units

Pressure represents the force that a gas molecule exerts against the walls of its container. It can be depicted as force per area.

Example #1: What happens to the pressure if the same amount of gas molecules is transferred from a 5.0 L containerto a 10.0 L container?

Concept #2: Pressure Unit Conversions

Example #2: The pressure in Denver, Colorado (elevation 5280 ft), averages about 24.9 inHg. Convert this pressure intommHg and atm.