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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 order to accurately study the effect that changes in pressure, temperature and moles have on volume, chemists will often run their experiments under Standard Temperature and Pressure conditions

Concept #1: Standard Temperature and Pressure

Example #1: A sample of oxygen gas has a measured volume of 325 mL at STP. How many grams are present?

Concept #2: STP and Volume

Example #2: How many moles of chlorine gas occupy a volume of 15.7 L at STP?

Practice: A sample of dichloromethane gas (CH2Cl2) occupies 32.6 L at 310 K and 5.30 atm. Determine its volume at STP?

Practice: Which gas sample has the greatest volume at STP?

Practice: Nitrogen and hydrogen combine to form ammonia via the following reaction:

                      1 N2 (s)  +  3 H2 (g) → 2 NH3 (g)

What mass of nitrogen is required to completely react with 800.0 mL Hat STP?