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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

Gas Stoichiometry involves chemical reactions that contain gases.

Gas Stoichiometry

Concept #1: Gas Stoichiometry

Concept #2: Gas Stoichiometric Chart

Example #1: What mass of Ag2O is produced when 384 mL of oxygen gas at 736 mmHg and 25 ºC is reacted with excess solid silver?

Practice: The metabolic breakdown of glucose (C6H12O6) (MW: 180.156 g/mol) is given by the following equation:

C6H12O6 (s)  +  6 O2 (g) → 6 CO2 (g)  +  6 H2O (l)

Calculate the volume (in mL) of CO2 produced at 34°C and 1728.9 torr when 231.88 g glucose is used up in the reaction.

Practice: The oxidation of phosphorus can be represented by the following equation:

                       P4 (s)  +  5 O2 (g) → 2 P2O5 (g)

If 1.85 L of diphosphorus pentoxide form at a temperature of 50.0 ºC and 1.12 atm, what is the mass (in g) of phosphorus that reacted?

Practice: Determine the mass (in grams) of water formed when 15.3 L NH(at 298 K and 1.50 atm) is reacted with 21.7 L of O2 (at 323 K and 1.1 atm).

4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g)