All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Sections
Pressure Units
The Ideal Gas Law
The Ideal Gas Law Derivations
The Ideal Gas Law Applications
Chemistry Gas Laws
Chemistry Gas Laws: Combined Gas Law
Mole Fraction
Partial Pressure
The Ideal Gas Law: Molar Mass
The Ideal Gas Law: Density
Gas Stoichiometry
Standard Temperature and Pressure
Effusion
Root Mean Square Speed
Kinetic Energy of Gases
Maxwell-Boltzmann Distribution
Velocity Distributions
Kinetic Molecular Theory
Van der Waals Equation
Additional Practice
Manometer
Collecting Gas Over Water
Additional Guides
Boyle's Law
Charles Law
Ideal Gas Law

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)