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

A gas is seen as a collection of molecules or individual atoms that are in constant motion. The Kinetic-Molecular Theory tries to use data of real gases to predict how an ideal gas would behave if they existed.  

Examining the Kinetic-Molecular Theory

Concept #1: Understanding the Kinetic-Molecular Theory

Example #1: Which conditions of P and T make for the most ideal gas?

Concept #2: Kinetic Molecular Theory Postulates

Practice: Which of the following statements would correctly explain the non-ideal behavior of a gas based on the Kinetic Molecular Theory (KMT)?


a) At high temperatures the attractive forces between molecules becomes negligible.
b) At high pressure the volume of gas molecules become significant.
c) An increase or decrease in the moles of gas causes the gas constant value to change.

Practice: Which of the following statements is/are true for gas molecules according to the Kinetic Molecular Theory?

I.Increasing the amount of gas molecules increases the pressure by increasing the force of the collisions.
II.Decreasing the temperature of a gas decreases the pressure by increasing the force of the collisions.
III.Decreasing the volume of a gas increases pressure by increasing the frequency of the collisions.

a) I only

b) II only 

c) III only 

d) I and II 

e) II and III

Practice: Which statement is TRUE about kinetic molecular theory?

a) A single particle does not move in a straight line.
b) The size of the particle is large compared to the volume.
c) The collisions of particles with one another is completely elastic.
d) The average kinetic energy of a particle is not proportional to the temperature.

Practice: Based on the kinetic-molecular theory, which of the following is/are true?
I.At a given temperature, all gases have the same average kinetic energy.
II.At a given temperature, different gases have the same average velocities.
III.The average kinetic energy is proportional to the absolute temperature.


a.I only
b.II only
c.I & III only
d.I, II & III