CHEMISTRY TOPIC SUMMARY
Name: ________________________
Topic N: Gas Laws
Purple Packet
Textbook Reference
Topic N: 151 - 164
Chapter 13
Purpose
Gases behave differently from the other two commonly studied states of matter, solids and liquids, so
we have different methods for treating and understanding how gases behave under certain conditions.
Gases, unlike solids and liquids, have neither fixed volume nor shape. They are molded entirely by the
container in which they are held. The early gas laws were developed at the end of the 18th century,
when scientists began to realize that relationships between the pressure, volume and temperature of a
sample of gas could be obtained which would hold for all gases. Gases behave in a similar way over a
wide variety of conditions because to a good approximation they all have molecules which are widely
spaced, and nowadays the equation of state for an ideal gas is derived from kinetic theory. The earlier
gas laws are now considered as special cases of the ideal gas equation, with one or more of the variables
held constant.
Schedule
A and B
2/6 and
2/7
2/8 and
2/11
2/12 and
2/13
2/14 and
2/15
Due
In-Class
 Read Page 151  Notes
 Practice Problems
 WK 1 (pages
 Lab - LAB APPROPRIATE ATTIRE
157-158)
REQUIRED!!
 WK 2 (pages
 Lab - LAB APPROPRIATE ATTIRE
159-160)
REQUIRED!!
 Review WK
 Review
(pages 163 TEST
164)
HW Assignments
 Worksheet 1 (pages
157-158)
 Worksheet 2 (pages
159-160)
 Review Worksheet
(pages 163-164)
 N/A
Vocabulary
Kinetic Molecular Theory
Ideal Gas
Pressure
Temperature (OC and Kelvin)
Boyle’s Law
Charles’s Law
Avagadro’s Law
Combined Gas Law
Ideal Gas Law
STP
Dalton’s Law of Partial
Pressures
By the end of this Topic, you should be able to demonstrate proficiency in the following areas:
Essential Understandings
The concepts developed in this standard include the following:
 Molar volume = 22.4 L/mole for any gas at standard temperature and pressure (STP).
 Atoms and molecules are in constant motion.
 The phase of a substance depends on temperature and pressure.
 Temperature is a measurement of the average kinetic energy in a sample. There is a direct relationship
between temperature and average kinetic energy.
 The kinetic molecular theory is a model for predicting and explaining gas behavior.
CHEMISTRY TOPIC SUMMARY
Name: ________________________
 Gases have mass and occupy space. Gas particles are in constant, rapid, random motion and exert pressure
as they collide with the walls of their containers. Gas molecules with the lightest mass travel fastest.
Relatively large distances separate gas particles from each other.
 Equal volumes of gases at the same temperature and pressure contain an equal number of particles.
Pressure units include atm, kPa, and mm Hg.
 An ideal gas does not exist, but this concept is used to model gas behavior. A real gas exists, has
intermolecular forces and particle volume, and can change states. The Ideal Gas Law states that PV =
nRT.
 The pressure and volume of a sample of a gas at constant temperature are inversely proportional to each
other (Boyle’s Law: P1V1 = P2V2).
 At constant pressure, the volume of a fixed amount of gas is directly proportional to its absolute
temperature (Charles’ Law: V1/T1 = V2/T2).
 The Combined Gas Law (P1V1/T1 = P2V2/T2) relates pressure, volume, and temperature of a gas.
 The sum of the partial pressures of all the components in a gas mixture is equal to the total pressure of a
gas mixture (Dalton’s law of partial pressures).
Knowledge, and Skills
In order to meet this standard, it is expected that students will
The concepts developed in this standard include the following:
 explain the behavior of gases and the relationship between pressure and volume (Boyle’s Law), and
volume and temperature (Charles’ Law).
 solve problems and interpret graphs involving the gas laws.
 perform stoichiometric calculations involving the following relationships:
- mass-volume;
- mole-volume;
- volume-volume; and
- volume-particle.