The kinetic molecular theory of gases explains gas behavior and macroscopic properties based on the motion of particles. Key concepts include random motion, no net energy loss in collisions, equal average kinetic energy, and the absence of molecular attraction. The theory also incorporates Boltzmann's equation and defines five major variables: pressure, temperature, molar mass, volume, and amount of substance.

1. Kinetic Molecular
Theory of Gases
Chemistry 10

2. Kinetic Molecular Theory
It is the basis of the description
of the behaviour and
macroscopic properties of gases

3. Concepts of Kinetic Molecular Theory:
Gases are made up of large number of particles that are
constantly moving in random
Gases are made up of no defined volume but with a defined
mass
When gas particles collide, there will be no net loss or gain in the
kinetic energy of the particles
The average kinetic energy is the same throughout all the kinds
of gases
The molecules of any type of gas never attract each other
Gases exhibit the properties of compressibility and expansibility

6. Boltzmann’s Equation
It is a set of equation that was
formulated by Ludwig Boltzmann
in order to describe the behaviour
of a thermodynamic system in a
non-equilibrium stage

7. 5 Major Variables in
Kinetic Molecular
Theory
Chemistry 10

8. Symbol: Name: Unit/Conversion:
P Pressure 1 atm = 760 torr = 760 mmHg = 101.3
kPa
T Temperature Kelvin (K) = °C + 273
M Molar Mass 1.429 g/mol
V Volume 1 L = 1000 mL
n Amount of
Substance
𝑔/𝑚𝑜𝑙−1