The document outlines the principles of the kinetic molecular theory of gases, highlighting the relationship between gas properties like temperature, pressure, and volume. It explains key concepts such as the behavior of gas particles, the nature of gas collisions, and factors affecting gas behavior. Additionally, it includes an experiment demonstrating molecular movement and questions assessing understanding of the concepts discussed.

1. Kinetic Molecular Theory
of Gases

2. At the end of the period, students will be able to:
1.Understand the basic principles of Kinetic Molecular Theory of
Gases .
2.Determine the factors affecting the gas properties like
temperature, pressure and volume, and
3.Take and pass with mastery level of at least 75%.
OBJECTIVE

3. Direction: Fill the boxes with correct letters to complete the world being described.
Some of the letters are done for you as a clue.
E
1. It cannot be created or destroyed; it can only be conserved and converted from one form to another?
R
2. Anything that takes up space having volume and has mass?
M
3. A group of two or more atoms held together by chemical bonds.
A
4. A substance that has no fixed size or shape.
A
5. The smallest and basic unit of particles.

4. EXPERIMENT
I have here a glass of water. I will drop a few drops of red food coloring
in it.
a. What happens?
 The red food coloring drops should make their way down the glass of
water slowly, spread out and finally tint all of the water a reddish
color.
b. Why does it happen?
• It happens because both substances are made out of molecules
that are constantly moving. These molecules have energy.

6. Kinetic energy is energy that is in motion and
causing changes. Any object or particle that is in
motion has kinetic energy based on its mass and
speed.
So, Kinetic Molecular Theory was proposed by
James Clerk Maxwell and Ludwig Boltzmann in
19th
century.

7. Three basic assumptions
When you say in particle volume, gas takes up the volume to its
container. It means that it has no definite volume and no definite shape.
When you say in particle motion, gas participates are in constant,
random and straight-line motion. Which means the arrangement of gas
particles is very far apart from one another.
When you say in particle is elastic collision is the collision in which
colliding objects rebound without lasting deformation or heat
generation. Collisions between the gas particles and the wall of the
container exert a force on the wall.

9. Then, we will recall the properties of gases. What are
these? Give me one.
Gas volume changes with pressure and temperature.
When you say pressure, it is defined as force exerted.
So, gas volume changes with pressure in a way of
exerting force that can compress the gas. Gas is very
compressible. (Example-plastic bottle)

10. Gas volume changes with temperature
Temperature affects the behavior of gas particles or
molecules. At higher temperature, the gas volume
increases. At lower temperature, the gas volume
decreases. (Example-hot air balloon)
Gases exert pressure
Gas exert pressure due to the force gas exerts on a
containers wall. (a person blowing up a balloon

11. Gases have low viscosity
Gases flow much more freely than liquids and solid. Low
viscosity allows gases to be transported through pipes
over long distance but also to leak rapidly out of small
holes. (Example- LPG tank)
Gases are miscible
 Miscibility is the property of two substances to
mix in all proportions. (Example miscible)

12. Modified True or False. White TRUE if the statement is correct; if it is wrong
writes FALSE.
1. The gas is composed of a small number of identical molecules moving in
random directions, separated by distances that are large compared to their
size.
2. The molecules undergo not perfectly elastic collisions with each other and
with the walls of the container, but otherwise do not interact.
3. The transfer of kinetic energy between molecules is heat.
4. Pressure will compress a gas, reducing its volume and giving it a greater
density and concentration of particles.
5. The higher the temperature, the lesser the kinetic energy of the particles and
vice versa.