Presentation1fdfdfdffdgggyfyfyfffw8.pptx

ghdhd

1. Kinetic Molecular Theory of Gases

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

3. The smallest and basic unit of particles. 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 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. 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.

5. 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 19 th century.

6. 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.

7. 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)

8. 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

9. 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)

10. Modified True or False. White TRUE if the statement is correct; if it is wrong writes FALSE. 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. The molecules undergo not perfectly elastic collisions with each other and with the walls of the container, but otherwise do not interact. The transfer of kinetic energy between molecules is heat. Pressure will compress a gas, reducing its volume and giving it a greater density and concentration of particles. The higher the temperature, the lesser the kinetic energy of the particles and vice versa.