1 / 12

Properties of Gases Quarter 4 Lesson

Properties of Gases

Edison16
Download Presentation

Properties of Gases Quarter 4 Lesson

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Kinetic Molecular Theory • All matter is made of atoms or molecules that are in constant motion • These particles contain energy • The movement of these particles is random • VIDEO CLIP

  2. Gases

  3. Properties of Gases • Gases have mass • Gases take shape & volume of their container • Gases are compressible (because they are separated by great distances) • Gases move through each other easily • “Diffusion” • perfume, skunks! • Gases exert pressure

  4. Pressure • Gas molecules hit walls of container, exerting a force • Pressure depends on • Number of impacts (collisions) per unit time • Force of each impact

  5. Barometer animation

  6. What is air pressure? • pressure exerted on us by weight of gases above our heads (& all around our body) • at sea level: air pressure = 1 atmosphere (atm) = 760 torr = 760 mmHg = 101.3 kPa

  7. When we talk about gases, we use a model to show how it would “ideally” behave. • The model = Kinetic Molecular Theory Of Gases • Under the KMT, we make 4 assumptions about the behavior of Gases

  8. Kinetic Molecular Theory of Gases • Particles move in rapid, random, straight line motion • ELASTIC Collisions = When they hit one another and the walls of their container, they do not lose potential energy – they do not slow down • They are separate by great distances (the gas is mostly empty space) therefore the volume of the gas molecule is negligible • Gas molecules do not attract or repel one another

  9. Real vs. ideal gas • Ideal gas obeys all assumptions of KMT all the time • It’s a model • It doesn’t exist • Real gases • Molecules really do have volume • And molecules will interact, especially at high pressure & low temperature NOTE: when molecules are close together they will interact and could possibly condense LINK

  10. High pressure – Look what happens to this gas

  11. Low temperature– Look what happens to this gas

  12. When we measure the temperature of a gas, we are measuring the average kinetic energy of the particles

More Related