1. Chapter 6 Lesson 3-The behavior of gases

2. Understanding Gas Behavior  Gases behave differently than solids and liquids  Changes in temperature, pressure, and volume affect gases  Kinetic molecular theory- is an explanation of how particles in matter behave:  1.Small particles make up all matter  2.The particles are in constant, random motion  3.The particles collide with other particles, other objects, or the sides of the container  4.When particles collide no energy is lost.

3. Understanding Gas behavior  Gas molecules collide with the container they are in.  As a result, the molecules exert a pressure on their container.  Pressure- the amount of force applied per unit of area  The more a gas is compressed then the higher the pressure

4. Pressure and Volume  At a constant temperature-  Bigger container ( more volume) then less pressure  The particles hare more room to move so less particles are bumping into each other and the container  Smaller container (less volume) then more pressure  The particles have less room to move so they are constantly bumping into each other  So an inverse proportion  It is also a famous law- Boyle’s Law

5. Boyle’s law  Robert Boyle- British (1627-1691)  Boyle’s law- if the pressure of a gas increases if the volume of the gas decreases, and if the volume of the gas increases then the pressure decreases

6. Temperature and Volume  At a constant pressure-  At a low temperature, the average kinetic energy is low so the particles are close together so the volume of the gas is low.  At high temperature, the average kinetic energy is increased so the volume of the gas is increased.  They are directly proportional  This is another famous law- Charles’s law

7. Charles’s Law  Jacque Charles (1746-1823)- French scientist  Charles’s law states- that the volume of a gas increases with increasing temperature, if the pressure is constant.