This document discusses the kinetic molecular theory and Boyle's law. It explains that gases are made of molecules that are far apart from each other and move randomly, colliding with the container walls. According to Boyle's law, if the volume of a container decreases, the pressure increases because the molecules collide with the walls more frequently. The document provides the formula for Boyle's law, P1V1 = P2V2, and gives examples of using it to calculate pressure and volume.

1. BOYLES LAW

2. SOLIDS, LIQUIDS AND GASES
 How are the molecules/atoms arranged?
 Solids: Tightly packed and vibrate
 Liquids: Farther apart and can move past each
other.
 Gases: Very far apart and collide with one another
randomly.

4. KINETIC MOLECULAR THEORY
 1) Gases particles are very small compared to
distance separating them.
 2) Gas molecules are in constant random motion
and collide with one another and walls of container
= gas pressure.
 3) Collisions are elastic- no loss of total kinetic
energy.
 4) As temp increases so does the speed of the
molecules and the average kinetic energy
increases.

5.  Kinetic Molecular theory

6. BOYLE’S LAW: P-V RELATIONSHIPS
 Gases can be compressed.
 Decreased volume = increased pressure
 Increased volume = decreased pressure
 Why?
 Pressure is the result of the collisions with the sides
of the container.
 If container (volume) becomes smaller the
molecules collide with the sides of the container
more often = increased pressure.

8.  Marshmellow pals in a vacuum

9. P1V1 = P2V2
 What would the pressure in a can be if it can deliver
8000 ml of Helium at 1.3 atm and the can has a
volume of 480 ml?

10.  What would the volume of a can be if it can hold
5000 ml of a gas at 100 kPa and the pressure
inside the can is 150 kPa?