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?