1. The Ideal Gas Laws by Elizabeth Kelley Buzbee AAS, RRT-NPS, RCP
Kingwood College Respiratory
Care program

2. Gas molecules bounce off one another
because they have kinetic energy

3. If we capture a number of these gas molecules into a container with rigid walls, not only will they bounce off one another, they bounce off the walls of the container.
This can read by a monometer as a pressure.

4. If the same number of molecules are crowded together into a smaller
container, as long as the temperature remains the same these molecules will
Bounce off one another and off the walls of the contain making the pressure
higher than it was.
So as long as the temperature stays the same [k] if the Volume drops, the P rises.
This is Boyles’ Law

5. We capture more gas into a rigid container. These molecules
will have a certain pressure within the volume of this container.

6. We heat this container of gas
If the temperature rises, & the volume of the container stays the same, kinetic energy of the molecules will cause them to bounce faster so that the pressure will rise.
Gay-Lussac’s Law: if the volume is constant [k]
then the pressure and temperature vary directly

7. When the temperature drops, the pressure will drop again.

8. In this case, we capture
These gas molecules in
a container that can increase
in size as the molecules bounce off it… like a balloon
Gets bigger as we add gas
Because the volume rises
the pressure stays the same.
If heat is applied, again the
faster moving molecules
will only make the container
larger so that the pressure
Stays the same.
Charle’s Law: if the pressure is constant [k]
then the temperature and volume vary directly.