Kinetic Theory & Ideal Gas Lab

Kinetic Theory of Gases

This model describes a gas as a large number of submicroscopic particles (atoms or molecules), all of which are in constant, rapid, random motion. The pressure a gas exerts is due to the force of these particles colliding with the walls of the container. The temperature of the gas is a measure of the average kinetic energy of the particles.

What to look for

• Hotter gas means faster particles, so they hit the walls harder and more often.
• Observe how these changes affect the pressure gauge on the right.
• **Listen closely!** The "hiss" of particle collisions changes with temperature and pressure, and you'll hear the piston move.