3.5 Kinetic Molecular Theory

The KMT describes the behavior of ideal gases:

1. Gas molecules are in constant, random, rapid motion.

2. Gas molecules are much smaller than the space between them.

3. Gas molecules do no experience IMFs or gravity.

4. Gas molecules have the same kinetic energy at any given temperature.

5. Gas molecules experience perfectly elastic collisions.

KE = ½ mv²

• The heavier a gas, the slower it moves at a given temperature.

• Gases move faster as temperature increase.

Maxwell-Boltzmann Distribution

O₂ is the heaviest and coldest, so moves the slowest.

H₂ is the lightest and warmest, so moves the fastest.