Kinetic molecular theory

Definition

The kinetic molecular theory explains the behavior of gases in terms of motion and energy of their molecules. It states that gas particles are in constant, random motion and that the temperature of a gas is proportional to the average kinetic energy of its molecules.

5 Must Know Facts For Your Next Test

1. Gas particles are in constant, random motion.
2. The volume of individual gas particles is negligible compared to the volume of the container.
3. Collisions between gas particles are perfectly elastic, meaning no energy is lost.
4. The average kinetic energy of gas particles is directly proportional to the temperature in Kelvin.
5. There are no intermolecular forces acting between ideal gas particles.

Review Questions

• How does temperature affect the average kinetic energy of gas molecules?
• What assumptions does the kinetic molecular theory make about collisions between gas particles?
• Why are intermolecular forces considered negligible in an ideal gas according to the kinetic molecular theory?

Related terms

Ideal Gas Law: $PV = nRT$, where $P$ is pressure, $V$ is volume, $n$ is moles, $R$ is the universal gas constant, and $T$ is temperature.

Boyle's Law: $P_1V_1 = P_2V_2$, stating that for a given amount of gas at constant temperature, pressure and volume are inversely proportional.

Charles's Law: $\frac{V_1}{T_1} = \frac{V_2}{T_2}$, indicating that for a given amount of gas at constant pressure, volume is directly proportional to temperature.