The kinetic theory of gases explains the physical behavior of gases based on certain assumptions. It applies to ideal (or perfect) gases, which are theoretical models used to simplify gas behavior.
Postulates of the Kinetic Theory of Gases
1. Random Motion
- Gas molecules move randomly in straight lines, colliding with each other and with the walls of the container.
2. Elastic Collisions
- Collisions between gas molecules are perfectly elastic, meaning no energy is lost during collisions.
3. Negligible Volume
- The actual volume occupied by gas molecules is negligible compared to the volume of the container.
4. Negligible Forces of Attraction
- The forces of attraction between gas molecules are negligible, allowing them to move independently.
5. Temperature and Kinetic Energy
- The temperature of a gas is directly proportional to the average kinetic energy of its particles.
Key Insight
- This theory provides the foundation for understanding gas laws (Boyle’s, Charles’s, and Avogadro’s laws).
- Real gases deviate slightly from these assumptions under high pressure or low temperature, but the model remains a powerful tool for predicting gas behavior.
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