Assumptions of the Kinetic Theory of Gases:
1. Particles are in constant, random motion: Gas particles move in all directions with a range of speeds, colliding with each other and the walls of their container.
2. Negligible volume of particles: Compared to the volume of the container, the volume of the individual gas particles is considered insignificant.
3. Elastic collisions: When particles collide, no energy is lost to friction or other factors. Kinetic energy is transferred between particles.
4. No intermolecular forces: Gas particles are assumed to have negligible attraction or repulsion between them.
5. Average kinetic energy is proportional to temperature: The average kinetic energy of gas particles is directly proportional to the absolute temperature of the gas.
The Non-Assumption:
The kinetic theory does NOT assume that all particles have the same speed. In reality, the particles have a distribution of speeds. Some move faster, some move slower, and the average speed is related to temperature.
Key Point: While the kinetic theory simplifies the behavior of gases, it provides a powerful framework for understanding gas properties.
