Assumptions of the Kinetic Molecular Theory:
1. Gases consist of tiny particles (atoms or molecules) that are in constant, random motion.
2. The volume of the gas particles is negligible compared to the total volume of the container. (This is why gases are highly compressible.)
3. There are no attractive or repulsive forces between gas particles. (This is why gases tend to expand to fill their containers.)
4. Collisions between gas particles and the container walls are perfectly elastic. (No energy is lost during these collisions.)
5. The average kinetic energy of the gas particles is directly proportional to the absolute temperature of the gas. (This explains why gases expand when heated.)
The Answer:
The assumption NOT made by the kinetic molecular theory is:
* The gas particles are all moving at the same speed.
Why?
The kinetic molecular theory states that the *average* kinetic energy is proportional to temperature. This means that while some particles move faster, others move slower. The distribution of speeds is described by the Maxwell-Boltzmann distribution.
Let me know if you'd like more explanation on any of these points!
