Experimental observations on the behavior of gases can be explained by a simple theoretical model known as the kinetic molecular theory, which is used to explain the laws of gases determined experimentally.
This theory is based on a series of postulates. One of the postulates that could explain why in a sample of oxygen at constant temperature the kinetic energy of all the balls remains constant is:
- Collisions between gas particles or collisions with the vessel walls are perfectly elastic. None of the energy of a gas particle is lost when it collides with another particle or with the walls of the vessel.
Step-by-step explanation: If the oxygen particles lose energy when colliding with each other or with the walls of the container then their kinetic energy will decrease with time. This is analogous to a bouncing ball. When dropping a ball vertically, it will be observed that with each rebound it will reach a lower height, which is due to the loss of kinetic energy by friction with the ground or with the air that surrounds it.