In a sample of oxygen gas at room temperature, the average kinetic energy of all the balls stays constant. which postulate of kinetic molecular theory best explains how this is possible?

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.

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.

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The se-ci  bonds is more polar  than s-br bond