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? (3 points)

Attractive forces between gas particles are negligible because the particles of an ideal gas are moving so quickly.

Collisions between gas particles are elastic; there is no net gain or loss of kinetic energy.

Gases consist of a large number of small particles, with a lot of space between the particles.

Gas particles are in constant, random motion, and higher kinetic energy means faster movement.

Collisions between gas particles are elastic; there is no net gain or loss of kinetic energy this postulate of Kinetic Molecular Theory best explain that how this is possible.

Hence, Option B is correct answer.

What is Kinetic Molecular Theory ?

The Kinetic Molecular Theory or KMT states that gases are composed of a large number of particles. In these particles are much smaller than the distance between particles. No attraction or repulsion between these particles.

What are the Postulates of Kinetic Molecular Theory ?

The postulates of kinetic theory of gases are:

Collision are perfectly elastic.
No energy is lost or gained from collision.

There is no change in energy of either the particles or the wall upon collision.
The lighter gas molecules moves fast as compared to heavier molecules.

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.

Thus from the above conclusion we can say that Collisions between gas particles are elastic; there is no net gain or loss of kinetic energy this postulate of Kinetic Molecular Theory best explain that how this is possible.

Hence, Option B is correct answer.

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