Which of the following is a postulate of the kinetic molecular theory of gases?

• A. Gas particles are strongly attracted to each other.
• B. The average kinetic energy of gas particles decreases as temperature increases.
• C. Gas particles are in constant, random motion and collide elastically with the walls of the container.
• D. The volume of the gas particles is significant compared to the total volume of the gas.

Answer: (C)

Verified step by step guidance

1. Recall that the kinetic molecular theory of gases is a model that explains the behavior of ideal gases based on the motion and interactions of gas particles.
2. Identify the key postulates of the kinetic molecular theory, which include: gas particles are in constant, random motion; collisions between particles and container walls are elastic (no energy loss); the volume of individual gas particles is negligible compared to the container volume; and there are no significant attractive or repulsive forces between particles.
3. Evaluate each given statement against these postulates: - 'Gas particles are strongly attracted to each other' contradicts the assumption of negligible intermolecular forces. - 'The average kinetic energy of gas particles decreases as temperature increases' contradicts the direct relationship between temperature and kinetic energy. - 'Gas particles are in constant, random motion and collide elastically with the walls of the container' aligns perfectly with the kinetic molecular theory. - 'The volume of the gas particles is significant compared to the total volume of the gas' contradicts the assumption that particle volume is negligible.
4. Conclude that the correct postulate is the one stating that gas particles are in constant, random motion and collide elastically with the container walls.
5. Understand that this postulate explains gas pressure as the result of collisions of particles with the container walls and supports the ideal gas behavior.