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

• A. Gas particles lose energy with each collision.
• B. Gas particles are in constant, random motion and collide elastically with the walls of the container.
• C. Gas particles attract each other strongly, causing them to condense at room temperature.
• D. The volume of a gas particle is significant compared to the total volume of the gas.

Answer: (B)

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 gas particles and with container walls are perfectly elastic (no energy loss); gas particles have negligible volume compared to the container; and there are no significant attractive or repulsive forces between particles.
3. Evaluate each statement in the problem against these postulates: - 'Gas particles lose energy with each collision' contradicts the elastic collision postulate. - 'Gas particles are in constant, random motion and collide elastically with the walls of the container' aligns with the theory. - 'Gas particles attract each other strongly' contradicts the assumption of negligible intermolecular forces. - 'The volume of a gas particle is significant compared to the total volume' 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 properties like pressure and temperature in gases, as the collisions of particles with container walls create pressure, and the kinetic energy of particles relates to temperature.