According to the kinetic molecular theory, how does a gas exert pressure on the walls of its container?

• A. By the chemical reaction of gas particles with the container material
• B. By the expansion of gas particles as temperature increases
• C. By the attraction between gas particles and the container walls
• D. By the collisions of gas particles with the container walls

Answer: (D)

Verified step by step guidance

1. Recall the kinetic molecular theory, which describes the behavior of gas particles in terms of their motion and interactions.
2. Understand that gas particles are in constant, random motion and move in straight lines until they collide with something.
3. Recognize that gas pressure is caused by gas particles colliding with the walls of the container, transferring momentum to the walls during each collision.
4. Note that these collisions are elastic, meaning no energy is lost, and the cumulative effect of many collisions per unit area results in measurable pressure.
5. Conclude that the pressure exerted by a gas on its container walls is due to the frequency and force of these collisions, not due to chemical reactions, expansion of particles, or attractions.