According to the kinetic molecular theory, how do gas particles exert pressure on the walls of their container?

• A. By expanding in size and pushing against the walls
• B. By attracting the walls through intermolecular forces
• C. By forming bonds with the container material
• D. By colliding with the walls and transferring momentum during each collision

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 either each other or the walls of their container.
3. Recognize that gas particles do not expand in size, nor do they form bonds with the container or attract the walls through intermolecular forces in an ideal gas scenario.
4. Focus on the concept that pressure is caused by gas particles colliding elastically with the container walls, transferring momentum during each collision.
5. Conclude that the pressure exerted by a gas on the walls of its container arises from the cumulative effect of many such collisions per unit area and per unit time.