According to the kinetic-molecular theory, which statement best describes the behavior of gas particles in an ideal gas?

• A. Gas particles occupy a significant volume compared to the total volume of the container.
• B. Gas particles lose energy during collisions with the container walls.
• C. Gas particles move in random, straight-line motion and experience elastic collisions with each other and the container walls.
• D. Gas particles are attracted to each other by strong intermolecular forces.

Answer: (C)

Verified step by step guidance

1. Recall the key postulates of the kinetic-molecular theory for ideal gases, which describe the behavior of gas particles.
2. Understand that according to the theory, gas particles are considered to have negligible volume compared to the container, so they do not occupy a significant portion of the container's volume.
3. Recognize that gas particles move in continuous, random, straight-line motion until they collide with either other particles or the container walls.
4. Note that collisions between gas particles and with the container walls are perfectly elastic, meaning no kinetic energy is lost during these collisions.
5. Acknowledge that ideal gas particles do not exert intermolecular forces on each other; they neither attract nor repel one another.