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 move in random, straight-line motion and experience elastic collisions with each other and the container walls.
• C. Gas particles lose energy during collisions, causing the temperature to decrease over time.
• D. Gas particles are attracted to each other by strong intermolecular forces.

Answer: (B)

Verified step by step guidance

1. Recall the key postulates of the kinetic molecular theory (KMT) for ideal gases, which describe the behavior of gas particles.
2. Understand that according to KMT, gas particles are considered to have negligible volume compared to the container, meaning their own size is very small relative to the space they occupy.
3. Recognize that gas particles move in constant, random, straight-line motion until they collide with either other particles or the container walls.
4. Note that collisions between gas particles and with container walls are perfectly elastic, meaning there is no net loss of kinetic energy during collisions.
5. Remember that ideal gases assume no intermolecular forces between particles, so particles neither attract nor repel each other.