Which statement is true according to the kinetic molecular theory?

• A. The volume of the individual gas particles is significant compared to the total volume of the gas.
• B. Gas particles are in constant, random motion and collide elastically with each other and the walls of the container.
• C. Gas particles lose energy with every collision.
• D. Gas particles attract each other strongly, causing them to stick together.

Answer: (B)

Verified step by step guidance

1. Recall the main postulates of the kinetic molecular theory (KMT) which describe the behavior of ideal gases.
2. Understand that according to KMT, gas particles are considered to have negligible volume compared to the container volume, so the volume of individual particles is insignificant.
3. Recognize that KMT states gas particles are in constant, random motion and that collisions between particles and with container walls are perfectly elastic, meaning no net loss of kinetic energy occurs during collisions.
4. Note that KMT assumes no attractive or repulsive forces between gas particles, so they do not stick together or lose energy upon collision.
5. Conclude that the true statement according to KMT is that gas particles are in constant, random motion and collide elastically with each other and the walls of the container.