Which statement is true about the kinetic molecular theory?

• A. The average kinetic energy of gas particles decreases as temperature increases.
• B. Gas particles attract each other strongly, causing gases to condense easily.
• C. Gas particles are in constant, random motion and collisions between them are perfectly elastic.
• D. The volume of individual gas particles is significant compared to the total volume of the gas.

Answer: (C)

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 in constant, random motion, meaning they move in straight lines until they collide with either the container walls or other particles.
3. Recognize that collisions between gas particles are considered perfectly elastic, meaning there is no net loss of kinetic energy during collisions.
4. Note that the average kinetic energy of gas particles is directly proportional to the temperature, so it increases as temperature increases, not decreases.
5. Remember that gas particles are assumed to have negligible volume compared to the container volume, and that gas particles do not attract or repel each other significantly in an ideal gas.