Which of the following statements is true about the kinetic molecular theory?

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

Answer: (D)

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 and the collisions between gas particles are perfectly elastic, meaning no kinetic energy is lost during collisions.
3. Recognize that KMT assumes gas particles have negligible volume compared to the container volume, so the volume of individual particles is not significant.
4. Note that KMT states gas particles do not attract or repel each other significantly; this explains why gases do not easily condense at room temperature under ideal conditions.
5. Remember that the average kinetic energy of gas particles is directly proportional to the temperature, so it increases as temperature increases, not decreases.