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

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

Answer: (A)

Verified step by step guidance

1. Recall the main postulates of the kinetic molecular theory (KMT) of gases, 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 and with the container walls are perfectly elastic, meaning no kinetic energy is lost during collisions.
3. Recognize that the average kinetic energy of gas particles is directly proportional to the temperature in kelvins, so it increases as temperature increases, not decreases.
4. Note that the volume of individual gas particles is considered negligible compared to the total volume of the gas, which is why gases are mostly empty space.
5. Remember that KMT assumes no intermolecular forces (no attraction or repulsion) between gas particles, so gas particles do not experience strong attractive forces.