Which of the following statements about the kinetic molecular theory is NOT correct?

• A. Gas particles are in constant, random motion and collide elastically with each other and the walls of the container.
• B. The average kinetic energy of gas particles is directly proportional to the absolute temperature of the gas.
• C. The volume of individual gas particles is negligible compared to the volume of the container.
• D. Gas particles experience strong attractive and repulsive forces between each other.

Answer: (D)

Verified step by step guidance

1. Review the key postulates of the kinetic molecular theory (KMT) for gases, which describe the behavior of ideal gas particles.
2. Recall that according to KMT, gas particles are in constant, random motion and collisions between them and the container walls are perfectly elastic, meaning no energy is lost during collisions.
3. Understand that the average kinetic energy of gas particles is directly proportional to the absolute temperature (in Kelvin), which means as temperature increases, particle speed and kinetic energy increase.
4. Recognize that the volume of individual gas particles is considered negligible compared to the total volume of the container, allowing gases to be treated as point particles in ideal conditions.
5. Identify that the statement 'Gas particles experience strong attractive and repulsive forces between each other' contradicts the KMT assumption that there are no intermolecular forces acting between ideal gas particles, making this statement incorrect.