Which one of the following is NOT a statement of the kinetic molecular theory?

• A. The average kinetic energy of gas particles is directly proportional to the temperature in kelvins.
• B. Gas particles attract each other strongly at all times.
• C. The volume of individual gas particles is negligible compared to the volume of the container.
• D. Gas particles are in constant, random motion.

Answer: (B)

Verified step by step guidance

1. Recall that the kinetic molecular theory (KMT) describes the behavior of ideal gases based on several key assumptions about gas particles.
2. List the main postulates of KMT: (1) Gas particles are in constant, random motion; (2) The volume of individual gas particles is negligible compared to the container volume; (3) Gas particles do not exert attractive or repulsive forces on each other; (4) Collisions between gas particles are perfectly elastic; (5) The average kinetic energy of gas particles is directly proportional to the temperature in kelvins.
3. Analyze each given statement and compare it to the KMT postulates: Confirm that statements about average kinetic energy, negligible particle volume, and constant random motion align with KMT.
4. Identify the statement that contradicts KMT: 'Gas particles attract each other strongly at all times' conflicts with the assumption that there are no intermolecular forces in ideal gases.
5. Conclude that the statement about strong attraction between gas particles is NOT part of the kinetic molecular theory.