Which of the following statements about the kinetic molecular theory of gases is incorrect?

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

Answer: (B)

Verified step by step guidance

1. Step 1: Understand the kinetic molecular theory (KMT) of gases, which describes the behavior of ideal gases based on several key assumptions about gas particles.
2. Step 2: Review the first statement: Gas particles are in constant, random motion and collide elastically with each other and the walls of the container. This is a fundamental postulate of KMT and is correct.
3. Step 3: Examine the second statement: Gas particles experience strong intermolecular forces that significantly affect their motion. According to KMT, gas particles are assumed to have negligible intermolecular forces, so this statement contradicts the theory and is incorrect.
4. Step 4: Consider the third statement: The volume of individual gas particles is negligible compared to the total volume of the gas. This is another key assumption of KMT, making this statement correct.
5. Step 5: Analyze the fourth statement: The average kinetic energy of gas particles is directly proportional to the absolute temperature of the gas. This is a core concept in KMT and is correct.