Which of the following statements is NOT correct according to the kinetic-molecular theory of gases?

• A. Gas particles experience significant attractive and repulsive forces.
• B. The average kinetic energy of gas particles is proportional to the absolute temperature.
• C. Gas particles are in constant, random motion.
• D. The volume of individual gas particles is negligible compared to the volume of the container.

Answer: (A)

Verified step by step guidance

1. Review the key postulates of the kinetic-molecular theory of gases, which describe the behavior of ideal gases.
2. Recall that according to the theory, gas particles are considered to have negligible volume compared to the container, meaning their own size is very small relative to the space they occupy.
3. Understand that gas particles are in constant, random motion, which explains properties like pressure and diffusion.
4. Remember that the average kinetic energy of gas particles is directly proportional to the absolute temperature (measured in Kelvin), linking temperature to particle motion.
5. Identify that the statement claiming gas particles experience significant attractive and repulsive forces contradicts the theory, as it assumes these forces are negligible for ideal gases.