I'm here to help you with that question. Let's go through the provided options:
1. The kinetic energy of the molecules changes continuously
- This is a correct assumption of the kinetic theory of ideal gases. The kinetic energy of gas molecules is directly related to their motion and temperature.
2. A gas consists of a large number of molecules
- This is also a valid assumption. Gases are composed of a large number of molecules that move freely and independently of each other.
3. The gas molecules are in a state of continuous random motion
- This is another correct assumption. According to the kinetic theory of gases, gas molecules are in constant, random motion.
4. The attraction between the molecules is negligible
- This is the assumption that is NOT part of the kinetic theory of ideal gases. In reality, there can be interactions (attractions or repulsions) between gas molecules, especially at close distances.
Therefore, the correct answer is:
- The attraction between the molecules is negligible
I hope this clarifies things for you! Let me know if you need further assistance.
