Which of the following postulate of kinetic molecular theory does not hold at low temperature and high pressure?
Correct answer: D. The volume occupied by the gas molecules is negligible as compared to the the total volume of the gas.
- A. Gases are considered to be composed of minute discrete particles called molecules.
- B. The molecules move in straight line.
- C. The pressure of gas is produced due to the collision of molecules with the wall of container.
- D. The volume occupied by the gas molecules is negligible as compared to the the total volume of the gas.
Explanation
This is because when you increase the pressure, the particles are closer together. At high pressure, they are so close together that the volume of the particles makes up a significant portion of the volume of the gas. When gases are at low pressure, they are spread far apart enough that the volume of the individual molecules is so small in comparison to the volume of the gas that you can disregard the individual volumes.
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About Kinetic Molecular Theory
Kinetic molecular theory explains gases as rapidly moving particles separated by large distances, with negligible volume and negligible intermolecular attraction in the ideal model. It relates temperature to average kinetic energy and explains gas pressure, Boyle's and Charles's laws, diffusion, effusion and the conditions under which real gases deviate from ideal behavior.
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