Which assumption is made by the kinetic molecular theory of an ideal gas?
Correct answer: B. The volume of the molecules themselves is negligible compared with the volume of the container
- A. Gas molecules attract one another strongly
- B. The volume of the molecules themselves is negligible compared with the volume of the container
- C. Collisions between molecules lose energy as heat
- D. The molecules all move at the same speed
Explanation
The ideal model treats molecules as point masses with negligible volume and no intermolecular forces, colliding perfectly elastically so no kinetic energy is lost. Molecular speeds are not uniform but spread over the Maxwell-Boltzmann distribution, with only the average kinetic energy fixed by temperature. Real gases deviate exactly where these assumptions fail.
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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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