According to kinetic molecular theory, which of the following statements is/are correct? a. Gases consist of particles (atoms or molecules) in continuous random motion b. Collisions between particles are elastic c. The volume occupied by particles is negligibly small d. Attractive forces between particles have a negligible effect on their behaviour
Correct answer: A. All statements are correct
- A. All statements are correct
- B. Only (b) and (c)
- C. Only (a), (b) and (c)
- D. Only (a) and (b)
Explanation
According to the Kinetic Molecular Theory of gases, gas molecules are in constant random motion and exhibit elastic collisions. The volume of the gas is negligible as compared to the container and no attractive forces are present between the gas molecules. This theory can be used to explain both the Charle's and Boyle's law and is applicable to ideal gases only.
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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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