Statement I: In the kinetic theory of gases, collisions between gas particles and the walls of the container are considered elastic.
Statement II: Gas molecules are considered pointlike, volumeless particles with no intermolecular forces and in constant, random motion.

Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1

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Both the Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1

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Statement 1 is correct but Statement 2 is not correct

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Statement 1 is not correct but Statement 2 is correct

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Both the Statement 1 and Statement 2 are not correct

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Solution

The correct option is B Both the Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1
Gas particles are constantly colliding with each other and the walls of a container. These collisions are elastic; that is, there is no net loss of energy from the collisions.Temperature remains the same, so the average kinetic energy and the rms speed should remain the same.
In Kinetic theory Gas molecules are considered pointlike, volumeless particles with no intermolecular forces and in constant, random motion.

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Statement I: In the kinetic theory of gases, collisions between gas particles and the walls of the container are considered elastic.Statement II: Gas molecules are considered pointlike, volumeless particles with no intermolecular forces and in constant, random motion.

Statement I: In the kinetic theory of gases, collisions between gas particles and the walls of the container are considered elastic.
Statement II: Gas molecules are considered pointlike, volumeless particles with no intermolecular forces and in constant, random motion.