Statement 1: According to the Kinetic Moecular Theory, the particles of a gas are in random motion at absolute zero temperature.
Statement 2: The degree of random motion of gas molecules varies inversely with the temperature of the gas.

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

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Both 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 E
Statement 1 is not correct but Statement 2 is correct

Statement 1: According to the Kinetic Molecular Theory, the particles of a gas are in random motion at all temperatures except absolute zero. The particles move in all directions in straight lines until their direction is changed on collision with each other. The average kinetic energy of molecules is directly proportional to the absolute temperature. At absolute zero, the average kinetic energy of gas molecules is zero. Hence, the velocity of gas molecules is zero.
Statement 2: The degree of random motion of gas molecules varies directly with the temperature of the gas. Higher is the temperature, higher is the degree of random motion.
Hence, both statements 1 and 2 are not correct.

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Statement 1: According to the Kinetic Moecular Theory, the particles of a gas are in random motion at absolute zero temperature.Statement 2: The degree of random motion of gas molecules varies inversely with the temperature of the gas.

Statement 1: According to the Kinetic Moecular Theory, the particles of a gas are in random motion at absolute zero temperature.
Statement 2: The degree of random motion of gas molecules varies inversely with the temperature of the gas.