Assertion :If a gas container is placed in a moving train, the temperature of gas will increase. Reason: Kinetic energy of gas molecules will increase.

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

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Assertion is correct but Reason is incorrect

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Assertion is incorrect but Reason is correct

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Solution

The correct option is D Assertion is incorrect but Reason is correct
The assertion is incorrect since the temperature depends only on the relative velocity of particles with respect to the container which does not change when the train moves.

Since kinetic energy has a general expression $K E = {K E}_{C M} + \frac{1}{2} m v_{c}^{2}$ where the first term is the expression of kinetic energy about centre of mass and v is the velocity of centre of masss. Since v will increase in moving train, kinetic energy of gas molecules will increase.

Hence assertion is incorrect but reason is correct.

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Similar questions

Assertion (A) All collision of reactant molecules lead to product formation.

Reason (R) Only those collisions in which molecules have correct orientation and sufficient kinetic energy lead to compound formation.

(a) Both assertion and reason are correct and the reason is correct explanation of assertion
(b) Both assertion and reason are correct, but reason does not explain assertion.
(c) Assertion is correct, but reason is incorrect
(d) Both assertion and reason are incorrect
(e) Assertion is incorrect but reason is correct.

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