Assertion :Under free expansion, $(\frac{d U}{d V})_{T}$ is +ve when attractive forces are dominant between gas molecules [U, V, T represent internal energy, volume and temperature of gas respectively]. Reason: Internal energy is a state function.

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 B Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
When attractive forces are dominant on volume increase particles will move away against attraction force for this system requires extra energy at constant temperature, hence internal energy will increases hence $(\frac{d U}{d V})_{T}$ is +ve.

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Similar questions

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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
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(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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Assertion :Under free expansion, (dUdV)T is +ve when attractive forces are dominant between gas molecules [U, V, T represent internal energy, volume and temperature of gas respectively]. Reason: Internal energy is a state function.

Assertion :Under free expansion, $(\frac{d U}{d V})_{T}$ is +ve when attractive forces are dominant between gas molecules [U, V, T represent internal energy, volume and temperature of gas respectively]. Reason: Internal energy is a state function.