Assertion :The pressure of a fixed amount of an ideal gas is proportional to its temperature. Reason: Frequency of collisions and their impact both increase in proportion to the square root of temperature.

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 ideal gas equation is $P V = n R T$ . Thus when amount of gas ( $n$ ) is held constant, the pressure of gas varies with temperature and volume. Hence, the assertion is incorrect.
Both frequency of collisions and impart are directly proportional to root mean square speed which is proportional to square root of absolute temperature. Hence, the 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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