Assertion :The equilibrium of $A (g) ⇌ B (g) + C (g)$ is not affected by changing the volume. Reason: $K_{c}$ for the reaction does not depend on volume of the container.

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 incorrect but Reason is correct

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Both Assertion and Reason are incorrect

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Solution

The correct option is C Assertion is incorrect but Reason is correct
The equilibrium of $A (g) ⇌ B (g) + C (g)$ is affected by changing the volume. The reaction proceeds through an increase in the number of moles of gaseous species. When the volume of the container is decreased, the pressure is increased and the equilibrium will shift in the backward direction.
$K_{c}$ for the reaction does not depend on the volume of the container. It is dependent on temperature only.
Hence, the assertion is incorrect but the Reason is correct.

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Assertion (A) Order of the reaction can be zero or fractional.

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(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.

Assertion (A) Rate constant determined from Arrhenius equation are fairly accurate for simple as well as complex molecules.

Reason (R) Reactant molecules undergo chemical change irrespective of their orientation during collision.

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Assertion :The equilibrium of A(g)⇌B(g)+C(g) is not affected by changing the volume. Reason: Kc for the reaction does not depend on volume of the container.

Assertion :The equilibrium of $A (g) ⇌ B (g) + C (g)$ is not affected by changing the volume. Reason: $K_{c}$ for the reaction does not depend on volume of the container.