Assertion :Increase in pressure does not cause a shift in equilibrium for the formation of $H I$ . Reason: Formation of $H I$ is an exothermic reaction.

If both assertion and reason are correct and reason is the correct explaination of the assertion.

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If both assertion and reason are correct, but reason is not the correct explanation of the assertion.

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If assertion is correct, but reason is incorrect

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If assertion is incorrect, but reason is correct

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Solution

The correct option is B If both assertion and reason are correct, but reason is not the correct explanation of the assertion.
For the formation of $H I$ : $H_{2} + I_{2} \to 2 H I$ , the number of molecules of a product is equal to the no. of molecules of reactants, therefore change in pressure does not affect the position of equilibrium. Here, the formation reaction is exothermic since heat is released during the formation of the product.

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(a) Assertion and reason both are correct and reason is correct explanation of assertion.
(b) Assertion and reason both are wrong statements.
(c) Assertion is correct statement but reason is wrong statement.
(d) Assertion is wrong statement but reason is correct statement.
(e) Both assertion and reason are correct statements but reason is not correct explanation of assertion.

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Assertion :Increase in pressure does not cause a shift in equilibrium for the formation of HI. Reason: Formation of HI is an exothermic reaction.

Assertion :Increase in pressure does not cause a shift in equilibrium for the formation of $H I$ . Reason: Formation of $H I$ is an exothermic reaction.