Assertion :A change of pressure has no effect in case of the equilibrium, $N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$ Reason: The reaction, $N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$ is highly exothermic reaction.

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 C Assertion is correct but Reason is incorrect
A change of pressure has no effect in case of the equilibrium, $N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$

The number of moles of gaseous reactants is equal to the number of moles of gaseous products.

The reaction, $N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$ is a highly endothermic reaction as the triple bond in nitrogen is very strong and requires a large amount of energy for dissociation. The enthalpy change for the reaction is -200 kJ/mol.

Hence, the assertion is correct but Reason is incorrect.

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