Consider the following equilibrium in a closed container:
N₂O₄(g) ⇌ 2NO₂(g)
At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statem

Question

Consider the following equilibrium in a closed container:
N₂O₄(g) ⇌ 2NO₂(g)
At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statement holds true regarding the equilibrium constant (Kp) and degree of dissociation (α)?

Prashant Kotian · Accepted Answer

Correct answer: D. The equilibrium constant Kp depends only on temperature, so it remains unchanged. Halving the volume increases the pressure. According to Le Chatelier's principle, an increase in pressure shifts the equilibrium towards the side with fewer gaseous moles (backward direction), thereby decreasing the degree of dissociation (α). Therefore, correct answer is D.

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