For the reaction aA rightleftharpoons lL + mM | vedclass

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(D) According to Le Chatelier's principle,if the volume of the reaction vessel is increased,the pressure decreases. To counteract this,the equilibrium

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$a > (l + m)$

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(D) According to Le Chatelier's principle,if the volume of the reaction vessel is increased,the pressure decreases. To counteract this,the equilibrium shifts towards the side with a greater number of moles of gas. Given that the degree of dissociation decreases when the volume increases,it implies that the equilibrium shifts in the backward direction (towards the reactant $A$). This happens when the number of moles of gaseous products is less than the number of moles of gaseous reactants. Therefore,$(l + m)  (l + m)$.

For the reaction $aA \rightleftharpoons lL + mM$,if the volume is suddenly increased,the degree of dissociation decreases. What does this indicate?

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