What would happen to a reversible reaction at | vedclass

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(D) When an inert gas is added to a system at equilibrium at constant pressure,the total volume of the system increases. As a result,the concentration

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It remains unaffected

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(D) When an inert gas is added to a system at equilibrium at constant pressure,the total volume of the system increases. As a result,the concentration (moles per unit volume) of all gaseous reactants and products decreases. According to Le Chatelier's principle,the equilibrium will shift in the direction that increases the total number of moles of gaseous species to counteract the decrease in concentration. If the number of moles of gaseous products is greater than the number of moles of gaseous reactants,the reaction shifts towards the product side. If the number of moles of gaseous reactants is greater than the number of moles of gaseous products,the reaction shifts towards the reactant side. If the total number of moles of gaseous reactants equals the total number of moles of gaseous products,the equilibrium remains unaffected.

What would happen to a reversible reaction at equilibrium when an inert gas is added while the pressure remains unchanged?

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