Consider the following statements regarding chemical equilibrium and Le Chatelier principle: 1. Increasing the pressure on an equilibrium gaseous system with a decrease in total moles of gas shifts the equilibrium in the forward direction. 2. Adding an inert gas at constant volume to a gaseous equilibrium system alters the molar concentrations of reactants and products, shifting the equilibrium position. Which of the statements given above is/are correct?

💡 Solution & Explanation

According to Le Chatelier principle, increasing pressure on a gaseous equilibrium system shifts the reaction toward the side with fewer moles of gas to counteract the stress. However, adding an inert gas at constant volume increases the total pressure without changing the individual partial pressures or molar concentrations of the reacting species, leaving the equilibrium position completely unaffected. Catalyst addition also leaves the equilibrium position unchanged while speeding up attainment of equilibrium.