Q7 What is the effect of adding chlorine gas( at constant volume and temperature) to an equilibrium mixture of this reaction? CO(g) + Cl2(g) <~~~> COCl2(g) a. The reaction shifts towards the productsb. The reaction shifts toward the reactantsc. The reaction does not shift in either directiond. The reaction slows down

Le Chatelier’s principles, also known as the equilibrium law, are used to predict the effect of some changes on a system in chemical equilibrium. It states that equilibrium adjusts the forward and backward reactions in such a way to accept the changes affecting the equilibrium conditions. When factors like concentration, pressure, temperature, inert gases that affect equilibrium are changed, the equilibrium will shift in that direction where the effects caused by these changes are nullified.The given chemical reaction is: CO (g) + Cl2 (g) → COCl2 (g) Addition of Cl2 (g) at equilibrium will increase the reactant concentration. The forward reaction is favored as the concentration of the reactant is increased. The equilibrium of the reaction shift towards the use of reactants in the reaction, which decreases the concentration of the reactants. Therefore, the forward reaction will be favored and equilibrium will shift towards the right. Hence, the correct option is: a. The reaction shifts towards the products