Explain the effect of addition of an inert gason the following equilibrium reaction : 35 3 2PCl (g) PCl (g) Cl (g)+(i) under conditions of constant pressure.(ii) under conditions of constant volume

(i) Under conditions of constant pressure:

1. The addition of an inert gas does not affect the equilibrium constant (K) of the reaction.
2. According to Le Chatelier's principle, when an inert gas is added at constant pressure, the total pressure of the system increases, but the partial pressures of the reactants and products remain unchanged.
3. As a result, the equilibrium position of the reaction does not shift in either direction.
4. The concentration of each species in the reaction mixture remains the same, and the reaction proceeds at the same rate as before the addition of the inert gas.

(ii) Under conditions of constant volume:

1. The addition of an inert gas at constant volume does not affect the equilibrium constant (K) of the reaction.
2. However, according to Le Chatelier's principle, when an inert gas is added at constant volume, the total number of moles of gas in the system increases.
3. To maintain the constant volume, the system will adjust by shifting the equilibrium position in the direction that reduces the total number of moles of gas.
4. In the given reaction, the forward reaction produces 2 moles of gas (PCl3), while the reverse reaction produces 3 moles of gas (PCl2 + Cl2).
5. Therefore, the equilibrium position will shift towards the side with fewer moles of gas, which is the forward reaction in this case.
6. As a result, the concentration of PCl3 will increase, while the concentrations of PCl2 and Cl2 will decrease.
7. The reaction will continue until a new equilibrium is established with the adjusted concentrations of the reactants and products.