Question

Onsider this reversible reaction:

Answer 1

You can shift the equilibrium to the right if you

• Increase the concentration of PCl_5

• Increase the temperature

• Decrease the concentration of Cl_2

• Decrease the total pressure of the system

Decreasing the concentration of PCl_3 will shift the equilibrium to shift to the right, but there will be less PCl_3 at the new equilibrium.

Answer 2

Answer:

                    PCl₅(g) + heat ↔ PCl₃(g) + Cl₂(g)

              On increasing the concentration of PCl5(g), the equilibrium will shift in forward direction and produce more PCl₃.

Explanation:

               According to Le Chatlier's Principle " If we apply any external stress on a system at equilibrium, the system minimize the effect by itself to regain equilibrium". In above reaction initially  the system is in equilibrium. when we increase the concentration of reactant (PCl₅), the system goes to forward and produce more product (PCl₃).

              After some time reaction will go in backward direction to regain equilibrium position while consuming  PCl₃ and Cl₂. Finally reaction will again in equilibrium position.