Question

For the reaction PCl5(g) <--> PCl3(g) Cl2(g) at equilibrium, which statement correctly describes the effects of increasing pressure and adding PCl5, respectively

Answer 1

The given question is incomplete. The complete question is :

For the reaction
`PCl_5(g)\rightleftharpoons PCl_3(g)+Cl_2(g)` at equilibrium, which statement correctly describes the effects of increasing pressure and adding
`PCl_5`, respectively

a) Increasing pressure causes shift to reactants, adding
`PCl_5` causes shift to products.

b) Increasing pressure causes shift to products ,adding
`PCl_5` causes shift to reactants.

c) Increasing pressure causes shift to products, adding
`PCl_5` causes shift to products.

d) Increasing pressure causes shift to reactants,adding
`PCl_5` causes shift to reactants

Answer: Increasing pressure causes shift to reactants, adding
`PCl_5` causes shift to products.

Step-by-step explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

For the given equation:

`PCl_5(g)\rightleftharpoons PCl_3(g)+Cl_2(g)`

a) If the pressure is increased, the volume will decrease according to Boyle's Law. Now, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where decrease in pressure is taking place. As the number of moles of gas molecules is lesser at the reactant side. So, the equilibrium will shift in the left direction. i.e. towards reactants.

b) If
`PCl_5` is added, the equilibrium will shift in the direction where
`PCl_5` is decreasing. So, the equilibrium will shift in the right direction. i.e. towards products.