Question

The reaction

POCl3 (g) <===> POCl (g) + Cl2 (g)
is at equilibrium.
Which of the following statements describes the behavior of the system if the partial pressure of chlorine is reduced by 50%?

A. POCl3 will be consumed as equilibrium is established
B. Cl2 will be consumed as equilibrium is established

Answer 1

The correct answer is option A.

Step-by-step explanation:

`POCl_3 (g)\rightleftharpoons POCl (g) + Cl_2 (g)`

Reducing the partial pressure of chlorine gas means that removal of chlorine gas from the equilibrium will shift the equilibrium in the direction according to Le Chatelier's principle.

On a removal of product from the equilibrium shifts the reaction in the forward reaction for reestablishment.So, when the partial pressure of chlorine is reduced by 50% the equilibrium will shift in forward direction in which
`POCL_3` will be consumed to form more chlorine gas.

Hence, A is correct .