Question

If the reaction starts with a mixture of PCl5, PCl3 and Cl2 at pressures of 0.820 atm, 1.322 atm and 0.911 atm respectively, is the reaction at equilibrium

Answer 1

The reaction is not in equilibrium

Step-by-step explanation:

For the reaction:

PCl₅ ⇄ PCl₃ + Cl₂

Equilibrium constant, Kp, is defined as:

`Kp = (P_(PCl_3)P_(Cl_2))/(P_(PCl_5)) = 0.497`

When this ratio is = 0.497, the reaction is in equilibrium. Replacing the pressures of the problem, reaction quotient, Q, is:

`Q =(1.322atm*0.911atm)/(0.820atm) = 1.469`

As Q ≠ Kp, the reaction is not in equilibrium

To reach the equilibrium, the reaction will shift to the left producing more reactant and decreasing amount of products.