If the mixture is analyzed and found to contain 1.2 bar of Cl2, 1.6 bar of Br2 and 7.8 bar of BrCl, describe the situation

Question

Consider the gas-phase reaction, Cl₂(g) + Br₂(g) <=> 2 BrCl(g), for which K_p = 32 at 500 K. If the mixture is analyzed and found to contain 1.2 bar of Cl₂, 1.6 bar of Br₂ and 7.8 bar of BrCl, describe the situation:

Correct Answer:

B. Q < K and more products will be made to reach equilibrium.

Answer 1

Cl₂(g) + Br₂(g) <==> 2 BrCl(g)

Q = (BrCl)² /(Cl₂)(Br₂) = (7.8)2 /(1.2)(1.6)

Q = 31.69

Since Kp is 32, Q is < K and therefore in order to reach equilibrium, the reaction will have to move toward the products