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 0.45 bar of Cl₂, 0.65 bar of Br₂ and 3.1 bar of BrCl, describe the situation:

	1.	Q < K and more products will be made to reach equilibrium.
	2.	Q < K and more reactants will be made to reach equilibrium.
	3.	Within 1 decimal place, Q = K and the reaction is at equilibrium
	4.	Q > K and more products will be made to reach equilibrium.
	5.	Q > K and more reactants will be made to reach equilibrium.

Answer 1

answer : 5. Q > K and more reactants will be made to reach equilibrium.

Cl₂(g) + Br₂(g) <=============> 2 BrCl(g)

0.45      0.65                                     3.1

Q = [BrCl]^2 / [Cl2][Br2]

    = 3.1^2 / 0.45 x 0.65

    = 32.85

Q = 32.86

K_p = 32

Q > K and more reactants will be made to reach equilibrium.