Bromine monochloride, BrCl decomposes into bromine and chlorine and reaches the equilibrium: 2BrCl (g) ⇌ Br 2 (g) + Cl 2 (g) for which K c = 32 at 500 K. If initially pure BrCl is present at a concentration of 3.3 × 10 –3 mol L –1 , what is its molar concentration in the mixture at equilibrium?

Question

Philoid · Accepted Answer

For the given reaction, let’s assume that x mol/L of BrCl decompose in order to attain equilibrium.

The given reaction is

Equilibrium constant (K_c) is defined as a number that expresses the relationship between the amounts of products and reactants present at equilibrium in a reversible chemical reaction at a given temperature.

Here, K_c = 32

For the given reaction,

Where, [Br₂]=concentration of Br₂ in mol/L at equilibrium

[Cl₂]=concentration of Cl₂ in mol/L at equilibrium

[BrCl]=concentration of BrCl in mol/L at equilibrium

Molar concentration of BrCl at equilibrium = (0.0033 mol/L – 0.003 mol/L) = 0.0003 mol/L

Bromine monochloride, BrCl decomposes into bromine and chlorine and reaches the equilibrium:2BrCl (g) ⇌ Br2 (g) + Cl2 (g) for which Kc= 32 at 500 K. If initially pure BrCl is present at a concentration of 3.3 × 10–3 mol L–1, what is its molar concentration in the mixture at equilibrium?