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Class 11
Chemistry
Equilibrium
bromine monochloride brcl decomposes into bromine...

Question:
Bromine monochloride, BrCl decomposes into bromine and chlorine and reaches the equilibrium:

2BrCl (g) ↔ Br₂ (g) + Cl₂ (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?

Answer:

Let the amount of bromine and chlorine formed at equilibrium be x. The given reaction is:

2BrCl (g) ↔ Br₂ (g) + Cl₂ (g)

Initial Conc. 3.3x10^-3 0 0

at equilibrium 3.3x10^-3 -2x x x

Now, we can write,

Kc = [Br₂][Cl₂] / [BrCl]²

⇒ (x) x (x) / (3.3x10^-3 -2x)²= 32

⇒ x / (3.3x10^-3 -2x) = 5.66

⇒ x = 18.678x10^-3 - 11.32x

⇒ x + 11.32x = 18.678x10^-3

⇒ 12.32x = 18.678x10^-3

⇒ x = 1.5 x 10^-3

Therefore, at equilibrium,

[BrCl] = 3.3x10^-3- (2 x 1.5 x 10^-3)

= 3.3x10^-3 - 3.0x10^-3

= 0.3 x 10^-3

= 3.0 x 10^-4 mol L^-1

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