7.22. Bromine monochloride (BrCl) decomposes into bromine and chlorine and reaches the equilibrium: 2BrCl (g) ⇌ Br2 (g) + Cl2 (g) The value of Kc is 32 at 500 K. If initially pure BrCl is present at a concentration of 3.3 x10-3mol L-1, what is its molar concentration in the mixture at equilibrium?

Let x moles of BrCl decompose in order to attain the equilibrium. The initial molar concentration and the molar concentration at equilibrium point of different species may be represented as follows: 2BrCl2?(g) ?→?Ar2?(g)+Cl2?(g) 3.3*10−3m 0 0 3.3*10−3−2αα? α ∴ Kc?= (α*α)? /(3.3*10−3−2α)2 ⇒ α2 / (3.3*10−3−2α)2?=32 ⇒ α / (3.3*10−3−2α)2?=4 ⇒ α=18.67*10−3−8 α ⇒ (1+ 8 α =18.67*10−3 ⇒ α= 1.5162*10−3 ∴ Molar concentration of BrCl at equation [BrCl] =3.3*10−3−2α =3.3*10−3−2*1.562*10−3 =0.267*10−3M

7.22. Bromine monochloride (BrCl) decomposes into bromine and chlorine and reaches the equilibrium:
2BrCl (g) ⇌ Br₂ (g) + Cl₂ (g)
The value of Kc is 32 at 500 K. If initially pure B_rCl is present at a concentration of 3.3 x10^-3mol L^-1, what is its molar concentration in the mixture at equilibrium?

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Vishal Baghel | Contributor-Level 10

8 months ago

Let x moles of BrCl decompose in order to attain the equilibrium. The initial molar concentration and the molar concentration at equilibrium point of different species may be represented as follows:
2BrCl₂?(g) ?→?Ar_2?(g)+Cl₂?(g)

3.3*10⁻³m 0 0

3.3*10⁻³−2αα? α

∴ Kc?= (α*α)