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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 3.30 x 10-3 mol L-1, what is its molar concentration in the mixture at equilibrium.

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On taking the square not

5.656 = \(\frac{x/2}{(0.0033-x)}\)

\(\frac{x}{(0.0033-x)}\) = 11.31 or 12.31, x = 0.0037

x = \(\frac{0.037}{12.31}\) = 0.003

∴ Molar concentration of BrCl at equilibrium point

= 0.033 - 0.003 = 0.0003 mol L-1

= 3 x 10-4 mol L-1

Therefore, [BrCl] equilibrium = 3 x 10-4 mol L-1

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