Equilibrium constant question?

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Answer 1 · 2016-09-09T14:09:42

$["HCl"] = "55 mol/L"$ .

Your chemical equation is

$"2HBr" + "Cl"_2 ⇌ "2HCl" + "Br"_2$

$K_c = (["HCl"]^2["Br"_2])/(["HBr"]^2["Cl"_2]) = 1.0 × 10^4$

In your problem, the equilibrium concentrations are

$["HBr"] = "0.075 mol/L"$
$["Cl"_2] = "0.50 mol/L"$
$["Br"_2] = "0.037 mol/L"$

∴ $(["HCl"]^2 × 0.037)/(0.075^2 × 0.50) = 4.0 × 10^4$

$["HCl"]^2 = (0.075^2 × 0.50 × 4.0 × 10^4)/0.037 = 30400$

$["HCl"] = "55 mol/L"$