If 0.25 mol of br2 and 0.55 mol of cl2 are introduced into a 3.0-l container at 400 k, what will be the equilibrium concentration of br2

Question

Chemistry

Reyna Hines

14 December, 14:34

If 0.25 mol of br2 and 0.55 mol of cl2 are introduced into a 3.0-l container at 400 k, what will be the equilibrium concentration of br2

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Adriana Harding · Answer 1

Answer is: the equilibrium concentration of Br ₂ is 0,02 mol/L.

Chemical reaction: Br₂ + Cl₂ → 2BrCl.

Kc = 7,0.

c₀ (Br₂) = 0,25 mol : 3 L.

c₀ (Br₂) = 0,083 mol/L.

c₀ (Cl₂) = 0,55 mol : 3 L.

c₀ (Cl₂) = 0,183 mol/L.

Kc = c (BrCl) ² : c (Br₂) · c (Cl₂).

7 = (2x) ² : (0,083 mol/L - x) · (0,183 mol/L - x).

7 = 4x² : (0,083 mol/L - x) · (0,183 mol/L - x).

Solve q uadratic equation: x = 0,063 mol/L.

c (Br₂) = 0,083 mol/L - 0,063 mol/L = 0,02 mol/L.