A 0.366 mol sample of pcl5 (g) is injected into an empty 4.45 l reaction vessel held at 250 °c. calculate the concentrations of pcl5 (g) and pcl3 (g) at equilibrium.

Question

Carsen Johns

Chemistry

12 July, 11:04

A 0.366 mol sample of pcl5 (g) is injected into an empty 4.45 l reaction vessel held at 250 °c. calculate the concentrations of pcl5 (g) and pcl3 (g) at equilibrium.

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Dangelo Moran · Answer 1

Chemical reaction: PCl₅ → PCl₃ + Cl₂.

n (PCl₅) = 0,366 mol.

V (PCl₅) = 4,45 L.

c (PCl₅) = n (PCl₅) : V (PCl₅).

c (PCl₅) = 0,366 mol : 4,45 L.

c (PCl₅) = 0,082 mol/L.

Kc = 1,80.

[PCl₃] = [Cl₂] = x.

Kc = [PCl₃] · [Cl₂] : [PCl₅].

1,80 = x² : (0,082 mol/L - x).

Solve quadratic eqaution: x = [PCl₃] = 0,078 mol/L.

[PCl₅] = 0,082 mol/L - 0,078 mol/L.

[PCl₅] = 0,004 mol/L.