or the equilibriumPCl5(g) → PCl3 (g) + Cl2 (g)Kc = 0.19 mol dm-3 at 250°CThe equilibrium mixture at this temperature contains PCl5 at a concentration of 0.20 moldm-3 and PCl3 at a concentration of 0.010 mol dm-3 . Calculate the concentration of Cl2 inthis mixture
Question
or the equilibriumPCl5(g) → PCl3 (g) + Cl2 (g)Kc = 0.19 mol dm-3 at 250°CThe equilibrium mixture at this temperature contains PCl5 at a concentration of 0.20 moldm-3 and PCl3 at a concentration of 0.010 mol dm-3 . Calculate the concentration of Cl2 inthis mixture
Solution
To calculate the concentration of Cl2 in the equilibrium mixture, we can use the equilibrium constant (Kc) and the concentrations of PCl5 and PCl3.
Given: Kc = 0.19 mol dm-3 [PCl5] = 0.20 mol dm-3 [PCl3] = 0.010 mol dm-3
The balanced equation for the reaction is: PCl5(g) → PCl3(g) + Cl2(g)
Using the equilibrium constant expression, we have: Kc = [PCl3] * [Cl2] / [PCl5]
Substituting the given values, we get: 0.19 = (0.010) * [Cl2] / (0.20)
To find [Cl2], we can rearrange the equation: [Cl2] = (0.19 * 0.20) / 0.010
Calculating this, we find: [Cl2] = 3.8 mol dm-3
Therefore, the concentration of Cl2 in the equilibrium mixture is 3.8 mol dm-3.
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