A sample of pure PCl 5 was introduced into an evacuated vessel at 473 K- After equilibrium was attained- concentration of PCl 5 was found to be 0-5- 10 -1 mol L -1- If value of K c is 8-3- 10 -3- what are the concentrations of PCl 3 and Cl 2 at equilibrium- PCl 5 g - PCl 3 g - Cl 2 g

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Standard XII

Chemistry

Interhalogen Compounds - Preparation

A sample of p...

Question

A sample of pure ${P C l}_{5}$ was introduced into an evacuated vessel at 473 K. After equilibrium was attained, concentration of ${P C l}_{5}$ was found to be $0.5 \times 10^{- 1} m o l L^{- 1}$ . If value of $K_{c}$ is $8.3 \times 10^{- 3}$ , what are the concentrations of ${P C l}_{3}$ and ${C l}_{2}$ at equilibrium?
${P C l}_{5} (g) ⇌ {P C l}_{3} (g) + {C l}_{2} (g)$

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Solution

The equilibrium reaction is :
$P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)$
Let x M be the equilibrium concentrations of $P C l_{3}$ and $C l_{2}$ .
The equilibrium constant expression is:
$K_{c} = \frac{[P C l_{3}] [C l_{2}]}{[P C l_{5}]}$
$8.3 \times 10^{- 3} = \frac{x \times x}{0.05}$
$x = [P C l_{3}] = [C l_{2}] = 2.04 \times 10^{- 2} M$

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A sample of pure PCl5 was introduced into an evacuated vessel at 473 K. After equilibrium was attained, concentration of PCl5 was found to be 0.5×10−1mol L−1. If value of Kc is 8.3×10−3, what are the concentrations of PCl3 and Cl2 at equilibrium?PCl5(g)⇌PCl3(g)+Cl2(g)

The equilibrium reaction is :PCl5(g)⇌PCl3(g)+Cl2(g)Let x M be the equilibrium concentrations of PCl3 and Cl2.The equilibrium constant expression is: Kc=[PCl3][Cl2][PCl5]8.3×10−3=x×x0.05x=[PCl3]=[Cl2]=2.04×10−2M