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Question
\[\ce{PCl5, PCl3 and Cl2}\] are at equilibrium at 500 K in a closed container and their concentrations are 0.8 × 10–3 mol L–1, 1.2 × 10–3 mol L–1 and 1.2 × 10–3 mol L–1 respectively. The value of Kc for the reaction \[\ce{PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)}\] will be ______.
Options
1.8 × 103 mol L–1
1.8 × 10–3
1.8 × 10–3 L mol–1
0.55 × 104
Solution
\[\ce{PCl5, PCl3 and Cl2}\] are at equilibrium at 500 K in a closed container and their concentrations are 0.8 × 10–3 mol L–1, 1.2 × 10–3 mol L–1 and 1.2 × 10–3 mol L–1 respectively. The value of Kc for the reaction \[\ce{PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)}\] will be 1.8 × 10–3.
Explanation:
The chemical equation is given as
Kc = `([PCl_5][PCl_3])/([Cl2])`
= 0.8 × 10–3 mol L–1 × 1.2 × 10–3 mol L–1 / 1.2 × 10–3 mol L–1
= 1.8 × 10–3 mol L–1.
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