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2 moles of \( P C l_{5} \) when heated in a closed vessels of 2 litre capacity at equilibrium \( 40 \% \) of \( P C l_{5} \) dissociated in \( P C l_{3} \) and \( C l_{2} . \) What is the value of the equilibrium constant?

1. 0.267
2. 0.786
3. 0.345
4. 1.879

Correct answer: 0.267

Solution

If 40% of 2 moles dissociate, 0.8 mol of PCl5 reacts to form 0.8 mol each of PCl3 and Cl2, leaving 1.2 mol PCl5. In a 2 L vessel, the equilibrium concentrations give Kc = ([PCl3][Cl2])/[PCl5] = 0.267.

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