Starting with 2 moles of PCl5 in 1 liter container 0.5 moles of PCl5 dissociates till equilibrium at 25oC, Equilibrium constant ‘KC’ is ____
Question
Starting with 2 moles of PCl5 in 1 liter container 0.5 moles of PCl5 dissociates till equilibrium at 25oC, Equilibrium constant ‘KC’ is ____
Solution
The reaction for the dissociation of PCl5 can be written as:
PCl5 ⇌ PCl3 + Cl2
Initially, we have 2 moles of PCl5. At equilibrium, 0.5 moles of PCl5 have dissociated. Therefore, we have:
PCl5: 2 - 0.5 = 1.5 moles PCl3: 0 + 0.5 = 0.5 moles Cl2: 0 + 0.5 = 0.5 moles
The equilibrium constant Kc is given by the expression:
Kc = [PCl3][Cl2] / [PCl5]
Substituting the equilibrium concentrations into this expression gives:
Kc = (0.5 * 0.5) / 1.5 = 0.1667
Therefore, the equilibrium constant Kc is 0.1667.
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