Two moles of `PCI_5` were heated to `327^@C` in a closed two litre vessel and when equilibrium was achieved, `PCI_5` was found to be 40% dissociated into `PCI_3 and CI_2` calculate the equilibrium constant `(K_c)` for the reaction.

Explanation

To calculate the equilibrium constant \( K_c \) for the dissociation of \( PCl_5 \) into \( PCl_3 \) and \( Cl_2 \), we can follow these steps:

### Step 1: Write the balanced chemical equation.
The dissociation of phosphorus pentachloride can be represented as:
\[ PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g) \]

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