`PCl_5` was found to dissociate to the extent of 42% at `227^@C` and 1 atm. Find the equilibrium constant at (i) constant pressure, and (ii) constant volume.

Explanation

To solve the problem of finding the equilibrium constant for the dissociation of \( PCl_5 \) at \( 227^\circ C \) and 1 atm, we will follow these steps:

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

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