`PCl_(5)` was taken 2 atm in a closed vessel at `154^(0)C`. Keeping the temperature constant, `PCl_(5) Leftrightarrow PCl_(3)+Cl_(2)` equilibrium is estabilished when 50% of `PCl_(5)` decomposes. Calculate the `K_(p)` for the equilibrium.

Explanation

To solve the problem of calculating the equilibrium constant \( K_p \) for the reaction \( PCl_5 \leftrightarrow PCl_3 + Cl_2 \), we will follow these steps:

### Step 1: Identify Initial Conditions
Initially, we have:
- \( PCl_5 = 2 \, \text{atm} \)
- \( PCl_3 = 0 \, \text{atm} \)
- \( Cl_2 = 0 \, \text{atm} \)

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