`PCl_5` dissociates as
`PCl_5(g)hArrPCl_3(g) +Cl_2(g)`
5 moles of `PCl_5` are placed in a 200 litre vessel which contains 2 moles of `N_2` and is maintained at 600 K. The equilibrium pressure is 2.46 atm. The equilibrium constant `K_p` for the dissociation of `PCl_5` is __________`xx10^(-3)`. (nearest integer)
(Given: `R = 0.082 "L atm K"^(-1) "mol"^(-1)`, Assume ideal gas behaviour)

Explanation

To solve the problem, we will follow these steps:

### Step 1: Write the dissociation equation and set up the initial conditions.
The dissociation of \( PCl_5 \) can be represented as:
\[ PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g) \]
Initially, we have:
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