A sample of `HI(g)` is placed in flask at a pressure of `0.2 atm`. At equilibrium. The partial pressure of `HI(g)` is `0.04 atm`. What is `K_(p)` for the given equilibrium?
`2HI(g) hArr H_(2)(g)+I_(2)(g)`

Explanation

To solve the problem, we need to determine the equilibrium constant \( K_p \) for the reaction:

\[ 2HI(g) \rightleftharpoons H_2(g) + I_2(g) \]

**Step 1: Identify the initial conditions and changes at equilibrium.**
- The initial pressure of \( HI \) is given as \( 0.2 \, \text{atm} \).
- At equilibrium, the partial pressure of \( HI \) is \( 0.04 \, \text{atm} \).

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