What is the effect on the Equillibirium of halving the pressure by doubling the volume on the following reaction at 300 K?
`H_2(g) + I_2(g) hArr 2HI(g)`

Explanation

To analyze the effect of halving the pressure by doubling the volume on the equilibrium of the reaction \( H_2(g) + I_2(g) \rightleftharpoons 2HI(g) \) at 300 K, we can follow these steps:

### Step 1: Identify the Reaction and Count Moles
The given reaction is:
\[ H_2(g) + I_2(g) \rightleftharpoons 2HI(g) \]

Now, let's count the number of moles of gas on each side of the reaction:
- Left side: \( 1 \, (H_2) + 1 \, (I_2) = 2 \, \text{moles} \)
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