3.2 moles of HI (g) were heated in a sealed bulb at `444^(@)C` till the equlibrium was reached its degree of dissociation was found to be `20%` Calculate the number of moles of hydrogen iodide, hydrogen and iodine present at eth equlibrium point and determine the value of equlibrium constnat for the reaction `2Hl(g)hArrH_(2)(g)+I_(2)(g).` Considering the volume of the container 1 L.

Explanation

To solve the problem, we need to calculate the number of moles of hydrogen iodide (HI), hydrogen (H2), and iodine (I2) present at equilibrium, as well as the equilibrium constant (Kc) for the reaction:

\[ 2 \text{HI} (g) \rightleftharpoons \text{H}_2 (g) + \text{I}_2 (g) \]

### Step 1: Determine the initial moles of HI
We are given that there are 3.2 moles of HI initially.

### Step 2: Calculate the degree of dissociation
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