For the dissociation of gaseous `HI, 2HI(g) hArr H_(2)(g)+I_(2)(g)`. If 2 moles of HI are taken initially and `20%` HI is dissociated at equilibrium then the value of `K_(c)` in a 1 litre flask at 300K will be

Explanation

To find the equilibrium constant \( K_c \) for the dissociation of gaseous \( HI \) given the reaction:

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

we will follow these steps:

### Step 1: Determine Initial Moles
Initially, we have 2 moles of \( HI \).
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