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For the dissociation of gaseous HI, 2HI(...

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

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To find the equilibrium constant \( K_c \) for the dissociation of gaseous HI, we will follow these steps: ### Step 1: Write the balanced chemical equation The dissociation of hydrogen iodide (HI) can be represented as: \[ 2 \text{HI}(g) \rightleftharpoons \text{H}_2(g) + \text{I}_2(g) \] ### Step 2: Determine initial moles and the degree of dissociation We start with 2 moles of HI. Given that 20% of HI is dissociated at equilibrium, we can calculate the moles of HI that dissociate: ...
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