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.

3.2 moles of HI (g) were heated in a sealed bulb at `444^(@)C` till th

1.	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.
Answer» `K_(c)=0.0156,[Hl]=2.56M,[H_(2)]=[l_(2)]=0.32M`

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