$4.5 \mathrm{mol}$ each of ${\mathrm{H}}_2$ and ${\mathrm{I}}_2$ are present in a 10 lit vessel. At equilibrium, the mixture contains 3 mole HI, $\mathrm{Kp}$ for ${\mathrm{H}}_2+{\mathrm{I}}_2\rightleftharpoons 2\mathrm{HI}$ and mass of ${\mathrm{I}}_2$ at equilibrium (in $\mathrm{g}$) respectively are

It is given to find the $K_p$for ${\mathrm{H}}_2+{\mathrm{I}}_2\rightleftharpoons 2\mathrm{HI}$ and mass of ${\mathrm{I}}_2$ at equilibrium (in $\mathrm{g}$ ) $4.5 \mathrm{mol}$ each of ${\mathrm{H}}_2$ and ${\mathrm{I}}_2$ are present in a 10 lit vessel. At equilibrium the mixture contains 3 mole HI.

4.5 moles each of hydrogen and iodine which is heated in a sealed 1olitre vessel.

${\mathrm{H}}_2( \mathrm{g})+{\mathrm{I}}_2( \mathrm{g})\leftrightharpoons 2\mathrm{HI}\left(\mathrm{g}\right)$

I   4.5            4.5             0

C -x               -x               2x

E 4.5-x          4.5- x      2x

2x= 3

x = 1.5

Since 1 mole of ${\mathrm{H}}_2$ and one mole of ${\mathrm{I}}_2$ combine to give 2 moles of HI then 3 moles of HI would be formed by ICE table,

${\mathrm{K}}_{\mathrm{C}}$$=\frac{[\mathrm{HI}{]}^2}{\left[{\mathrm{H}}_2\right]\left[{\mathrm{I}}_2\right]}$

$=\frac{[3{]}^2}{\left[3\right]\left[3\right]}$

=1

Hence the correct option is (A) 1; 0.3.