Answer
See the complete table below:
Work Step by Step
First, write the equilibrium expression for the reaction $H_{2}(g) + I_{2}(g) \leftrightharpoons 2HI(g) $
Equilibrium constant $K_{eq} = \frac{[HI]^{2}}{[H_{2}][I_{2}]}$
Now, in the 1st row, we have to find $k_{eq}$. All the other values are given.
After putting all the values in the equilibrium expression we have
$K_{eq} = \frac{0.0922^{2}}{0.355\times0.388} \approx 0.0617$
In the 2nd row, we have to find $[H_{2}]$.
$[H_{2}] = \frac{[HI]^{2}}{[H_{2}]k_{eq}} = \frac{0.387^{2}}{9.6\times0.0455} \approx 0.343$
In the 3rd row, we have to find $[HI]$
$[HI] = \sqrt{k_{eq}[H_{2}][I_{2}]} = \sqrt{50.2\times0.0485\times0.0468}\approx 1.067$
