In the Haber process $30 \mathrm{litre}$ of dihydrogen and $30 \mathrm{litres}$ of dinitrogen were taken for reaction which yielded only  $50\%$ of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end?

In the two gaseous reactions (i) and (ii) at $250°\mathrm{C}$,

(i) $\mathrm{NO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{NO}}_2\left(\mathrm{g}\right), {\mathrm{K}}_1$

(ii) $2{\mathrm{NO}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right), {\mathrm{K}}_2$

The equilibrium constants ${\mathrm{K}}_1$ and ${\mathrm{K}}_2$ are related as:

For the reaction,

${\mathrm{CH}}_4\left(\mathrm{g}\right)+2{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CO}}_2\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right);$ ${\mathrm{\Delta }}_{\mathrm{r}}\mathrm{H}=-170.8 \mathrm{kJ} {\mathrm{mol}}^{-1}$.

Which of the following statements is not true?

The value of equilibrium constant of the reaction

$\mathrm{HI}\left(\mathrm{g}\right)\rightleftharpoons \frac{1}{2}{\mathrm{H}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{I}}_2$ is $8.0$
The equilibrium constant of the reaction
${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{I}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{HI}\left(\mathrm{g}\right)$ will be:

The values of ${\mathrm{K}}_{{\mathrm{P}}_1}$ and ${\mathrm{K}}_{{\mathrm{P}}_2}$ for the reactions $\mathrm{X}\rightleftharpoons \mathrm{Y}+\mathrm{Z}$ ........(1) and $\mathrm{A}\rightleftharpoons 2\mathrm{B}$ .......(2) are in the ratio $9:1$. If degree of dissociation of $\mathrm{X}$ and $\mathrm{A}$ be equal, then total pressure at equilibrium $\left(1\right)$ and $\left(2\right)$ are in the ratio: