Which one of the following conditions will favour maximum formation of the product in the reaction

${\mathrm{A}}_{2\left(\mathrm{g}\right)}+{\mathrm{B}}_{2\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{X}}_{2\left(\mathrm{g}\right)},{\mathrm{\Delta }}_{\mathrm{r}}\mathrm{H}=-\mathrm{X} \mathrm{kJ}?$

${\mathrm{A}}_{2\left(\mathrm{g}\right)}+{\mathrm{B}}_{2\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{X}}_{2\left(\mathrm{g}\right)},{\mathrm{\Delta }}_{\mathrm{r}}\mathrm{H}=-\mathrm{XkJ}$
Given, ${\mathrm{n}}_{\mathrm{g}\left(\text{ pro }\right)}=2;{\mathrm{n}}_{\mathrm{g}\left(\text{ react }\right)}=1$
According to Lechatelier’s principle,
(i) For an exothermic reaction, $\mathrm{\Delta H}=-\mathrm{ve}$ ; decreases the temperature and shifts the equilibrium to right.
In other words, low temperature is favourable for high yield of the product (X₂).
(ii) For a given reaction, pressure increases and equilibrium shifts in the forward direction; direction in which the number of moles of the gas decreases.