In the manufacture of ammonia by the Haber's process, $\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)+92.3 \mathrm{~kJ}$, which of the following conditions is unfavourable?

For the following reaction, $\mathrm{N}_{2}+3 \mathrm{H}_{2} \rightleftharpoons 2 \mathrm{NH}_{3}+923 \mathrm{~kJ}$ (i) Reducing temperature is favourable as it is an exothermic process and shift equilibrium towards right. (ii) Also on removing $\mathrm{NH}_{3}$ equilibrium shift towards right according to Le-Chatelier's principle. (iii) $\Delta n_{g}$ is negative for the process. Increase in pressure, equilibrium towards right. For an exothermic reaction, increasing ten, erature shifts the reaction to reactant side.