Consider the given equilibrium reaction at 473 K, namely $$\text{Li}_3\text{N}(s) + 2\text{H}_2(g) \rightleftharpoons \text{LiNH}_2(s) + 2\text{LiH}(s)$$ with $$\Delta H_{rxn}^\circ = -200$$ kJ per mol. The number of moles of $$\text{H}_2(g)$$ present at equilibrium can be maximised by

A

increasing the temperature and increasing the pressure

B

increasing the temperature and decreasing the pressure

C

decreasing the temperature and increasing the pressure

D

decreasing the temperature and decreasing the pressure