For the reversible reaction: ${\text{N}}_2(g)+3{\text{H}}_2(g)\rightleftharpoons 2{\text{NH}}_3(g)+\text{heat}$, the equilibrium shifts in the forward direction:

Using Le Chatelier's Principle:Temperature: The reaction is exothermic. Decreasing temperature shifts equilibrium toward the heat-producing side (forward).Pressure: There are $4$ moles of gas on the left and $2$ moles on the right. Increasing pressure shifts equilibrium to the side with fewer moles (forward).Concentration: Increasing reactants or removing products shifts equilibrium forward.Thus, increasing pressure and decreasing temperature favor the forward reaction.