Final answer:
In the synthesis of ammonia by the reaction N2(g) + 3H2(g) → 2NH3(g), an increase in reactants or a decrease in temperature or pressure will cause the reaction to shift toward the production of ammonia. An increase in products or an increase in temperature or pressure will cause the shift toward reactants.
Step-by-step explanation:
The question focuses on the chemical equilibrium of the synthesis of ammonia and its response to changes in conditions. The reaction in question is N₂ (g) + 3H₂ (g) ⇒ 2NH₃ (g), which is famously known as the Haber process. If equilibrium is disturbed for this exothermic reaction according to Le Chatelier's principle, the system will adjust to counteract the change.
When the equilibrium is stressed by an increase in reactants, the reaction will shift toward products to reduce the number of added reactants. Conversely, if the amount of products is increased, the reaction will shift toward reactants. Additionally, an increase in pressure or a decrease in temperature will also drive the reaction towards the production of more ammonia (products) because there are fewer gas molecules on the product side of the equation compared to the reactant side. However, a decrease in pressure or an increase in temperature will shift the reaction in favor of reactants.