What are the optimal conditions for the Haber Process N2(g) + 3H2(g) <--> 2NH3(g)? Use Le Chatelier's principle to derive your answer.

When considering the optimal reaction conditions, one must check for pressure, temperature, concentration and catalysts involved. Le Chatelier's principle states that if a change to the system is made, the chemical equilibrium will shift in a way such that the applied changes are counteracted. The goal therefore, is to maximize the amount of product by applying changes that will shift the equilibrium to product side.To determine the pressure, the number of species on each side must be considered. As there are fewer molecules on the product side (2) than the reactant side (4), the reaction is favored by HIGH pressures since that will drive it towards the side with fewer molecules. This value is usually around 200 atmTo determine the temperature, the heat of reaction must be considered. The reaction is exothermic (produces heat), therefore to induce that effect, the reaction should occur at low temperatures. This value is usually around 400-450 CTo determine the concentration/feed ratios, the molar quantities of feed required to produce the product must be considered. A mol of nitrogen reacts with 3 mols of hydrogen, therefore the optimal ratio is 3:1 H2 to N2.The catalysts cannot be deduced from the given reaction and is instead determined by standards in industry. Iron Oxide catalysts are the most common catalyst used for the Haber process due to its low cost and availability. However, newer processes have emerged where Ruthenium catalyst are used. In an exam condition you would answer with iron oxide.The reason why students learn about this reaction is due to its significant importance in our lives. Ammonia is used mainly to produced fertilizers, and are the reason why we can eat and live on this planet as we currently do. Furthermore, it is a perfect example of the importance of Le Chatelier's principle. Before its discovery, fertilizers were produced from nitrous acids or by separating it from vegetable or animal products. Only by understanding Le Chatelier's principle were we able to discover a 'direct' route for producing ammonia on mass scales. And as a result of this discovery, our population has been booming. Graphs online for trends of global ammonia production vs the global population, show strong correlations.