Final answer:
The reaction of nitrogen gas (N₂) and hydrogen gas (H₂) to produce ammonia (NH₃) in the industrial process is known as the Haber process. It is a synthesis reaction used to manufacture ammonia for fertilizer, where nitrogen and hydrogen react under specific conditions to form ammonia with maximum yield when present in excess.
Step-by-step explanation:
The industrial process involving the reaction of nitrogen gas (N₂) and hydrogen gas (H₂) to produce ammonia (NH₃) is known as the Haber process. This is a type of chemical reaction that falls under the category of synthesis or combination,
where two or more reactants combine to form a single product. In this case, nitrogen and hydrogen gases react under high pressure and temperature, in the presence of a catalyst, to produce ammonia, which is a key ingredient in fertilizer.
The balanced chemical equation for the production of ammonia through the Haber process is: N₂(g) + 3H₂(g) → 2NH₃(g). This demonstrates that one mole of nitrogen reacts with three moles of hydrogen to yield two moles of ammonia.
For example, if you are given 6.2 moles of nitrogen, you could produce 12.4 moles of ammonia, and you would require 18.6 moles of hydrogen to fully react with the nitrogen. In order to produce 11 moles of ammonia, you would need to start with 5.5 moles of nitrogen.
To achieve maximum yield in the production of fertilizer from ammonia, it is crucial to have an excess of nitrogen and hydrogen gases, given their role as starting materials in the Haber cycle.