This question is about the industrial production of ammonia.
In the Haber process, ammonia (NH3\text{NH}_3NH3) is produced from nitrogen (N2\text{N}_2N2) and hydrogen (H2\text{H}_2H2).
During the process, unreacted nitrogen and hydrogen gases are recycled back into the reactor. Explain why these unreacted gases are recycled.
Which catalyst is used in this industrial reaction?
Describe the chemical test for hydrogen gas. Give the result if hydrogen gas is present.
- Test:
- Result:
The synthesis of ammonia is exothermic: N2(g)+3H2(g)⇌2NH3(g)\text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightleftharpoons 2\text{NH}_3(\text{g})N2(g)+3H2(g)⇌2NH3(g)
The reaction profile below represents this reaction when it is uncatalysed:
How would the reaction profile be different if a catalyst was used? Select one option:
- The final energy level of the products would be lower.
- The starting energy level of the reactants would be higher.
- The curve would reach a lower peak.
- The activation energy would be greater.
Ammonia is a key industrial precursor. Suggest one major industrial use of ammonia.