The Haber process is an industrial process. It produces ammonia (NH3), which is used to make fertilisers.
Nitrogen + Hydrogen ⇌ Ammonia (+heat)
N2 + 3H2 ⇌ 2NH3 (+heat)
Conditions for the Haber process
Pressure = 200 atm
Temperature = 450C
Iron catalyst
Pressure in the Haber process
200 atm
Higher pressure favours the forward reaction (as there are 4 moles of gas on the left, but only 2 on the right)
Therefore, higher pressure = higher yield
However, pressure is expensive
Temperature in the Haber process
450C
Forward reaction is exothermic, and so increasing the temperature will move the equilibrium the wrong way, decreasing the yeild (increasing the temperature decreases the yield)
However, decreasing temperature decreases the rate of reaction
450C is a compromise between a high yield and a fast rate of reaction
In the Haber process, ammonia is formed as a gas, but as it cools, it liquifies in the condenser, before being removed.
Iron Catalyst in the Haber process
Makes the reaction faster
Without the catalyst, the temperature would have to increase to give a better rate of reaction, which would decrease the yield.
Temperature in the Haber process
450C
Forward reaction is exothermic, and so increasing the temperature will move the equilibrium the wrong way, decreasing the yield (increasing the temperature decreases the yield)
However, decreasing temperature decreases the rate of reaction
450C is a compromise between a high yield and a fast rate of reaction
