The Haber Process (5) Flashcards
The haber process is an important industrial process. It produces ___________ which is used to make ____________
Ammonia
Fertilisers
____________ and ___________ are needed to make ammonia
Nitrogen and Hydrogen ↔ Ammonia
How is nitrogen obtained
Easily from the air
How is hydrogen obtained
From natural gas or cracking hydrocarbons
Because the reaction is reversible, not all of the nitrogen and hydrogen will convert to ___________. The reaction reaches a ____________ equilibrium
Ammonia
Dynamic
Industrial conditions:
Pressure?
200 atmospheres
Industrial conditions:
Temperature?
450°C
Industrial conditions:
Catalyst
Iron
The reaction is reversible, so there’s a _____________ to be made
Comprimise
Higher pressures favour the ____________ reaction
Forward
The percentageis set as high as possible to give the best % yield without making the plant too _____________ to build
Expensive
The forward reaction is ______thermic, which means that increasing the temperature will actually move the _____________ the wrong way - away from the ammonia and towards the N2 and H2
Exothermic
Equilibrium
The yield of ammonia would be better at __________ temperatures. The trouble is that a ___________ temperature means a __________ rate of reaction (this means that ______________ is reached more slowly). So they ___________ temperature anyway, to get a much __________ rate of reaction. 450°C is a compromise between maximum __________ and speed of __________. This is because it’s better to wait 20 seconds for a 10% yield than to have to wait 60 seconds for a 20% yield.
Lower Lower Slower Equilibrium Increase Faster Yield Reaction
The ammonia is formed as a ______, but as it cools in the ___________ it liquefies and is removed. The unused hydrogen and nitrogen are recycled so nothing is waster
Gas
Condenser
The ________ catalyst makes the reaction go ___________, but doesn’t affect the % yield
Iron
Faster
