The Haber Process
Le Chatelier's principle · how conditions change the yield and rate of ammonia
N2(g) + 3H2(g) ⇌ 2NH3(g) ΔH = −92 kJ/mol
Conditions
450 °C
200 atm
Lots
Surface area of iron in the reactor
1 : 3
The plant Hover over or tap any part to find out what it does · 1 s ≈ 1 hour of plant time
Equilibrium yield i
–
% NH₃ if left to reach equilibrium
NH₃ leaving reactor i
–
% ammonia after one pass
Rate of production i
–
tonnes of NH₃ per day
Time to equilibrium i
–
how quickly the mixture settles
Graphs
Percentage of ammonia in the gas inside the reactor (hover over the reactor to see it). The dashed line is the equilibrium position.
What just happened?
Change one condition at a time and watch the yield, the rate and the molecules. This panel will explain each change using Le Chatelier's principle: if you change the conditions of a system at equilibrium, the position of equilibrium shifts to oppose the change.
Results
| # | Investigating | Temp (°C) | Pressure (atm) | Catalyst (%) | N₂ : H₂ | Recycling | Equilibrium yield (% NH₃) | NH₃ leaving reactor (%) | Rate (t/day) | Time to equilibrium (s) |
|---|---|---|---|---|---|---|---|---|---|---|
| No results yet — choose what you are investigating, set your conditions and press Record. | ||||||||||