The Haber Process for the Production of Ammonia
- Created by: alexdakota
- Created on: 14-10-15 21:03
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- The Haber Process for the Production of Ammonia
- N2(g)+3H2(g)
- reversible reaction with Fe(s) catalyst
- exothermic reaction
- = 2NH3(g)
- Optimum Conditions
- high pressure
- because there are more gas molecules in the reactants than the products
- this means equilibrium will shift to the right to oppose this change so more products are formed
- low temperature
- because the forward reaction is exothermic
- equilibrium will shift to the right to oppose this changes so more products are formed
- high pressure
- Actual Conditions
- 200 atmospheres
- because high pressures are dangerous, hard and expensive to contain and lots of energy is required
- however, this pressure is enough to still shift equilibrium to the right
- 450°C
- this is because low temperatures would slow down the rate at which ammonia is produced
- this temperature allows the rate of reaction to be worthwhile aswell as still shifting equilibrium to the right
- 200 atmospheres
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