BRAINCAKEThe Haber Process
The Haber process is used in the manufacture of ammonia from nitrogen gas and hydrogen gas.
N2(g) + 3H2(g) &rlhar 2NH3 (g) ΔH = -92kJmol-1
Using Le Chatelier's principle, the best conditions for a high yield is a low temperature and high pressure. Both will push the equilibrium to the right.
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Key terms in this lesson
- Catalyst
- A substance that increases the rate of a chemical reaction without being used up, by providing an alternative reaction pathway with a lower activation energy.
- Le Chatelier's principle
- The principle that when a system at equilibrium is subjected to a change, the system readjusts to minimise the effect of that change.
More in Equilibrium
- Le Chatelier's Principle
- Effect of Changing the Concentration on the Position of Equilibrium
- Effects of Temperature on the Position of Equilibrium
- Effects of Pressure on the position of Equilibrium
- Effects of Catalysts on the Position of Equilibrium
- The Equilibrium Law
- Calculating the Equilibrium Constant
- Significance of the Equilibrium Constant
All 10 lessons in Equilibrium · All OCR AS-level Chemistry topics