JAMB - Chemistry (2005 - No. 38)
N\(_2\)(g) + 3H\(_2\)(g) ↔ 2NH\(_3\)(g) ΔH = - 90 kJ
In the equation above, the yield of ammonia can be decreased by
In the equation above, the yield of ammonia can be decreased by
increasing the pressure
removing the ammonia as it is formed
increase the temperature
adding a catalyst
Wyjaśnienie
Increasing temperature in the Haber process decreases the yield of ammonia because the forward reaction is exothermic, and Le Chatelier's principle states that increasing temperature shifts the equilibrium position towards the endothermic (reverse) direction, reducing ammonia production.