Haber process and LeChatelier's Principle?

Question

I have a chemistry test tomorrow, and one of our objectives is to apply LeChatelier's Principle to Haber's Process. I'm having a difficult time trying to do that. Can anyone help me please? ^-^

Answer 1

First look at the balanced equation

N2 + 3H2 == 2NH3 + Energy

Based on Le Chatelier's Principle, a high pressure will push the reaction to the right and the Haber process is run at high pressure.

Unfortunately the forward process is exothermic, so high temperature retards the production of ammonia. But a cold temperature slows the reaction rate too much. So this is a compromise and the reaction is run at a high temperature to speed the reaction, and the high pressure is used to force the reaction towards ammonia.

Removing ammonia from the reaction also help push the forward reaction.

Answer 2

LeChatelier's principle states that if you reduce the concentration of a reaction product, the equilibrium point in the reaction will shift "to the right" (more reaction product will be produced). I would think that in the Haber process, since the NH3 is a gas and is removed from the reaction as the desired product, this forces the reaction to continue producing NH3.