Industrial reaction conditions for the production of ammonia is as shown below in the graph:

    

Describe how the yield changes as the pressure is increased.

Industrial reaction conditions for the production of ammonia is as shown below in the graph:

The ideal temperature used by Haber is approximately ${450}^{°} \mathrm{C}$. Outline the reasons why a higher temperature would be used to increase production of ammonia instead of a lower temperature.

Industrial reaction conditions for the production of ammonia is as shown below in the graph:

 A pressure of $200 \mathrm{atm}$ is used during the process. Why does industry not use a much higher pressure to maximise yield?

Industrial reaction conditions for the production of ammonia is as shown below in the graph:

Explain with reference to the position of the equilibrium why increasing the pressure of this closed system favours the forward reaction. 

The Haber's process describes the industrial production of ammonia gas on a large scale: ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\stackrel{ }{\rightleftharpoons }2{\mathrm{NH}}_3\left(\mathrm{g}\right); ∆{\mathrm{H}}^{°}=-92 \mathrm{kJ} {\mathrm{mol}}^{-1}$. Predict the effect of the following change on the position of the equilibrium in the process.

Nitrogen gas is added to the system at equilibrium.