Shown below is the Haber process for the commercial production of ammonia.

N₂(g) + 3H₂(g) <=====> 2NH₃(g) + 92 kJ

Discuss how Haber maximized the production of ammonia by manipulating this equilibrium. Also point out the importance of this industrial process to a growing world population. Make sure to establish a link between ammonia and protein.

Haber process

Step-by-step explanation

N2(g) + 3H2(g) <=====> 2NH3(g) + 92 kJ

yield can be maximised in following way

1 ) by using catalyst eg - Fe

2 ) optimising temperature since reaction is exothermic so low temperature is favourable for forward reaction.But since rate of reaction reduces due to low temperature catalyst is employed.

3 ) by increasing pressure reaction shifts in forward direction according to Le - Chatlier principle.

4 ) removal of product ( ammonia) at equilibrium facilitate more product formation.

If you look at a graph of global population, you will see it shoot upwards just as Haber-Bosch fertilisers start being widely applied. 

Haber-Bosch was the only reason for the spike in food yields.

Nitrogen processing is critical for the mass production of ammonia and fertilizer, necessary to help feed our growing world population and meet the needs for industrial and institutional applications. We help nitrogen producers minimise water risk, maximise performance and optimise safety, reliability and profitability to help ensure the livelihood of future generations.