In the Haber process used to produce ammonia, the conditions are $450^\circ\text{C}$ and $250$ atmospheres. Nitrogen and hydrogen are fed in a $1":"3$ ratio by volume. This reaction releases heat. $\text{N}_2\text{(g)} + 3\text{H}_2\text{(g)} \rightleftharpoons 2\text{NH}_3\text{(g)} \quad \Delta H = -92\,\text{kJ mol}^{-1}$. Which change would lead to a higher yield of ammonia?
- Adecreasing the concentration of nitrogen
- Bdecreasing the pressure
- Cdecreasing the temperature
- Dusing equal amounts of the two reactants