Which statement is true about the yield of ammonia in the Haber process?

The yield of ammonia in the Haber process is influenced by temperature and pressure conditions due to the principles of chemical equilibrium and Le Chatelier's principle.

In the Haber process, nitrogen and hydrogen gases react to form ammonia, and the reaction is exothermic, meaning it releases heat. By lowering the temperature, the equilibrium shifts to favor the formation of ammonia, increasing the yield. However, very low temperatures can slow down the reaction rate, which is why a balance must be struck.

Increasing the pressure also affects yield. The reaction involves a decrease in the number of gas molecules (four moles of reactants form two moles of product). Therefore, increasing pressure shifts the equilibrium toward the side with fewer gas molecules, resulting in a higher yield of ammonia.

Using more nitrogen than hydrogen does not directly improve yield, as the stoichiometry of the reaction is crucial; a balanced ratio is essential for efficiency. Similarly, while catalysts speed up the reaction, they do not affect the position of equilibrium or the overall yield of the products. Lastly, the yield cannot remain constant regardless of conditions because the dynamic nature of the reaction allows external conditions to shift equilibrium concentrations significantly. Thus, understanding the role of temperature and pressure conditions is fundamental in maximizing ammonia yield in