An increase in pressure would generally increase the yield of ammonia in accordance with Le Chatelier's principle. This principle states that if you change the conditions of a chemical equilibrium, the system will adjust to counteract that change. Here's why:
1. Balanced Equation: The synthesis of ammonia is represented by the balanced chemical equation: N₂(g) + 3H₂(g) ⇌ 2NH₃(g). This reaction involves the conversion of nitrogen gas (N₂) and hydrogen gas (H₂) into ammonia gas (NH₃).
2. The Principle: When pressure is increased, the system will shift in the direction that reduces the change in pressure. In this case, since there are four moles of gas on the left side (N₂ and 3H₂) and only two moles on the right side (2NH₃), an increase in pressure favors the forward reaction, which generates more ammonia gas.
3. Equilibrium Shift: As you increase the pressure, the equilibrium position of the reaction will shift to the right, promoting the formation of more ammonia molecules.
So, increasing pressure under constant temperature and other conditions will result in a higher yield of ammonia by favoring the forward reaction and leading to the production of more ammonia gas molecules.