Concept:Maximizing yield in an industrial reversible reaction requires manipulating pressure, temperature, and concentrations according to Le Chatelier's Principle.
Formula:$$ \text{N}_{2(g)} + 3\text{H}_{2(g)} \rightleftharpoons 2\text{NH}_{3(g)} \quad \Delta H < 0 $$
Solution:- High Pressure: Shifts equilibrium right because there are fewer moles of gas on the product side (4 moles vs 2 moles).
- Low Temperature: Shifts equilibrium right because the forward reaction is exothermic (releases heat).
- Continual Removal: Dropping the concentration of \( \text{NH}_3 \) forces the system to constantly try and replace it, preventing equilibrium from ever halting the reaction.
- Combining these three factors yields the absolute maximum amount of product.
Why other options are incorrect:Low pressure favors reactants. High temperature favors reactants. Continual addition of ammonia would violently drive the reaction backwards.
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