Concept:Le Chatelier's Principle dictates optimal conditions for the Haber process based on thermodynamics and stoichiometry.
Formula:$$ \text{N}_2 + 3\text{H}_2 \rightleftharpoons 2\text{NH}_3 \quad \Delta H < 0, \Delta n = -2 $$
Solution:- The reaction produces heat (exothermic). Decreasing the temperature shifts the equilibrium forward to replace lost heat, yielding more \( \text{NH}_3 \).
- The reaction goes from 4 moles of gas to 2 moles of gas. Increasing pressure favors the side with fewer moles of gas to reduce pressure. Thus, high pressure shifts it forward.
- Therefore, maximum yield requires Low Temperature and High Pressure.
Why other options are incorrect:High temperature would shift the reaction backwards. Low pressure would favor the side with more moles (reactants).
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