Concept:In reactions where gases combine to form fewer moles of gas, high pressure thermodynamically favors the product side.
Formula:$$ 4 \text{ moles of reactant gas} \rightleftharpoons 2 \text{ moles of product gas} $$
Solution:- Le Chatelier's Principle states that increasing pressure shifts equilibrium towards the side with fewer gas molecules.
- In the Haber process, 4 moles of reactants (\( \text{N}_2 + 3\text{H}_2 \)) form 2 moles of product (\( 2\text{NH}_3 \)).
- Applying 200 atm of pressure heavily forces the reaction forward, drastically increasing the yield of Ammonia.
Why other options are incorrect:It certainly doesn't lower yield or rate. High pressure actually increases costs due to the need for thick, heavy-duty industrial piping, so it is strictly done for yield, not cost reduction.
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