Chemistry · Factors affecting equilibrium: concentration, pressure, temperature, the effect of catalyst, Le Chatelier's principle
As per Braun's principle, yield of Ammonia will be more in Haber's process under
As per Braun's principle, yield of Ammonia will be more in Haber's process under conditions \( \boldsymbol{L}=\operatorname{Low} ; \boldsymbol{H}=\operatorname{high} ; \boldsymbol{T}=\operatorname{Temp} ; \boldsymbol{P}= \) Pressure)
- A. \( L T ; L P \)
- B. \( L T ; H P \)
- C. \( H T ; H P \)
- D. \( H T ; L P \)
Step-by-step solution
Braun's principle (Le Chatelier's principle) states that a system at equilibrium will shift to counteract changes. The Haber process is exothermic, so low temperature shifts equilibrium toward ammonia. Also, the reaction reduces the number of gas molecules (4 to 2), so high pressure favors product formation. Thus, low temperature and high pressure maximize yield.
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