Which of the following conditions is required for maximum yield of ammonia through Haber's process?
Correct answer: D. Decreasing temperature
- A. Increasing temperature
- B. Decreasing concentration of reactant
- C. Decreasing Pressure
- D. Decreasing temperature
Explanation
The reaction between N2 and H2 to give NH3 is exothermic. N2 + 3H2 → 2NH3 ΔH = -92.46KJ/mol. Hence, the yield of ammonia can be increased by decreasing temperature as in exothermic reactions decrease in temperature favors forward reaction i.e, yield of ammonia in this case. The yield of ammonia can also be increased by increasing pressure or removing the product continuously. Hence, option D is correct.
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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