A chemical engineer wants to use the Haber process in order to produce ammonia as raw material for fertilizers. Which of the following parameters must the chemical engineer AVOID in order to obtain the maximum yield of ammonia?N2(g) + 3H2(g) -> 2NH3(g) ΔH0 = -92.6 kJ/mol
Correct answer: A. Increase the temperature
- A. Increase the temperature
- B. Use a catalyst
- C. Adding more nitrogen gas
- D. Increase the pressure
Explanation
According to Le Chatelier's Principle, increasing the temperature will shift the equilibrium of the exothermic Haber process to the left, which will result in a lower yield of ammonia. Therefore, to obtain the maximum yield of ammonia, the chemical engineer should avoid increasing the temperature.
This question appeared on the NUMS 2019 (cancelled sitting) paper, which you can sit online with every answer explained.
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About Le Chatelier's Principle
Le Chatelier's principle predicts how an equilibrium responds when concentration, pressure or temperature changes. Questions apply it to reversible reactions, identify the direction of shift and distinguish genuine equilibrium changes from the effect of a catalyst, which changes the rate of reaching equilibrium but not its position.
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