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.
Last updated
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.
Practise Chemical Equilibrium
625 free Chemical Equilibrium MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
Exams that ask Chemistry questions like this
Chemistry is on 12 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
Related questions
Adding a catalyst to a system at equilibrium
An exothermic reaction is allowed to reach equilibrium; if heat energy is then removed, the equilibrium will shift
By decreasing the pressure the reaction will go to that direction where_________________?
Change in pressure will only affect the substance which are in:
Consider the following endothermic reaction: N2(g) + O2(g) → 2NO(g). What will happen to the equilibrium if the temperature of the system is raised?