The synthesis of ammonia is a reversible reaction. What does the term "reversible reaction" mean in a closed system?, The reaction only goes forward until all reactants are completely used up., The forward reaction stops completely once the backward reaction begins, The products can easily be converted back to reactants only by changing the catalyst., The reaction can proceed in both the forward and backward directions simultaneously., From which sources are the raw materials, nitrogen and hydrogen, obtained for the industrial manufacture of ammonia?, Nitrogen from burning fossil fuels; Hydrogen from the electrolysis of pure water., Nitrogen from the atmosphere; Hydrogen from reacting zinc with hydrochloric acid., Nitrogen from liquid air; Hydrogen from the catalytic cracking of petroleum., Nitrogen from ammonia gas; Hydrogen from natural gas., Which set of conditions represents the standard operating parameters for the Haber process in industry?, 200 oC, 450atm, Nickel catalyst, 450 oC, 200atm, Iron catalyst, 200 oC, 450atm, Iron catalyst, 450 oC, 200atm, Nickel catalyst, Why do we not use a much lower temperature, even though a lower temperature increases the equilibrium yield of ammonia?, At lower temperatures, the iron catalyst becomes completely poisoned and stops working., The forward reaction is endothermic, so it cannot occur at low temperatures., The rate of reaction would be too slow, making the process economically unviable., Lower temperatures will cause the ammonia gas to liquefy inside the reactor chamber., Which method is best used to collect a dry sample of ammonia gas?, Over water because it is insoluble in water., Downward delivery because it is denser than air., Using a calcium chloride drying tube., Upward delivery because it is less dense than air., Why is the industrial production of ammonia so vital to global society?, It is used directly as a clean fuel for modern vehicles., It is used to manufacture nitrogenous fertilizers to sustain global food production., It is the primary raw material used to manufacture plastics and nylon., It is used to neutralize acidic oceans caused by carbon dioxide emissions., In the Haber process, a pressure of 200 atmospheres (atm) is used. Even though a higher pressure (e.g., 1000 atm) would significantly increase the percentage yield of ammonia, why is a higher pressure NOT used in industry?, The cost of building and maintaining strong, explosion-proof equipment is too high, High pressure favors the backward reaction, reducing the amount of ammonia produced., The iron catalyst would be crushed and deactivated by the extreme pressure., Nitrogen and hydrogen gases would liquefy, stopping them from reacting together, In a Haber process plant, only about 15% of the nitrogen and hydrogen is converted to ammonia on each pass through the reactor. How is the remaining 85% of unreacted gas handled to ensure the process remains economically viable?, It is released safely into the atmosphere through high chimneys., It is pumped into a separate chamber and reacted with oxygen to produce water., It is cooled down, separated from the liquefied ammonia, and pumped back into the reactor., It is discarded as chemical waste because recycled gases contain too many impurities.

Ammonia

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