The Haber process produces a smaller volume of gas than is reacted together. What effect will increasing the pressure have on this process?
  • The amount of ammonia is smaller
  • The amount of product is increased
  • The amount of reactant produced is larger
  • The reverse reaction occurs more quickly
The forward reaction of the Haber process is exothermic. What does this mean?
  • It is faster than the reverse reaction
  • It gives out energy
  • It takes in energy
  • It is slower than the reverse reaction
If a high pressure increases the amount of ammonia produced, why is the process not performed at a much higher pressure than 200 atmospheres?
  • It is too dangerous
  • The yield is too high
  • It is too expensive
  • Too much hydrogen and nitrogen are used
Here is the equation for the Haber process: N + 3H ⇌ 2NH How many moles of gases are there on each side of the equation?
  • LHS: 3 RHS: 4
  • LHS: 4 RHS: 2
  • LHS: 2 RHS: 4
  • LHS: 2 RHS: 2
Ammonia is found in fertilisers as ammonium nitrate. Name the acid that the ammonia is reacted with to produce ammonium nitrate.
  • Hydrochloric acid
  • Sulfuric acid
  • Ethanoic acid
  • Nitric acid
If the Haber process was carried out at low temperature, it would increase the amount of ammonia produced. Why is the process NOT carried out at low temperature?
  • The forward reaction would be too slow
  • The forward reaction would be too fast
  • The reverse reaction would give out too much energy
  • The forward reaction would give out too much energy
Which of the following statements is true about the role of the iron catalyst in the Haber process?
  • It speeds up only the forward reaction
  • It affects the amount of ammonia in the equilibrium mixture
  • It is used up during the reaction
  • It increases the rate of reaction in both directions
What happens to the hydrogen and nitrogen that are not used in the reaction?
  • They are recycled
  • They are put into the air
  • They are used to make other chemicals
  • They are dissolved in water
Ammonia can also be reacted with sulfuric acid to produce ammonium sulfate. Pick the correct equation for this reaction.
  • 2NH3 + H2SO4 → (NH4SO4)2 + H2O
  • NH3 + H2SO4 → (NH4SO4)2 + H2O
  • NH3 + H2SO4 → NH4SO4 + H2O
  • 2NH3 + H2SO4 → (NH4)2SO4
The conditions that are chosen for the Haber process, 450 C and 200atm, are the best conditions for what?
  • The highest yield of ammonia
  • The fastest yield of ammonia
  • The slowest reverse reaction
  • The most ammonia as quickly as possible
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