The Haber process produces a smaller volume of gas than is reacted together. What effect will increasing the pressure have on this process?
0%
The amount of ammonia is smaller
100%
The amount of product is increased
0%
The amount of reactant produced is larger
0%
The reverse reaction occurs more quickly
Q.2.
The forward reaction of the Haber process is exothermic. What does this mean?
0%
It is faster than the reverse reaction
100%
It gives out energy
0%
It takes in energy
0%
It is slower than the reverse reaction
Q.3.
If a high pressure increases the amount of ammonia produced, why is the process not performed at a much higher pressure than 200 atmospheres?
0%
It is too dangerous
0%
The yield is too high
50%
It is too expensive
50%
Too much hydrogen and nitrogen are used
Q.4.
Here is the equation for the Haber process: N + 3H ⇌ 2NH How many moles of gases are there on each side of the equation?
50%
LHS: 3
RHS: 4
50%
LHS: 4
RHS: 2
0%
LHS: 2
RHS: 4
0%
LHS: 2
RHS: 2
Q.5.
Ammonia is found in fertilisers as ammonium nitrate. Name the acid that the ammonia is reacted with to produce ammonium nitrate.
0%
Hydrochloric acid
50%
Sulfuric acid
0%
Ethanoic acid
50%
Nitric acid
Q.6.
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?
33%
The forward reaction would be too slow
0%
The forward reaction would be too fast
67%
The reverse reaction would give out too much energy
0%
The forward reaction would give out too much energy
Q.7.
Which of the following statements is true about the role of the iron catalyst in the Haber process?
0%
It speeds up only the forward reaction
50%
It affects the amount of ammonia in the equilibrium mixture
0%
It is used up during the reaction
50%
It increases the rate of reaction in both directions
Q.8.
What happens to the hydrogen and nitrogen that are not used in the reaction?
100%
They are recycled
0%
They are put into the air
0%
They are used to make other chemicals
0%
They are dissolved in water
Q.9.
Ammonia can also be reacted with sulfuric acid to produce ammonium sulfate. Pick the correct equation for this reaction.
0%
2NH3 + H2SO4 → (NH4SO4)2 + H2O
50%
NH3 + H2SO4 → (NH4SO4)2 + H2O
0%
NH3 + H2SO4 → NH4SO4 + H2O
50%
2NH3 + H2SO4 → (NH4)2SO4
Q.10.
The conditions that are chosen for the Haber process, 450 C and 200atm, are the best conditions for what?
0%
The highest yield of ammonia
50%
The fastest yield of ammonia
0%
The slowest reverse reaction
50%
The most ammonia as quickly as possible
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