DSE Chemistry
DSE Chemistry: Industrial Chemistry (Elective) — Practice Questions & Answers
Applying rate and equilibrium to industry, the Haber and Contact processes, principles of green chemistry, and the major electrolytic industries.
396 practice questions available for this topic — here are 10 with full answers and explanations.
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Practice questions with answers
1
Multiple choice · Easy
Which substance is used as the catalyst in the Haber process for manufacturing ammonia?
- Finely divided iron
- Platinum gauze
- Vanadium(V) oxide
- Nickel
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WhyFinely divided iron catalyses the reaction between N2 and H2.
2
Multiple choice · Medium
How does the catalyst increase the rate of the reaction in the Haber process?
- It provides an alternative pathway with a lower activation energy
- It increases the activation energy of the reaction
- It shifts the equilibrium to produce more ammonia
- It makes the forward reaction more exothermic
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WhyA catalyst provides an alternative reaction pathway with a lower activation energy.
3
Multiple choice · Hard
Which statement about the iron catalyst in the Haber process is correct?
- It lets equilibrium be reached faster without changing the equilibrium yield
- It increases the equilibrium yield of ammonia
- It is gradually used up and must be replaced each cycle
- It only speeds up the forward reaction
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WhyA catalyst speeds up both forward and reverse reactions equally, so equilibrium is reached sooner but the yield is unchanged.
4
Fill in the blank · Easy
In the Haber process, the reaction between nitrogen and hydrogen is catalysed by finely divided .
Answer:
iron / Fe
WhyIron (Fe) is the catalyst.
5
Fill in the blank · Medium
A catalyst increases reaction rate by providing an alternative pathway with a lower energy.
Answer:
activation
WhyActivation energy.
6
Fill in the blank · Hard
A catalyst speeds up a reaction but does not alter the position of the , so the equilibrium yield of ammonia is unchanged.
Answer:
equilibrium
WhyCatalysts do not shift equilibrium position.
7
Multiple choice · Easy
In industry, the hydrogen needed for the Haber process is mainly obtained from
- natural gas (methane) reacting with steam
- the electrolysis of molten sodium chloride
- the fractional distillation of liquid air
- the thermal decomposition of limestone
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WhyHydrogen is produced by reacting natural gas (methane) with steam.
8
Multiple choice · Medium
Which equation represents the steam reforming of methane used to make hydrogen for the Haber process?
- CH4 + H2O -> CO + 3H2
- CH4 + 2O2 -> CO2 + 2H2O
- C + H2O -> CO + H2
- 2H2O -> 2H2 + O2
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WhyCH4 + H2O -> CO + 3H2 is the steam reforming reaction.
9
Multiple choice · Hard
In the manufacture of ammonia, the nitrogen and hydrogen are obtained respectively from
- liquid air and steam reforming of methane
- steam reforming of methane and liquid air
- electrolysis of water and liquid air
- liquid air and electrolysis of brine
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WhyNitrogen comes from fractional distillation of liquid air; hydrogen from steam reforming of methane.
10
Fill in the blank · Easy
The hydrogen for the Haber process is obtained by reacting methane (natural gas) with .
Answer:
steam / water / H2O
WhySteam.
Key terms in Industrial Chemistry (Elective)
Industrial chemistry: The application of chemical reactions on a large scale to manufacture useful products.
Rate of reaction (industrial): The speed of a manufacturing reaction, optimised to maximise output economically.
Catalyst (industrial): A substance used in industry to speed reactions and lower energy costs without being consumed.
Yield (industrial): The amount of product obtained, often a compromise between rate and equilibrium position.
Optimum conditions: The set of temperature, pressure and catalyst chosen to give the best economic balance.
Haber process: The industrial process producing ammonia from nitrogen and hydrogen over an iron catalyst.
Contact process: The industrial process producing sulfuric acid via the oxidation of sulfur dioxide.
Activation energy (industrial): The energy barrier lowered by catalysts to make industrial reactions economical.
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