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Limestone - Reactions of
Carbon dioxide is given off when calcium carbonate is heated.

Limestone - Reactions of

Limestone is used to make cement, glass, and building materials. This GCSE Chemistry quiz explores limestone reactions, including thermal decomposition, limewater tests, and how calcium compounds cycle in industry.

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(quiz starts below)

Fascinating Fact:

If excess carbon dioxide is bubbled through limewater, the milkiness can disappear. This is because soluble calcium hydrogencarbonate forms in solution.

In GCSE Chemistry, limestone (calcium carbonate) is a key raw material. You learn how it thermally decomposes to make calcium oxide, how calcium hydroxide forms, and how these reactions link to the limewater test and industrial processes like cement manufacture.

Key Terms

  • Thermal Decomposition: Breaking down a compound by heating it, often producing simpler substances.
  • Limewater: A dilute solution of calcium hydroxide used to test for carbon dioxide.
  • Calcium Carbonate: The main compound in limestone, with the formula CaCO3.

Frequently Asked Questions

What happens when limestone is heated in GCSE Chemistry?

When limestone (calcium carbonate) is heated strongly, it thermally decomposes into calcium oxide and carbon dioxide. This reaction is used to make lime for building and industry.

How does limewater test for carbon dioxide?

Limewater turns milky when carbon dioxide is bubbled through it because a white precipitate of calcium carbonate forms. This is a common test for carbon dioxide gas.

What is the difference between calcium oxide and calcium hydroxide?

Calcium oxide (quicklime) is made by heating limestone, while calcium hydroxide (slaked lime) forms when calcium oxide reacts with water. They have different uses in building and treating acidic soils.

Try These Related Quizzes

1 .
Calcium oxide reacts with what to form calcium hydroxide?
Hydrogen
Carbon dioxide
Water
Oxygen
This process has the trivial name of slaking and calcium hydroxide is also known as slaked lime
2 .
In the presence of carbon dioxide, what happens to limewater?
It turns brown
It turns cloudy
It decolourises
It goes brick red
The cloudiness is caused by calcium carbonate which is insoluble in alkaline conditions
3 .
The chemical name for the main mineral that is found in limestone is...
calcium carbide
calcium carbonate
sodium carbonate
sodium chloride
Limestone forms in relatively shallow tropical seas
4 .
Choose the correct equation for the reaction that produces slaked lime (calcium hydroxide).
CaO + H2O → CaOH
CaO + H2O → Ca(OH)3
CaCO3 + O2 → CaO
CaO + H2O → Ca(OH)2
This is highly exothermic
5 .
On heating, limestone breaks down into calcium oxide and carbon dioxide. What is the name of this type of reaction?
Neutralisation
Combustion
Thermal decomposition
Reduction
Thermal = heat, decomposition = breaks down
6 .
Calcium hydroxide dissolves in water to produce what?
Limewater
Quicklime
Slaked lime
Limestone
This turns cloudy when we blow into it
7 .
Limestone is badly affected by acid rain. Choose the equation below that describes this reaction.
CaCO3 + H2SO4 → CaSO4 + CO2 + O2
CaCO3 + H2SO4 → CaSO4 + CO2 + H2O
CaO + H2SO4 → CaSO4 + H2O
CaCO3 + H2SO4 → CaSO3 + CO2
The sulfuric acid of acid rain is formed from oxides of sulfur that are released into the air from burning fuels
8 .
When calcium hydroxide is reacted with carbon dioxide, the substances produced are...
Calcium oxide and oxygen
Calcium sulfate and water
Calcium carbonate and oxygen
Calcium carbonate and water
Carbon dioxide is a weak acid so this is actually a neutralisation reaction
9 .
We can use limewater to test for the presence of which gas?
Carbon dioxide
Oxygen
Methane
Nitrogen
The carbon dioxide reacts chemically with the calcium hydroxide
10 .
Which gas is given off when calcium carbonate is heated strongly?
Carbon dioxide
Nitrogen
Water vapour
Oxygen
The limestone glows with a brilliant white light when this thermal decomposition is taking place
You can find more about this topic by visiting BBC Bitesize - Limestone [GCSE Chemistry only]

Author:  Kate Gardiner (Chemistry Educator & GCSE Quiz Writer)
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