2 BBC - GCSE Bitesize - Rocks and Builfin Materials - Calcium carbonate Deck
- 2 BBC - GCSE Bitesize - Rocks and Builfin Materials - Calcium carbonate Deck
Last Modified: 2013-06-02
CaCO3 > CaO + CO2
Here are the equations for the thermal decomposition of calcium carbonate:
calcium carbonate HEAT> calcium oxide + carbon dioxide
CaCO3CaO + CO2
Other metal carbonates decompose in the same way, including:
- sodium carbonate
- magnesium carbonate
- copper carbonate
Indeed, not all the carbonates of group 1 metals decompose at the temperatures reached by a Bunsen burner!
If calcium carbonate is heated strongly, it breaks down to form calcium oxide and carbon dioxide. Calcium oxide is yellow when hot, but white when cold.
Here are the equations for this reaction:
calcium carbonate calcium oxide + carbon dioxide
CaCO3 CaO + CO2
what kind of reaction is this?
Calcium oxide reacts with water to form calcium hydroxide, which is an alkali. Here are the equations for this reaction:
calcium oxide + water → calcium hydroxide
CaO + H2O → Ca(OH)2
What happens to the water in this reaction?
Carbonates react with acids to produce carbon dioxide, a salt and water. For example:
calcium carbonate + hydrochloric acid → carbon dioxide + calcium chloride + water
CaCO3 + 2HCl → CO2 + CaCl2 + H2O
- mortar, used to join bricks together, is made by mixing cement with sand and water
- concrete is made by mixing cement with sand, water and aggregate (crushed rock)
- Limestone is a valuable natural resource, used to make things such as glass and concrete.
- Limestone quarrying provides employment opportunities that support the local economy in towns around the quarry.
- Limestone quarries are visible from long distances and may permanently disfigure the local environment.
- Quarrying is a heavy industry that creates noise and heavy traffic, which damages people's quality of life.
What is the result of a
test for carbon
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