Decomposing carbonates

Decomposing carbonates

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Decomposing carbonates

Balancing Equations

We represent decomposition of carbonates by using chemical equations. These use chemical formulae for elements and compounds and help us to see how much of each chemical is reacting.

When calcium decomposes, we can show the chemical reaction like this:

CaCO3 ---> CaO + CO2

Equations must be perfectly balanced. There must be the same number of each type of atom on both sides of the equation. The mass of the products formed in the reaction is equal to the mass of the reactants.

Count the number of each type of atom on either side of the equation, if the numbers are equal, then the equation is balanced.

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Decomposing carbonates

Calcium carbonates decomposes when we heat it, producing quicklime(calcium oxide) and carbon dioxide

Calcium carbonate +                        Sodium carbonate -

 

Potassium carbonate -                     Magnesium carbonate +

 

Zinc carbonate +                              Copper carbonate+

 

+ = decomposes                               - = does not decompose

Investigations like this show that when many carbonates are heated in a bunsen flame they decompose. They from the metal oxide and carbon dioxide-just a calcium carbonate does. Sodium and potassium carbonate do not decompose at the temperature in the bunsen flame.

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