Reaction Prediction Worksheet #1a: Decompositions

Review: Decomposition reactions are those reactions which a single reactant is split apart.  This will most often be accomplished with heating, but can occasionally require electrical current to initiate.  When heated, the compounds formed in the combination reactions can decompose.  

Binary compounds decompose into their elements.

2HgO Ú 2Hg + O2

Acids can decompose into non-metallic oxides and water.

H2CO3 Ú H2O + CO2

Metallic hydroxide compounds (bases) can decompose into metallic oxides and water.

Ba(OH)2 Ú BaO + H2O

In addition, there are two special new kinds of decompositions you will need to know.

Metallic carbonates decompose into carbon dioxide and metallic oxides.

CuCO3 Ú CO2 + CuO

Metallic chlorates decompose into oxygen gas and metallic chlorides.

2NaClO3 Ú 3O2 + 2NaCl

Additionally, some compounds are stored in a hydrated form where the formula contains a certain number of attached water molecules.  These compounds can be decomposed into the anhydrous form of the compound and water.

CuSO4. 5H2O Ú CuSO4 + 5H2O
 
1.     CaCO3à 11.     Ba(ClO3)2à
2.     H2SO3à  12.     ZnOà
3.     Al(ClO3)3à 13.     BaCl2.2H2Oà
4.     MgCO3 à 14.     Cu(OH)2à
5.     H3PO4à 15.     ZnCO3à
6.     PbO à 16.     H2SO4 à
7.     KClO3à 17.     Ni(OH)2à
8.     CdCO3à 18.     SbCl3à
9.     NaOHà 19.     Na2CO3à
10.   Na2SO4. 4H2Oà 20.     KClO3à

 

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