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Law of Conservation of Matter
The main reason atoms cannot be destroyed in a chemical reaction is The Law of Conservation of Matter. The law states that matter can neither be created nor destroyed. This also holds true for atoms. Because atoms are neither created nor destroyed in a chemical reaction, when a compound breaks down, the atoms remain unchanged. What happens on one side of the chemical reaction or equation must also be present in the product or end result.
Balancing Equations
The Law of Conservation of Matter is evident in balancing a chemical equation. In a chemical reaction, what appears on the left side of the equation must also appear on the right side of the equation. For example, if you have 17 atoms on the reactant side (the starting materials in a reaction), then you must account for all 17 atoms on the product side. All that occurs is that the atoms rearrange themselves to form new compounds.
Example
If you combine ethylene and oxygen, the reaction will produce carbon dioxide and water. The equation is expressed as C2H4 + 3O2 --> 2CO2 + 2H2O. There are two carbons, six oxygens and four hydrogens on the reactant side. There is also the same amount of all three elements on the product side. This is a balanced equation.
Law of Conservation of Mass
The Law of Conservation of Mass is equivalent to the Conservation of Matter. Since the number of atoms in a chemical reaction never changes, neither does the mass or weight. The total mass of the reactants must be equivalent to the total mass of the products. So no matter what goes on during the reaction, the mass of the substances must remain constant. For example, in the equation 2H2 + O2 --> 2H2O, the mass of the hydrogen and oxygen must equal the mass of the water that is produced. The two hydrogens on the left equal four atomic mass units (amu) and when combined with the 32 amu of oxygen, it equals 36 amu. The water that is produced must also have 36 amu.