1. Formation of Iron Sulfate:
Iron (Fe) atoms from the iron metal react with the sulfate ions (SO4^2-) from copper sulfate, resulting in the formation of iron sulfate (FeSO4). This compound is soluble in water and produces a green-colored solution.
2. Displacement of Copper:
As the iron atoms displace the copper ions (Cu^2+) from the copper sulfate compound, metallic copper is formed. This copper is deposited on the surface of the iron metal as a reddish-brown coating.
3. Redox Reaction:
This reaction is an example of a redox reaction, involving both oxidation and reduction. Iron undergoes oxidation as its oxidation state changes from 0 (in elemental iron) to +2 (in iron sulfate). On the other hand, copper undergoes reduction as its oxidation state decreases from +2 (in copper sulfate) to 0 (in metallic copper).
Overall Reaction:
The overall chemical equation for the reaction can be written as:
Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s)
In summary, when iron reacts with copper sulfate, iron sulfate and metallic copper are formed. The iron atoms replace copper atoms in copper sulfate, leading to the formation of a green-colored iron sulfate solution and a reddish-brown copper coating on the iron metal.
