Answer:
3Fe(s) → 3Fe²⁺ + 6e⁻
The oxidized is the Fe
Explanation:
2Al³⁺ (aq) + 3Fe(s) → 2 Al(s) + 3Fe²⁺(aq)
In this case, the oxidized is the Fe, where in the reactant side it acts with 0 in the oxidation number and in products side it acts with +2.
As the oxidation number was increased, this is the oxidation.
It has lost electrons.
3Fe(s) → 3Fe²⁺ + 6e⁻
All the elements in ground state acts with 0 in oxidation number (solids)
Notice that in the main reaction, in reactant side Fe, must have 3 in Stoichiometry because the reaction is unballanced.
