Identify the species oxidized. 2 al3+(aq) + 2 fe(s) → 2 al(s) + 3 fe2+(aq)

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.

idk i’m struggling too