When metallic aluminum is added to a solution containing iron(ii) sulfate a reaction occurs. what species is being oxidized in the overall reaction? when metallic aluminum is added to a solution containing iron(ii) sulfate a reaction occurs. what species is being oxidized in the overall reaction? fe2+(aq) so42−(aq) al(s) al3+(aq)?

The Balance equation is as follow,

                              2 Al + 3 FeSO₄ → Al₂(SO₄)₃ + 3 Fe

Oxidation Number of elements in reactants,
                     
                             Al  =  0
                            Fe  =  +2
                         SO₄   =  -2

Oxidation Number of elements in products,
                     
                             Al  =  =3
                            Fe  =  0
                         SO₄   =  -2
Result:
          As the oxidation state of Al has changed from 0 to +3, means it has lost 3 electrons so it is oxidized.
          And the oxidation state of Fe has changed from  +2 to 0, so it has gained 2 electrons, hence it is reduced.

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The molar mass of a substance is defined as the mass of 1 mol of that substance, expressed in grams per mole, and is equal to the mass of 6.022 × 10 23 atoms, molecules, or formula units of that substance.