Question

When metallic aluminum is added to a solution containing iron(II) sulfate a reaction occurs. What species is being oxidized in the overall reaction? Al(s) Fe2+(aq) SO42−(aq) Al3+(aq)

Answer 1

Answer: Aluminium is getting oxidized in the given chemical reaction.

Step-by-step explanation:

Oxidation reaction is defined as the chemical reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.

`X\rightarrow X^(n+)+ne^-`

Reduction reaction is defined as the chemical reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.

`X^(n+)+ne^-\rightarrow X`

For the given chemical reaction:

`2Al(s)+3FeSO_4(aq.)\rightarrow Al_2(SO_4)_3(aq.)+3Fe(s)`

The half cell reactions for the above reaction follows:

Oxidation half reaction:
`Al\rightarrow Al^(3+)+3e^-`

Reduction half reaction:
`Fe^(2+)+2e^-\rightarrow Fe`

As, aluminium is loosing 3 electrons to form aluminium cation. Thus, it is getting oxidized. Iron is gaining 2 electrons to form iron anion. Thus, it is getting reduced.

Hence, the oxidized species of the given reaction is aluminium.