Study this chemical reaction: 2fe 3cl2 -> 2fecl3then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction.

Fe → Fe³⁺ + 3e⁻  Half reaction of oxidation

Cl₂ + 2e⁻ → 2Cl⁻  Half reaction of reduction

Explanation:

The main reaction is:

2Fe + 3Cl₂ → 2FeCl₃

Oxidation: The element increases the oxidation state

Fe changes from 0 to +3. It has released e⁻

Fe → Fe³⁺ + 3e⁻  Half reaction of oxidation

Reduction. The element decreases the oxidation state

Cl changes from 0 to -1. It has gained e⁻

Cl₂ + 2e⁻ → 2Cl⁻   (As chlorine is a dyatomic molecule we need a 2, to balance the chloride; at least the Cl gained to electrons) → Half reaction of reduction

One reaction releases 3 e⁻ and the other gains 2e⁻; therefore we have to multiply both reaction by 2 and 3, to balance the electrons to 6e⁻

(Fe → Fe³⁺ + 3e⁻  ) . 2

(Cl₂ + 2e⁻ → 2Cl⁻ ) . 3    and we sum both

2Fe + 3Cl₂ + 6e⁻ → 2Fe³⁺ + 6e⁻ + 6Cl⁻

So we cancel the electrons and we reach the balance reaction:

2Fe + 3Cl₂ → 2FeCl₃