The given reaction is a redox reaction involving the transfer of electrons between barium (Ba) and zinc (Zn). Here's how to break it down into half-reactions:

1. Identify the Oxidation and Reduction:

* Oxidation: Zinc (Zn) loses electrons and its oxidation state increases from 0 to +2.

* Reduction: Barium (Ba) gains electrons and its oxidation state decreases from +2 to 0.

2. Write the Half-Reactions:

* Oxidation Half-Reaction:

Zn(s) → Zn²⁺(aq) + 2e⁻

* Reduction Half-Reaction:

Ba²⁺(aq) + 2e⁻ → Ba(s)

Explanation:

* Zn(s) → Zn²⁺(aq) + 2e⁻: Zinc in its solid state (Zn(s)) loses two electrons to become a zinc ion (Zn²⁺) in solution.

* Ba²⁺(aq) + 2e⁻ → Ba(s): Barium ion in solution (Ba²⁺) gains two electrons to become solid barium metal (Ba(s)).

Important Note: The sulfate ion (SO₄²⁻) is a spectator ion in this reaction. It does not participate in the electron transfer and is not included in the half-reactions.