Consider    ClO3−(aq) + 5 Cl−(aq) + 6 H+(aq) ⟶ 3 Cl2(g) + 3 H2O(l) determine if each of the following statements is True or False.   ?

1) False
Cl₂ is a product. We can classify the reactants of a redox reaction to be an oxidizing agent or a reducing agent, but not the products.

2) True
2ClO₃⁻(aq) + 12H⁺(aq) + 10e⁻ → Cl₂(g) + 6H₂O(ℓ)


3) True
2Cl⁻(aq) → Cl₂(g) + 2e⁻
Cl⁻ is oxidized because its oxidation number increases from -1 to 0.
Hence, it is a reducing agent.

4) False
The oxidation number of H in H⁺ = +1
The oxidation number of H in H₂O = +1
The oxidation number of H is unchanged in the reaction. Hence, H⁺ is neither reduced nor oxidized.