Answer:
CrO₂⁻
ClO⁻
ClO⁻
Explanation:
Let's consider the following redox reaction.
2 CrO₂⁻(aq) + 2 H₂O(l) + 6 ClO⁻(aq) → 2 CrO₄²⁻(aq) + 3 Cl₂(g) + 4 OH⁻(aq)
We can identify both half-reactions.
Reduction: 6 H₂O(l) + 6 ClO⁻(aq) + 6 e⁻ → 3 Cl₂(g) + 12 OH⁻(aq)
Oxidation: 8 OH⁻(aq) + 2 CrO₂⁻(aq) → 2 CrO₄²⁻(aq) + 4 H₂O(l) + 6 e⁻
Which species is being oxidized?
CrO₂⁻ is being oxidized. Its oxidation number increases from +3 to +6.
Which species is being reduced?
ClO⁻ is being reduced. Its oxidation number decreases from +1 to 0.
Which species is the oxidizing agent?
The species being reduced is the oxidizing agent, that is, ClO⁻.
