Consider the following balanced redox reaction (do not include state of matter in your answers) : 2CrO2 - (aq) + 2H2O (l) + 6ClO - (aq) rightarrow 2CrO42 - (aq) + 3Cl2 (g) + 4OH - (aq) Which species is being oxidized? Which species is being reduced? Which species is the oxidizing agent?

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⁻.