Question

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?

Answer 1

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⁻.