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18 October, 07:09

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?

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  1. 18 October, 08:22
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    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⁻.
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