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Hydrogen peroxide can act as either an oxidizing agent or a reducing agent depending on the species present in solution. Write the balanced half-reaction equations for each situation. Write the balanced half-reaction equation for when H2O2(aq) acts as an oxidizing agent in an acidic solution. Phases are optional. half-reaction equation: Write the balanced half-reaction equation for when H2O2(aq) acts as a reducing agent in an acidic solution. Phases are optional. half-reaction equation: A disproportionation reaction is one in which a single species oxidizes and reduces itself. Write the complete balanced equation for the disproportionation reaction of H2O2(aq) . Phases are optional. disproportionation reaction:

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Answer:

1) H₂O₂ + 2H⁺ + 2e⁻ → 2H₂O

2) H₂O₂ → 2H⁺ + 2e⁻  O₂

3) 2H₂O₂ → 2H₂O + O₂

Explanation:

Half-reaction equation for when H₂O₂(aq) acts as an oxidizing agent in an acidic solution (this means H₂O₂ is reduced):

  • H₂O₂ + 2H⁺ + 2e⁻ → 2H₂O

It is a reduction because the oxidation number of O changes from -1 to -2.

Half-reaction equation for when H₂O₂(aq) acts as a reducing agent in an acidic solution (this means H₂O₂ is oxidized):

H₂O₂ → 2H⁺ + 2e⁻  O₂

It is an oxidation because the oxidation number of O changes from -1 to 0.

Disproportionation reaction of H₂O₂(aq):

2H₂O₂ → 2H₂O + O₂

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