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H2O2 can act as both an oxidizing and reducing agent.

Oxidizing agent:
- An oxidizing agent is a substance that accepts electrons from another substance during a chemical reaction.
- In the case of H2O2, it can donate one or both of its oxygen atoms to another substance, thereby accepting electrons and becoming reduced itself.
- For example, when H2O2 reacts with sulfur dioxide (SO2), it oxidizes SO2 to sulfuric acid (H2SO4) while itself getting reduced to water (H2O).
H2O2 + SO2 → H2SO4 + H2O

Reducing agent:
- A reducing agent is a substance that donates electrons to another substance during a chemical reaction.
- H2O2 can also act as a reducing agent in certain reactions.
- For example, when H2O2 reacts with potassium permanganate (KMnO4), it donates electrons to Mn(VII) in KMnO4, reducing it to Mn(II) while itself getting oxidized to water (H2O).
H2O2 + KMnO4 → MnO2 + O2 + H2O

Explanation:
- The ability of H2O2 to act as both an oxidizing and reducing agent is due to the presence of the peroxide (O-O) bond in its structure.
- The peroxide bond is relatively weak and can be broken, allowing H2O2 to release oxygen atoms that can accept electrons, acting as an oxidizing agent.
- At the same time, the oxygen atoms in the peroxide bond can also donate electrons, acting as a reducing agent.
- The ability of H2O2 to act as both an oxidizing and reducing agent makes it a versatile compound in various chemical reactions.
- It can participate in redox reactions where it transfers electrons to or accepts electrons from other substances.
- The exact role of H2O2 in a specific reaction depends on the nature of the reactants and the reaction conditions.