Hydrogen peroxide can act as either an oxidizing agent or a reducing agent, depe

Question

Hydrogen peroxide can act as either an oxidizing agent or a reducing agent, depending on the species present in solution. Write balanced half-reaction equations for each of the following:

(a) H2O2(aq) acting as an oxidizing agent in an acidic solution. Write the balanced half-reaction equation. Phases are optional.

(b) H2O2(aq) acting as a reducing agent in an acidic solution. Write the balanced half-reaction equation. Phases are optional.

(c) 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.

Explanation / Answer

An oxidizing agent is itself being reduced. gain of e- is reduction.
H2O2 + 2H+ + 2e- --> 2H2O

Reducing agent
2H2O2 + e- --> 2H2O + 2OH- This is probably not correct

Disproportionation
H2O2 + H2O2 --> 2H2O + O2

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