why H2O2 act as both oxidising agent or reducing agent.give reason.
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I think because it is unstable and does not have valence configuration
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When someting acts as an oxidising agent is gains electrons (removing them from the oxidised species). This can be shown by the relevant half-equations:
H2O2 + 2e –> 2OH–
or in the presence of acid:
H2O2 + 2H+ + 2e –> 2H2O
H2O2 + 2e –> 2OH–
or in the presence of acid:
H2O2 + 2H+ + 2e –> 2H2O
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