H2O2 cannot oxidise - DASH

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Question

H₂O₂ cannot oxidise

$ PbS $

Na₂SO₃

O₃

$ KI $

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Understanding Oxidation and Reduction Oxidation and reduction, commonly referred to as redox reactions, involve the transfer of electrons between substances. An oxidizing agent gains electrons (is reduced), while a reducing agent loses electrons (is oxidized). Identifying the Role of Hydrogen Peroxide ($H_2O_2$) Hydrogen peroxide ($H_2O_2$) is a versatile chemical that can act both as an oxidizing agent and a reducing agent depending on the reaction context. As an oxidizing agent, it can accept electrons from substances that are stronger reducing agents. Analyzing the Given Options Let's evaluate each option to determine whether $H_2O_2$ can oxidize the substance: $PbS$ (Lead(II) sulfide): This compound can act as a reducing agent. $H_2O_2$ can oxidize $PbS$ by accepting electrons from it. Na$_2$SO$_3$ (Sodium sulfite): Sodium sulfite is a known reducing agent. $H_2O_2$ can oxidize Na$_2$SO$_3$ by taking electrons from it. O$_3$ (Ozone): Ozone is a strong oxidizing agent itself. It has a higher tendency to gain electrons compared to $H_2O_2$, making it resistant to further oxidation by $H_2O_2$. $KI$ (Potassium iodide): Potassium iodide acts as a reducing agent. $H_2O_2$ can oxidize $KI$ by accepting electrons from it. Determining the Correct Answer Among the options provided, $O_3$ stands out as a strong oxidizing agent. Since $O_3$ is already highly oxidized, $H_2O_2$ cannot further oxidize it. Therefore, $O_3$ is the substance that $H_2O_2$ cannot oxidize.

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