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I saw a reaction by chemicalforce on YouTube where he decomposed $\ce{H2O2}$ into $\ce{H2O}$ and $\ce{O2}$ using potassium permanganate. The permanganate is a catalyst in the reaction.

I am wondering if this decomposition occurs because the initial $\ce{H2O2}$ decomposition reacts with the $\ce{KMnO4}$ and reproduces $\ce{H2O2}$ which then again decomposes?

How is the permanganate a catalyst?

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Potassium permanganate is involved in two ways.

It oxidizes hydrogen peroxide to oxygen:

$$\ce{2 MnO4- + 3 H2O2 -> 2 MnO2 + 2 OH- + 3 O2 + 2 H2O}$$

The formed $\ce{MnO2}$ acts as the catalyst of reaction:

$$\ce{2 H2O2 ->[MnO2] 2 H2O + O2}$$

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  • $\begingroup$ Hello Poutnik! Is it a mistake to call the first reaction a disproportionation? The oxidation state of oxygen goes down (to $-2$ in $\ce{H2O}$) and goes up (to $0$ in $\ce{O2}$). Or calling it a redox reaction is more accurate in this case? $\endgroup$
    – Metal Storm
    Commented Jan 11 at 21:04
  • $\begingroup$ You would not need permanganate for it. $\endgroup$
    – Poutnik
    Commented Jan 11 at 21:33

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