Decomposition of Hydrogen Peroxide by Potassium Permanganate


Introduction: Decomposition of Hydrogen Peroxide by Potassium Permanganate

It is a reaction between 50% Hydrogen peroxide (H2O2) and Potassium permanganate (KMnO4) . It is a very vigorous reaction which steam (H2O) and Oxygen (O2) are the desired products, side products include Manganese(IV) oxide (MnO2) and trace amount of Potassium compound.

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    13 Discussions

    Well, i guess KMnO4 acts as an catalyst to increase the reaction rate of H2O2 becoming H2O and O2, while it breaks up to K2MnO4, MnO2, and O2 due to the heat produced. Is it right?

    hai, Im amer faiz

    Im planning to make a chemical can you suggest a small container(material) to react h202 and kmno4.

    Referring back to Chemistrystudent, I hope this can help
    as I learned: the chemical reaction for this is 2H2+O2 -> Catalyst potassium permanganate -> 2H20

    Firstly, Hydrogen peroxide is partly oxdized to Oxygen, and the other part is reduced to Water, it is so called a Disproportionation reaction. Secondly, there are Two reaction in the process actually, one is reaction between KMnO4 and H2O2, which non-catalytic decomposition. Another reaction is H2O2 react with MnO2 which produced in the reaction of KMnO4, and this is the catalytic decomposition. And the reason I didn't balance the equation is simple, the equation have many solution, which means the most probably reaction is related to energetics and some other variable, so this equation cannot be balanced by simple maths.

    6 replies

    Hi! I'm doing a project on the effect of pH on the oxidizing power of permanganate ions on hydrogen peroxide, My pH range is 0-7. (For pH 0-3 I used Hcl and pH 4-7 I prepared buffer solutions) and I'm comparing their initial rates (The rate at which oxygen is formed) and I found ou that the initial rate of reaction increased from pH 0-3 and it decreased from pH 4-7 but I couldn't find any theoretical evidence to support my findings,, I was wondering if you could help me with some sources?

    Thank you in advance.


    When you reply to comments use the REPLY button (like I have), in this way the person get's a notification (as you should have received one for this).
    It would be better described as disproportionation, and you appreciate what I mean by there being little use in posting an equation (potassium superoxide?)

    Have you tried a drop of blood into peroxide?


    Firstly, you are right that disproportionation are more appropriate, but I just focus on the product Oxygen which peroxide oxidized to, so I mention only the oxidation, sorry for that mistake. And about the equation, potassium superoxide does formed in this reaction, but in a instant only, it worth me to mention because this specie is rare.

    I know catalyse in bloob act as a bio-catalyst, however, I am not well-experienced in Biology, so I didn't try to film it. I tried once when I am in High school, but not for now.

    I can imagine what will happen, probably an uncontrollable rocket or a explosion, thanks for you suggestion, but I don't think I can manage to film this...

    Only in a test tube: very dangerous!!

    Fix a test tube on The other side of a pole. Fill it with about 1/3 full of H2O2 30%.

    Put another 1/3 of gasoline in it, it will float. Light it: it will burn with a small flame on top of the test tube.

    Drop a tiny amount of crushed potassium permanganate crystals in the tube. Make sure you stay on the opposite side of the pole!!!

    Prepare for an 80 % hearing loss for the next few days....

    In what way is hydrogen peroxide oxidsed?
    As you're using manganate as a catalyst it's somewhat meaningless to add a dubious unbalanced equation.
    I'd wear thicker gloves than that & tip a bit of catalyst into the liquid(?)