Decomposition of Hydrogen peroxide by Potassium permanganate

[iskatelikeanoob]

what about 3% H2O2

[ekojk1242]

Ok now I know I might be asking a stupid question but, when will we use this information in our lives?

[alinan90]

We used Potassium Iodine (KI) and placed it in a closed beaker. The stopper had pressure sensor attached and that way you can measure how much O2 was released.

[kENNYko0i]

thank you, now i can finish my homework ;D

[DCJellybean]

is there a way of measuring the amount of gas given off?

if so how and is it safe for a classroom experment?

[roboticmehdi]

is there any catalyst which is not powder but rather a solid? i mean something like silver metal but not as expensive as silver. it must be solid so that the surface area remains same?? thanks...

[lambogeek]

we used mnO2 in school for catalyst

[arnrgrerlrors]

you did a mistake...the number of the oxygens is not right....test it again....:)

[Cforchemistry]

The equation is not balanced.

[PlayLikePros]

@arnrgrerlrors

2KMnO4 + 2H2O2 ==> K2O2 + 2MnO2 + 2H2O + 2O2

thats the balanced one

[coolliger]

Can I dispose of the manganese IV by adding water to make a solution, adding sodium carbonate, and filtering it off and throwing it out.

[Cforchemistry]

you can dispose by adding acid, makeing Mn2+ solution.

[coolliger]

@Cforchemistry

will any acid do?

[Cforchemistry]

i would say yes vinegar will do

[EmeraldxFairy]

Great vid! 5*

[solojam]

it sounded like the pop happend before they came in contact!

[Hydroxybenzeen]

Thanks I did not know that,

I tried the experiment myself using 8% solution. Afther the reaction the remaining liquid had a brownisch collor, indicating MnO2 had formed.

[Hydroxybenzeen]

The H2O2 is not oxidised by the potassium permanganate, the KMnO4 only acts as a cathalyst.

[Cforchemistry]

KMnO4 did react to form MnO2, and MnO2 is the catalyst.

[Kripo21]

What a mess. :D

[jellybeanlive]

very interesting... i shall investigate further.. thx

[bla287]

Aahh, the first time I see a video of that reaction where the uploader actually realizes that H2O2 works as a reducing agent in that case ;)

[Cforchemistry]

H2O2 is actually dispoprtioned to H2O and O2 is this case, proved that KMnO4 are really strong!

[bla287]

Well, isn't the disproportionation first happening then when there's MnO2? Because the KMnO4 somehow has to go down from +7 to +4, and thus needing a reducing agent?

[bla287]

What I meant to say first is that I read lots of comments on other vids where people clkaim that the H2O2 "oxidizes" the KMnO4 which is impossible

[Cforchemistry]

I do real science, so I should deliver correct information to all curious in it.Thanks for your comments and if you see anything wrong from my video, please let me know.

[Cforchemistry]

Actually starts when in contact with KMnO4, but reaction with KMnO4 is complex, so hard to investigate...

[bla287]

No, there's nothing wrong with your vid ;) I just thought the initial reaction (when there's no MnO2 yet) would be something like this:

Reduction:

MnO4(-) + 2 H2O + 3 e(-) → MnO2 + 4 OH(-); E° = +1.7V

Oxidation:

H2O2 → O2 + 2 H(+) + 2 e(-)

E° = +0.7V

So from the potentials, this should be possible. Of course, later on as there is more MnO2 present, another more complicated reaction occurs where the MnO2 just catalyzes the dismutation of H2O2 to H2O and O2, correct me if I'm wrong.

[Cforchemistry]

Nice to meet such an enthusiastic chemist like you, I hope we can still have such constructive discussion in the future!

[bla287]

Thanks ;)

[DF110018]

Nice video! Nice chemistry experiment!

[Cforchemistry]

Thanks

[dbc616]

That's instant!!!

[Cforchemistry]

85% Hydrogen peroxide reacts in a much more vigorous manner, but I dare not to try it.