http://www.bing.com:80/search?q=H2O2+KMnO4+MnO2+Koh+O2+H2OSearch resultshttp://www.bing.com:80/s/a/rsslogo.gifhttp://www.bing.com:80/search?q=H2O2+KMnO4+MnO2+Koh+O2+H2OCopyright © 2026 Microsoft. All rights reserved. These XML results may not be used, reproduced or transmitted in any manner or for any purpose other than rendering Bing results within an RSS aggregator for your personal, non-commercial use. Any other use of these results requires express written permission from Microsoft Corporation. By accessing this web page or using these results in any manner whatsoever, you agree to be bound by the foregoing restrictions.https://chemistry.stackexchange.com/questions/53533/why-is-h2o2-named-hydrogen-peroxideThe structure of $\ce {H2O2}$ is $\ce {H-O-O-H}$, and an $\ce {- O-O -}$ functional group is called a peroxide, by definition. The peroxide functional group is attached to a hydrogen atom, so it's called hydrogen peroxide.Wed, 08 Apr 2026 22:13:00 GMThttps://chemistry.stackexchange.com/questions/10375/half-equations-for-h2o2-for-its-reducing-and-oxidising-nature-in-acidic-and-alkaIs there a complete list of all the half equations for $\ce {H2O2}$ - both oxidation and reduction, in acidic and alkaline conditions? I've looked on the internet but can't seem to find a list with all of them.Mon, 06 Apr 2026 20:07:00 GMThttps://chemistry.stackexchange.com/questions/35869/does-h2o2-break-down-into-h2o-o-or-h2o-o2$\ce {H2O2}$ will homolytically cleave for form two $\ce {.OH}$ radicals. Radicals are very reactive and will start a chain reaction, but ultimately you will end up with water and oxygen products from $\ce {H2O2}$. (Why does it form two hydroxy radicals? because the O-O single bond is weak and unstable - see MO theory) How do we know this?Wed, 08 Apr 2026 09:42:00 GMThttps://chemistry.stackexchange.com/questions/171365/how-does-ki-catalyze-the-reaction-with-h2o2The equations $ (1)$ and $ (21)$ shows that $\ce {H2O2}$ can undergo spontaneous self-oxidation-reduction, and is therefore, thermodynamically unstable. Accordingly, $\ce {H2O2}$ decomposes spontaneously and exothermically, but slowly to oxygen and water at room temperature.Tue, 07 Apr 2026 10:26:00 GMThttps://chemistry.stackexchange.com/questions/7759/reaction-intermediates-of-mno2-catalyzed-h2o2-decomposition-reactionManganese dioxide catalyzes the decomposition of hydrogen peroxide to water and oxygen gas. But what are the intermediates in this catalyzed reaction?Wed, 08 Apr 2026 11:22:00 GMThttps://chemistry.stackexchange.com/questions/125517/what-is-the-rate-equation-of-decomposition-of-h2o2-with-catalystsThe decomposition of H2O2 is complex and has been the source of several studies. On iron oxide surface, here is a cited work `Catalytic Decomposition of Hydrogen Peroxide on Iron Oxide: Kinetics, Mechanism, and Implications’.Wed, 08 Apr 2026 19:36:00 GMThttps://chemistry.stackexchange.com/questions/146793/what-is-the-n-factor-of-h2o2-undergoing-disproportionation-reaction-liberating-o$$\ce {H2O2 + 2H+ + 2e → 2H2O}$$ Here 34.01 g of $\ce {H2O2}$ consumes two gram equivalents of hydrogen as an oxidizing agent. So the equivalent weight of this compound as an oxidizer in acidic medium is 34.01/2. The moral of the story is that normality is solely dependent on what reaction is being used!Tue, 07 Apr 2026 11:09:00 GMThttps://chemistry.stackexchange.com/questions/57130/the-effects-of-h2o2-hydrogen-peroxide-with-oils1 I have some 35% $\ce {H2O2}$ that I've been cutting down to 3% to create a product. Cheaper than buying pre cut solution from store. However, I've been thinking about trying to try it out with producing a new product which would induce mixing of the $\ce {H2O2}$ with pure oils and essential oils.Mon, 06 Apr 2026 08:33:00 GMThttps://chemistry.stackexchange.com/questions/116006/why-and-how-does-hydrogen-peroxide-decompose-in-the-presence-of-lightLike all other peroxides, hydrogen peroxide ($\ce {H2O2}$) also consists of a relatively weaker $\ce {O-O}$ bond, which is susceptible for light or heat. In the presence of light (the UV light from the sun catalyzes the reaction), $\ce {H2O2}$ spontaneously decomposes into water and oxygen.Mon, 06 Apr 2026 09:59:00 GMThttps://chemistry.stackexchange.com/questions/127385/what-is-the-mechanism-of-the-decomposition-of-hydrogen-peroxideBelow is one way to write it that shows what the enzyme does and avoids the uncertainty of the details: $$\ce {E + H2O2 -> E-O + H2O}\tag {1}$$ $$\ce {E-O + H2O2 -> E-O2 + H2O}\tag {2}$$ $$\ce {E-O2 -> E + O2}\tag {3}$$ In words, the enzyme binds to the first molecule of hydrogen peroxide, release one molecule of water and holds on to the other oxygen atom (via the iron bound to heme bound to ...Thu, 02 Apr 2026 05:03:00 GMT