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  • redox - Half equations for H2O2 for its reducing and oxidising nature . . .
    Is 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
  • Does H2O2 break down into H2O - Chemistry Stack Exchange
    $\ce {H2O2}$ 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?
  • How does KI catalyze the reaction with H2O2? - Chemistry Stack Exchange
    The 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
  • inorganic chemistry - Reaction intermediates of MnO2 catalyzed H2O2 . . .
    Manganese dioxide catalyzes the decomposition of hydrogen peroxide to water and oxygen gas But what are the intermediates in this catalyzed reaction?
  • What is the rate equation of decomposition of H2O2 with catalysts?
    The 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’
  • inorganic chemistry - What is the n factor of H2O2 undergoing . . .
    $$\ce {H2O2 + 2H+ + 2e → 2H2O}$$ 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!
  • The effects of H2o2 (hydrogen peroxide) with oils
    1 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
  • decomposition - Why and how does hydrogen peroxide decompose in the . . .
    Like 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
  • catalysis - What is the mechanism of the decomposition of hydrogen . . .
    Below 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





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