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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?
  • 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!
  • Potassium permanganate and hydrogen peroxide decomposition
    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?
  • 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
  • physical chemistry - Disproportionation of hydrogen peroxide . . .
    However, if you just keep H2O2 by itself, without any oxygen, it will still decompose This isn't captured by your proposed pair of half-equations, which essentially says that you need oxygen gas for the total reaction (i e sum of 2 half-reactions) to proceed
  • acid base - When does hydrogen peroxide act as a reducing and when as . . .
    In basic medium: $\ce {H2O2 + 2e- -> 2OH-}$ I was unable to find any pattern in all of the reactions I studied above (except for potassium ferrocyanide, for which the medium triggers the electron addition removal) to recognize when hydrogen peroxide behaves as an oxidising agent and when it behaves as a reducing agent
  • 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
  • Hydrogen peroxide and potassium iodide reactions
    2 What is the explanation for the two possible reactions of $\ce {H2O2}$ with $\ce {KI}$ in acid media (iodide-catalyzed decomposition of hydrogen peroxide or iodide oxidation by hydrogen peroxide) and what determines the prevalence of one over the other?





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