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 These are my first attempts: $\ce{H2O2 + 2e^- -> 2OH^-}$ (in alkaline conditions) $\ce{H2O2 + 2H^+ + 2e^- -> 2H2O}$ (in acidic conditions)
Does H2O2 break down into H2O - Chemistry Stack Exchange $\ce{H2O2}$ -> $\ce{H2O +1 2O2}$ This might make it easier to understand $\ce{H2O2}$ 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 $\ce{H2O2}$
How do I make 100 milliliters of 100mM H2O2 using 3% H2O2? Assume density 1 g ml for 3% solution which gives 0 03 g $\ce{H2O2}$ per ml, or 30 g $\ce{H2O2}$ per liter The molecular weight of $\ce{H2O2}$ is about 34 g mol so: $\dfrac{30}{34} \approx 1$ molar You want 100 mMolar which is 0 100 molar Thus you need a 10 fold dilution So add 10 ml of the 3% to 90 ml water to get 100 ml of solution
Why is oxygenated water not H2O2? - Chemistry Stack Exchange More precisely, the presence of H2O2 and other reactive oxygen species (ROS) have been cited in the literature as occurring in illuminated natural waters (see, for example, ‘Reactive Oxygen Species in Natural Waters ‘, by Neil V Blough and Richard G Zepp) To quote from an online two-page preview :
decomposition - Why and how does hydrogen peroxide decompose in the . . . $$\ce{O2^ - + H2O2 2HO^∙ + OH- + O2}$$ And as $\ce{H^+ + OH^- = H2O}$, the net product formation is not altered However, alkaline $\ce{H2O2}$ is well known to be less stable than acidic hydrogen peroxide (Ref 3) even in absence of light exposure, which accelerates its decomposition (which can involve radical pathways) liberating oxygen!
inorganic chemistry - What is the n factor of H2O2 undergoing . . . implying that n-factor of $\ce{H2O2}$ is 2 but I am calculating n-factor of $\ce{H2O2}$ as 1 because the definition of n-factor is "the no of electron gained or lost per mole" As we can see 2 electrons are participating in this reaction so electron exchanged per mole is 1 which is equal to n-factor
Why H2O2s molecular geometry is what it is. . . ? [duplicate] H2O2 looks like this when looked parallel to oxygen-oxygen bound:(source: Pubchem) Each hydrogen is in one of the three positions available around each oxygen(the two nonbonding electron pairs occupy the other two); even the oxygen-oxygen bound can rotate to set hydrogens in any position relative to each other
What is the rate equation of decomposition of H2O2 with catalysts? I would expect similar results with H2O2 for other transition metal oxides, but MnO2 is claimed to avoid a radical based path (per Wikipedia), and the decomposition reaction can be energetic (and possibly explosive with 30% H2O2 in a closed vessel) Here is another example at "Active sites and mechanisms for H2O2 decomposition over Pd catalysts