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Hydrogen peroxide is a chemical compound with the formula H 2 O 2.In its pure form, it is a very pale blue [5] liquid that is slightly more viscous than water.It is used as an oxidizer, bleaching agent, and antiseptic, usually as a dilute solution (3%–6% by weight) in water for consumer use and in higher concentrations for industrial use.
Latimer diagrams can be used in the construction of Frost diagrams, as a concise summary of the standard electrode potentials relative to the element.Since Δ r G o = -nFE o, the electrode potential is a representation of the Gibbs energy change for the given reduction.
Common oxidizing agents are oxygen, hydrogen peroxide, and the halogens. In one sense, an oxidizing agent is a chemical species that undergoes a chemical reaction in which it gains one or more electrons. In that sense, it is one component in an oxidation–reduction (redox) reaction. In the second sense, an oxidizing agent is a chemical species ...
In aqueous solutions, redox potential is a measure of the tendency of the solution to either gain or lose electrons in a reaction. A solution with a higher (more positive) reduction potential than some other molecule will have a tendency to gain electrons from this molecule (i.e. to be reduced by oxidizing this other molecule) and a solution with a lower (more negative) reduction potential ...
The reaction, using H 2 O 2 for the formation of ·OH, is carried out in an acidic medium (2.5-4.5 pH) [9] and a low temperature (30 °C - 50 °C), [10] in a safe and efficient way, using optimized catalyst and hydrogen peroxide formulations.
The first stage of Fenton's reaction (oxidation of Fe 3+ with hydrogen peroxide) is used in Haber–Weiss reaction; Fenton's reagent can be used in organic synthesis reactions: e.g. hydroxylation of arenes via a free radical substitution; Conversion of benzene into phenol by using Fenton's reagent; Oxidation of barbituric acid into alloxan.
Many industrial peroxides are produced using hydrogen peroxide. Reactions with aldehydes and ketones yield a series of compounds depending on conditions. Specific reactions include addition of hydrogen peroxide across the C=O double bond: R 2 C=O + H 2 O 2 → R 2 C(OH)OOH. In some cases, these hydroperoxides convert to give cyclic diperoxides:
In chemistry, the oxygen reduction reaction refers to the reduction half reaction whereby O 2 is reduced to water or hydrogen peroxide. In fuel cells, the reduction to water is preferred because the current is higher. The oxygen reduction reaction is well demonstrated and highly efficient in nature. [1] [2]