Hydrogen Peroxide in the Thermal Hydrogen Oxygen Reaction I. Thermal Decomposition of Hydrogen Peroxide

Abstract

The decomposition of hydrogen peroxide (at partial pressures of one to two millimeters of mercury) was studied in the presence of one atmosphere of oxygen or nitrogen by the use of a flow system. The concentration of H2O2 was measured photometrically, using the continuous ultraviolet absorption of this compound. Determination by this means was more rapid, and offered less chance for errors of manipulation than conventional chemical analysis. A first order reaction with an activation energy of 40 kcal./mole was found in the neighborhood of 520°C. Evidence is presented to support the conclusion that the reaction is partly, at least, homogeneous in boric acid treated vessels at temperatures in the 470 to 540°C range.

Studies on hydrogen–oxygen systems in the electrical discharge. III. Surface effects

“…Pure hydrogen peroxide vapor was used for that purpose because dissociation of water requires very high temperatures. The pyrolysis of hydrogen peroxide has been studied before in a flow system (14) but not from the viewpoint of the trapped products. It is well known that the homogeneous decomposition becomes gradually more important above 400 "C (15).…”

The ionic liquid [Bmim][FeCl₄] catalyzes the formation of iron doped mesoporous silica aerogels for H₂O₂ decomposition

“…The control measurements done without the addition of one of the aerogels show a roughly linear increase of the oxygen concentration in the gas phase above the liquid. This is due to the well known decomposition of H 2 O 2 even without any catalyst being present [30]. The same experiment was then done with adding the catalyst to the solution after 6 min.…”

“…Hydrogen peroxide is thermodynamically unstable and decomposes to water and oxygen at room temperature [30]. Many transition metals catalyze the decomposition and especially Fe 2+ can lead to a decomposition pathway including radical species like HO .…”

Investigation of advanced NO oxidation process with the delivery of ·OH from thermal decomposition of H2O2

“…When the H 2 O 2 vapour was heated to $500 8C, the homogeneous decomposition reaction occurred and generated ÁOH radicals (Equation (2)). [24,[29][30][31] This observation of the NO oxidation can be explained by the fact that ÁOH reacts with NO via those reactions (Equation (3)-(6)). Meanwhile, NO also can be oxidized by gas-phase H 2 O 2 and HO 2 Á (Equation (7)- (9)).…”