Catalytic decomposition sodium oxide

Chirnoga, E. (1926) The catalytic decomposition of sodium hypochlorite by finely divided metallic oxides. Journal of the Chemical Society, 1693-1703. 

A peroxide, probably Ag203, is stated to be produced by anodic oxidation of silver in acid solution.4 When solutions of sodium or potassium persulphate react with silver or silver nitrate, a peroxide with a higher percentage of oxygen than Ag2Oa is produced, the process being attended by catalytic decomposition of the persulphate with formation of the acid sulphate. Ammonium persulphate does not yield a peroxide, but the ammonium radical becomes oxidized to nitric acid.6... 

Specihcally with regard to the pyrolysis of plastics, new patents have been filed recently containing variable degrees of process description and equipment detail. For example, a process is described for the microwave pyrolysis of polymers to their constituent monomers with particular emphasis on the decomposition of poly (methylmethacrylate) (PMMA). A comprehensive list is presented of possible microwave-absorbents, including carbon black, silicon carbide, ferrites, barium titanate and sodium oxide. Furthermore, detailed descriptions of apparatus to perform the process at different scales are presented [120]. Similarly, Patent US 6,184,427 presents a process for the microwave cracking of plastics with detailed descriptions of equipment. However, as with some earlier patents, this document claims that the process is initiated by the direct action of microwaves initiating free-radical reactions on the surface of catalysts or sensitizers (i.e. microwave-absorbents) [121]. Even though the catalytic pyrolysis of plastics does involve free-radical chain reaction on the surface of catalysts, it is unlikely that the microwaves on their own are responsible for their initiation. 

Noller et a/. 23-725,767,900,952 continued their investigations on the catalytic decomposition of chlorinated and brominated hydrocarbons on Ba, Ca, Mg, A1 oxides and salts studies on these and related surfaces have reported by other workers - - - - - . Decomposition of chlorinated methanes on titanium , on sodium , and on other metal surfaces have been reported by Anderson et al. similar studies on 2-bromobutane with nickel and platinum surfaces have been made by Burwell et Nutt and Carter carried out a molecular beam study of the decomposition of methyl iodide on a hot tungsten filament. 

The kinetics of the catalytic decomposition of formic acid on sodium tungsten bronzes Naj,W03, with x in the range 0.11—0.85, and on tungstic oxide have been investigated manometrically in a static system at 150— 250 °C with acid pressures of 25—30 Torr. The decomposition products were CO2, CO, H2O, and Hg, the mole ratios C02 CO and H2 C02 being determined mass-spectrometrically. 

Peroxodisulfates (persulfates) are the best peroxidic oxidants for EDOT to form conducfive FEDOT complexes. The overall chemical equation can be written as follows with the example of polystyrenesulfonic acid as the counterion (Figure 6.3, depicted for the hexamer for simplification). Other peroxodisulfates than the sodium salt are also sufficient, like ammonium or potassium peroxodisulfate. Small amounts of mefal salfs of Fe(II) or Fe(III), for example Fe2(S04)3, musf be added to fhe reaction mixture. They provide the catalytic decomposition of peroxodisulfafe at defined reaction rates and so are pivotal for a high and reproducible conductivity of the PEDOTPSS complex formed. A detailed description of the PEDOTPSS complex and its synthetic parameters will follow in Chapter 9. 

A method based on the catalytic decomposition of hypobromite has been described by Anbar and Guttmann (1959) in which quantities of water as small as 25 mg. can be analyzed. A small pellet of clean sodium (10-20 mg.) is added to the sample of water to be analyzed (usually 50-1000 mg.) in a standard sealed tube (Fig. 4a) in which a small quantity of cobaltic oxide (1-3 mg.) is placed. The tube is fitted to a vacuum line, frozen in liquid nitrogen, pumped off, allowed to heat up in order to degas it, refrozen, and pumped off again. A small quantity of bromine (about 20 mg.) is distilled in and the tube sealed off and allowed to warm up to room temperature. The hypobromite... 

Basic oxides of metals such as Co, Mn, Fe, and Cu catalyze the decomposition of chlorate by lowering the decomposition temperature. Consequendy, less fuel is needed and the reaction continues at a lower temperature. Cobalt metal, which forms the basic oxide in situ, lowers the decomposition of pure sodium chlorate from 478 to 280°C while serving as fuel (6,7). Composition of a cobalt-fueled system, compared with an iron-fueled system, is 90 wt % NaClO, 4 wt % Co, and 6 wt % glass fiber vs 86% NaClO, 4% Fe, 6% glass fiber, and 4% BaO. Initiation of the former is at 270°C, compared to 370°C for the iron-fueled candle. Cobalt hydroxide produces a more pronounced lowering of the decomposition temperature than the metal alone, although the water produced by decomposition of the hydroxide to form the oxide is thought to increase chlorine contaminate levels. Alkaline earths and transition-metal ferrates also have catalytic activity and improve chlorine retention (8). 

Sodium chromate is produced as part of the process for obtaining Cr203, and it is probably the most important chromium compound. Although there are other oxides of chromium, Cr203 is very important because of its catalytic properties. One way to obtain this oxide is by the decomposition of ammonium dichromate,... 

Effect of sodium and aluminum on TS-1. The catalytic activities of aluminum and/or sodium containing TS-1 are depicted in Table IV. The data show that the addition of aluminum during the synthesis of TS-1 yields a material (TAS-1(D)) that has a lower conversion of n-octane oxidation and a smaller IR peak ratio. The existence of the acid sites due to the incorporation of aluminum into the framework of TS-1 may accelerate the decomposition of H2O2 to water and oxygen during the reaction. However, reducing the number of acid sites by exchanging with sodium ions only increases the conversion by 1% (Na/TAS-1(D)). Therefore, the addition of aluminum into the synthesis mixture most likely reduce the amount of titanium present in the sample. 

L. Pasteur, J. Tyndall, E. T. Chapman, P. Miquel, W. Spring, F. Schulz, etc. Air may be freed from dust particles, etc., in suspension by filtration through biscuit earthenware, asbestos, or cotton wool. When a beam of sunlight is passed through unfiltered air, it reveals a multitude of motes constantly in motion. Lucretius, in his Be natura remm (2.113, 60 b.c.), has given a very vivid description of the phenomenon. With filtered air, there is no such eflect, and J. Tyndall said that such air is optically empty. F. O. Rice showed that in a number of reactions— e.g. the oxidation of soln. of sodium arsenite or sulphite, the decomposition of hydrogen dioxide, etc.—the suspended dust in air acts as a catalytic agent. 

Other metals, the commonest being lead,2 bismuth, and manganese, in powder form exert a more moderate effect on the decomposition. Mercury would also fall into this class of moderate accelerators, but the catalytic action in this case is remarkable in being periodic or rhythmic. When the concentration of hydrogen ion is reduced to an almost negligible quantity by the addition of a little sodium acetate solution, a clean mercury surface in contact with hydrogen peroxide solution of approximately 10 per cent, concentration, at periodic intervals of about one second, becomes coated with a bronze film which suddenly disappears with a burst of oxygen from the contact layer of the two liquids the substance of the film, which is alternately formed and decomposed, is probably an unstable oxide, possibly mercurous peroxide.3... 

Thiosulfate solutions are generally prepared from sodium thiosulfate penta-hydrate, NajSjOa SHjO, which under ordinary conditions is not a primary standard. The solutions should be prepared from water free of heavy-metal impurities to avoid catalytic air oxidation. Ordinary air oxidation is negligible in rate and proceeds through the slow decomposition of thiosulfate to sulfite, which is rapidly air-oxidized to sulfate. Catalyzed air oxidation, on the other hand, proceeds through the reduction of metals such as copper(II) or iron(III), present as thiosulfate complexes, followed by air oxidation of the lower oxidation state ... 

---