Sulfur smoke

Hazardous decomp, prods. Linder combustion hydrogen sulfide, oxides of carbon and sulfur, smoke, fames HMIS Health 2, Flammability 1, Reactivity 0 Storage Keep container closed Polymox PPI-RC [AIzo]... 

Hydrotreating processes are applied to finished products to improve their characteristics sulfur content, cetane number, smoke point and the aromatics and olefins contents. 

Precipitators are currently used for high collection efficiency on fine particles. The use of electric discharge to suppress smoke was suggested in 1828. The principle was rediscovered in 1850, and independently in 1886 and attempts were made to apply it commercially at the Dee Bank Lead Works in Great Britain. The installation was not considered a success, probably because of the cmde electrostatic generators of the day. No further developments occurred until 1906 when Frederick Gardiner Cottrell at the University of California revived interest (U.S. Pat. 895,729) in 1908. The first practical demonstration of a Cottrell precipitator occurred in a contact sulfuric acid plant at the Du Pont Hercules Works, Pinole, California, about 1907. A second installation was made at Vallejo Junction, California, for the Selby Smelting and Lead Company. 

The products manufactured are predominantiy paraffinic, free from sulfur, nitrogen, and other impurities, and have excellent combustion properties. The very high cetane number and smoke point indicate clean-burning hydrocarbon Hquids having reduced harmful exhaust emissions. SMDS has also been proposed to produce chemical intermediates, paraffinic solvents, and extra high viscosity index (XHVI) lubeoils (see Lubrication and lubricants) (44). 

Recipe, in parts by wt smoked sheets, 100.00 zinc oxide, 5.00 filler, as indicated nondiscoloring antioxidant, 1.00 MBTS, 1.00 TMTD, 0.10 sulfur, 2.75 stearic acid, 3.00. 

A solution of sulfur trioxide [7446-11-9] dissolved in chlorosulfonic acid [7990-94-5] CISO H, has been used as a smoke (U.S. designation FS) but it is not a U.S. standard agent (see Chlorosulfuric acid Sulfuric acid and sulfur trioxide). When FS is atomized in air, the sulfur trioxide evaporates from the small droplets and reacts with atmospheric moisture to form sulfuric acid vapor. This vapor condenses into minute droplets that form a dense white cloud. FS produces its effect almost instantaneously upon mechanical atomization into the atmosphere, except at very low temperatures. At such temperatures, the small amount of moisture normally present in the atmosphere, requires that FS be thermally generated with the addition of steam to be effective. FS can be used as a fill for artillery and mortar shells and bombs and can be effectively dispersed from low performance aircraft spray tanks. FS is both corrosive and toxic in the presence of moisture, which imposes limitations on its storage, handling, and use. 

Chlorosulfuric acid is miscible with sulfur trioxide, sulfuric acid, and pyrosulfuryl chloride in all proportions. Mixtures with sulfur trioxide are used as smoke-forming agents. The properties of such mixtures have been described (3,15,16). Mixtures of chlorosulfuric acid and pyrosulfuryl chloride form an a2eotrope when distilled (17). 

Coal drying rotary, screen, suspension. Dust, smoke, particulates, sulfur oxides. Exhaust systems with cyclones and... 

Products of Combustion Heat, hght, smoke, and asphyxiating and toxic gases are produced by fire. In a hot, well-ventilated fire, combustion is usually nearly complete. Nearly all the carbon is converted to carbon dioxide, all the hydrogen to steam, and oxides of various other elements such as sulfur and nitrogen are produced. 

The problems with the combustion reaction occur because the process also produces many other products, most of which are termed air pollutants. These can be carbon monoxide, carbon dioxide, oxides of sulfur, oxides of nitrogen, smoke, fly ash, metals, metal oxides, metal salts, aldehydes, ketones, acids, polynuclear hydrocarbons, and many others. Only in the past few decades have combustion engineers become concerned about... 

Smoke concentrations ranged from 0.3 to more than 4 mg m . Daily means of the sampling stations are shown in Fig. 18-4. Sulfur dioxide measurements ranged from less than 0.1 ppm (260 /rg m ) to 1.34 ppm (3484 /Ag m" ). Also, 4 of the 11 stahons had at least one daily value in excess of 1 ppm, and 9 of the 11 stations had at least one daily value in excess... 

From the commencement of the fog and low visibility, many people experienced difficulty breathing, the effects occurring more or less simultaneously over a large area of hundreds of square kilometers. The rise in the number of deaths (Fig. 18-4) paralleled the mean daily smoke and sulfur dioxide concentrations daily deaths reached a peak on December 8 and 9, with many of them related to respiratory troubles. Although the deaths decreased when the concentrations decreased, the deaths per day remained considerably above the pre-episode level for some days. Would most of the persons who died have died soon afterward anyway If this were the case, a below-normal death rate would h ve occurred following the episode. This situation did not seem to exist, but detailed analysis was complicated by increased deaths in January and February 1953 which were attributed primarily to an influenza outbreak. 

An air pollution episode responsible for approximately 300 excess deaths occurred in London between November 26 and December 1, 1948. Concentrations of smoke and sulfur dioxide were 50-70% of the values during the 1952 episode. 

Compounds that induce bronchoconstriction include tobacco smoke, formaldehyde, and diethyl ether. Several other compounds, such as acidic fumes (e.g., sulfuric acid) and gases, such as ozone and nitrogen dioxide, as well as isocyanates, can cause bronchoconstriction. Also, cellular damage in the airways induces bronchoconstriction because of the release of vasoactive compounds. Frequently, different mechanisms work at the same time, provoking bronchoconstriction and increased secretion of mucus, both of which interfere with respiration. 

Two other principles that have been made commercially available are (11 rhe reaction between pyrosulfuric acid (H2S2O7) and water (water vapor in air) to form sulfuric acid aerosol and (2) rhe reaction between ritaiJium tetrachloride (TiCl4) and water to form titanium dioxide (TiO,) and hydrogen chloride il Id), higure 12.5 shows two different hand-held, disposable smoke emitters. 

The earliest information dealing with this phenomenon dates back to 600 B.c. It was found that a piece of amber after it had been rubbed was able to attract small fibers. More recent observations are from the 17th century, when William Gilbert noticed that amber, sulfur, and other dielectrics charged by friction could attract smoke. Similar observations were made by Boyle (1675) and Otto von Guericke (1672). Francis Hauksbee (1709) reported that he had discovered a phenomenon which is now called ionic wind or electric wind. Ionic wind and the glow from the corona discharge was discussed by Isaac Newton (1718). 

Si, and stannic tetrachloride. An effective smoke agent, whether it be mechanically dispersed from an aircraft spray tank or vaporized thermally, is a mixt of S trioxide and chlorosulfonic acid (FS smoke agent) which upon hydrolysis forms sulfuric and hydrochloric acid dispersions. Of course, all such formulations are highly corrosive, and, if not outright toxic, then conducive to pulmonary edema... 

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