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COLLOIDAL SULFUR

Sulfur, molten appears as a pale yellow crystalline solid with a faint odor of rotten eggs. Insoluble in water. A fire and explosion risk above 450° F. Transported as a yellow to red liquid. Handled at elevated temperature (typically 290°F) to prevent solidification and makes transfers easier. Hot enough that plastic or rubber may melt or lose strength. Causes thermal burns to skin on contact. Cools rapidly and solidifies if released. Equipment designed to protect against ordinary chemical exposure is ineffective against the thermal hazard. Exercise caution walking on the surface of a spill to avoid breakthrough into pockets of molten sulfur below the crust. Do not attempt to remove sulfur impregnated clothing because of the danger of tearing flesh if a burn has resulted. May be irritatin to skin, eyes and mucous membranes. Used in sulfuric acid production, petroleum refining, and pulp and paper manufacturing.

CAS NUMBER:7704-34-9
EC NUMBER:231-722-6

SYNONYMS:
231-722-6; 7704-34-9; 9035-99-8; Agri-Sul; AN-Sulfur Colloid Kit; Aquilite; Asulfa-Supra; Atomic sulfur; Bensulfoid; Brimstone; Colloidal sulfur; Colloidal-S; Devisulphur; elemental sulfur; Flour sulfur; Flour sulphur; Flowers of sulfur; Flowers of sulphur; Gofrativ; Ground vocle sulfur; Ground vocle sulphur; Precipitated sulfur; S; Sofril; Solfa; Soufre; Soufre [ISO-French]; Sperlox-S; Spersul; Spersul thiovit; Sublimed sulfur; Sublimed sulphur; Suffa; Sufran; Sufran D; Sulfex; Sulfidal; Sulforon; Sulfospor; Sulfur; sulfur (0); Sulfur (JP17); Sulfur (molten); Sulfur [NA1350] [Class 9]; Sulfur [UN1350] [Flammable solid]; Sulfur 10 microg/mL in Isooctane; Sulfur atom; Sulfur bactericide,fumigant; Sulfur Compounds; Sulfur hydride; Sulfur hydroxide; Sulfur in Isooctane standard solution, Specpure, 100g/g (0.010%); Sulfur in Isooctane standard solution, Specpure, 10g/g (0.001%); Sulfur in Isooctane standard solution, Specpure?, 25?g/g (0.0025%); Sulfur ointment; Sulfur precipitated; Sulfur Soap; Sulfur vapor; Sulfur, 99.998% trace metals basis; SULFUR, 99.999%; Sulfur, colloidal, metastable technetium-99 labeled; Sulfur, elemental; Sulfur, flakes, >=99.99% trace metals basis; Sulfur, LR, >=99%; Sulfur, molten [NA2448] [Class 9]; Sulfur, molten [UN2448] [Flammable solid]; Sulfur, monoclinic; Sulfur, PESTANAL(R), analytical standard; Sulfur, pharmaceutical; Sulfur, powder, 99.98% trace metals basis; Sulfur, powder, colloidal; Sulfur, precipitated


Sulfur, molten appears as a pale yellow crystalline solid with a faint odor of rotten eggs. Insoluble in water. A fire and explosion risk above 450° F. Transported as a yellow to red liquid. Handled at elevated temperature (typically 290°F) to prevent solidification and makes transfers easier. Hot enough that plastic or rubber may melt or lose strength. Causes thermal burns to skin on contact. Cools rapidly and solidifies if released. Equipment designed to protect against ordinary chemical exposure is ineffective against the thermal hazard. Exercise caution walking on the surface of a spill to avoid breakthrough into pockets of molten sulfur below the crust. Do not attempt to remove sulfur impregnated clothing because of the danger of tearing flesh if a burn has resulted. May be irritatin to skin, eyes and mucous membranes. Used in sulfuric acid production, petroleum refining, and pulp and paper manufacturing.Pure sulfur exists in two stable crystalline forms, alpha and beta, and at least two amorphous (liquid) forms. Alpha-sulfur: rhombic, octahedral, yellow crystals; beta-sulfur: monoclinic, prismatic, pale-yellow crystals.Pure sulfur is odorless, but traces of hydrocarbon impurity may impart an oily and/or rotten egg odor.Faint taste.Boiling Point:832.3 °F at 760 mm Hg.Melting Point:251 °F.Flash Point:405 °F.Insoluble in water; slightly soluble in ethanol, benzene, ethyl ether; soluble in carbon disulfide.Insoluble in water; slightly soluble in ethanol, benzene, ethyl ether; soluble in carbon disulfide.Dynamic viscosity of liquid (Pa.s): 0.17 at 120 °C; 0.008 at 140 °C; 0.0064 at 158 °C; 5.952 at 160 °C; 86.304 at 180 °C; 93.0 at 187.8 °C; 78.864 at 200 °C; 3.72 at 300 °C.Sulfur is not considered corrosive to the usual construction materials. However, acid-generating impurities, which may be introduced in handling and storage, create corrosive conditions..Ignites in air above 261 °C, in oxygen below 260 °C, burning to the dioxide; combines readily with hydrogen; combines in the cold with fluorine, chlorine, and bromine; combines with carbon at high temperatures; reacts with silicon, phosphorus, arsenic, antimony and bismuth at their melting points; combines with nearly all metals; with lithium, sodium, potassium, copper, mercury and silver in the cold on contact with the solid; with magnesium, zinc and cadmium very slightly in the cold, more readily on heating; with other metals at high temperatures. Does not react with iodine, nitrogen, tellurium, gold, platinum and iridium.When the liquid phase consists solely of octatomic sulfur rings, the temperature ranges at which the various modifications form are called the ideal freezing points. The temperature at which the crystalline forms are in equilibrium with liquid sulfur containing equilibrium amounts of S(pie) and S(mu) are called natural freezing points.At room temp the thermodynamic stable sulfur modification is orthorhombic sulfur that converts at 94 °C to monoclinic sulfur. The latter melts at 124-128 °C forming a mixture of liquid allotropes that includes cyclooctasulfur, cyclododecasulfur, as well as chain species.Sol in light petroleum and turpentine oil, and in hot aq soln of alkali hydroxides forming polysulfides and thiosulfates; Solubility: 1 in 60 chloroform, 1 in 600 ether.Research tool in studying mechanism of rubber vulcanization and polymerization of synthetic rubber, role of sulfur in the coking process and in steel, effect of sulfur on engine wear, sulfur removal in the viscose process, behaviour of detergents during ashing, sulfur deposition in diesel engines, action of sulfur in silver plating solutions, protein metabolism, surface active agents and surface phenomena, drug actions, etc.Sulfur is a keratolytic agent and scabicide.Topical sulfur preparations are used principally for the symptomatic treatment of acne vulgaris. Although the drug may relieve plugging and rupturing of follicles, ease the evacuation of comedones, and promote peeling of the skin, some clinicians believe that topical sulfur may also promote the formation of new comedones.opical 5-10% sulfur ointment (in a petrolatum base; no longer commercially available in the US) has been used for the treatment of scabies. Because sulfur ointment is messy, malodorous, tends to stain, and can produce an irritant dermatitis, its use has largely been supplanted by permethrin, lindane, or other scabicides for most patients.For relief of itching and scalp flaking associated with dandruff, 2-5% "sulfur" alone or, most often, in combination with salicylic acid, usually is used as a lotion shampoo. The lotion should be applied to wet hair and massaged vigorously into the scalp; the scalp then is rinsed thoroughly and application of the lotion and rinsing is repeated. The lotion usually is used as a shampoo twice weekly.The absorption, distribution, and elimination of "sulfur" following topical application have not been fully characterized. Topically applied "sulfur" reportedly penetrates the skin and is detectable in the epidermis within 2 hours after application and throughout the skin within about 8 hours; the drug is not detectable in skin 24 hours after application. Percutaneous absorption of the drug into systemic circulation reportedly occurred following topical application of a 25% "sulfur" ointment to abraded skin of animals but did not occur when the drug was applied to intact skin.Topically applied sulfur has mild antifungal and antibacterial activity. It has been suggested that when applied topically to the skin, sulfur forms hydrogen sulfide and/or polythionic acid, which may exert germicidal activity. In vitro studies indicate that sulfur has little if any fungistatic or fungicidal activity. Therefore, sulfur's antifungal activity probably results largely from its keratolytic action, causing shedding of fungal spores and hyphae embedded within the stratum corneum. In vitro, sulfur has been shown to have some antibacterial activity; the drug has a potent inhibitory effect against some streptococci, a moderate inhibitory effect against Staphylococcus aureus, and no activity against gram-negative bacteria. It has been suggested that the drug's antibacterial activity may partly result from inactivation of sulfhydryl groups contained in bacterial enzyme systems, since the antibacterial effect of the drug has reportedly been neutralized by addition of cysteine and other sulfhydryl-containing compounds to the culture medium. Topically applied sulfur is reportedly toxic to the parasitic arthropod Sarcoptes scabiei.The exact mechanism(s) of action of "sulfur" in the treatment of acne is not fully understood but is presumed to involve the drug's keratolytic and antibacterial effects. Although some studies indicate that "sulfur" may also be comedogenic, other studies have been unable to substantiate this effect and the drug generally is considered effective in the topical treatment of acne.The aim of this research was to analyze the effects and the modes of action of elemental sulfur (S(0)) in bioluminescence and respiration of Vibrio fischeri cells and the enzymes crude luciferase, pure catalase, and alcohol dehydrogenase (ADH). Metallic copper removed sulfur and reduced the toxicity of acetone extracts of sediment samples analyzed in the bioluminescence test. The sulfur inhibition of cell bioluminescence was noncompetitive with decanal, the luciferase substrate; reversible, with maximum toxicity after 15 min (EC50 = 11.8 ug/L); and almost totally recovered after 2 hr. In vitro preincubation of crude luciferase extract with sulfur (0.28 ppm) weakly inhibited bioluminescence at 5 min, but at 30 min the inhibition reached 60%. Increasing the concentration of sulfur in the parts per million concentration range in vitro decreased bioluminescence, which was not constant, but depended on exposure time, and no dead-end/total inhibition was observed. The redox state of enzymes in the in vitro system significantly affected inhibition. Hydrogen peroxide restored fully and the reducing agent dithiothreitol, itself toxic, restored only partially luciferase activity in the presence of sulfur. Sulfur (5.5 ppm) slightly inhibited ADH and catalase, and dithiothreitol enhanced sulfur inhibition. High sulfur concentrations (2.2 ppm) inhibited the bioluminescence and enhanced the respiration rate of V. fischeri cells. Elemental sulfur data were interpreted to show that sulfur acted on at least a few V. fischeri cell sites: reversibly modifying luciferase at sites sensitive to/protected by oxidative and reducing agents and by affecting electron transport processes, resulting in enhanced oxygen consumption. Sulfur together with an enzyme reducing agent inhibited the oxidoreductive enzymes ADH and catalase, which have /thiol/ groups, metal ion cofactors, or heme, respectively, in their active centers.Sulfur must be converted to pentathionic acid (H2S5O6) in order to exert germicidal action. Presumably oxidation of sulfur to pentathionic acid is accomplished by certain microorganisms or by epidermal cells when element is applied to skin. Sulfur possesses a keratolytic property, which may be the basis for the therapeutic action of the element in certain cutaneous disorders unassociated with infection.For sulfur (USEPA/OPP Pesticide Code: 077501) ACTIVE products with label matches. /SRP: Registered for use in the U.S. but approved pesticide uses may change periodically and so federal, state and local authorities must be consulted for currently approved uses.In manufacturing sulfuric acid, carbon disulfide, sulfites, plastics, enamels, metal-glass cements; in making gunpowder, matches; for bleaching wood pulp, straw, wool, silk, felt, linen.In making phosphatic fertilizers; fumigant; bleaching of dried fruits; element is good electrical insulator.Diseases: apple scab, brown rot, leaf spot, rust, and powdery mildew on apples, grapes, ornamentals, peaches, pecans, peanuts, roses. Insects: fleahoppers, mites on alfalfa, almonds, apricots, artichokes, bananas, barley, beans, beets, cabbage, carrots, cauliflower, citrus, corn, cotton, dates, eggplant, mangoes, melons, mustard greens, oats, onions, peppers, plums, potatoes, prunes, strawberries, sugar beets, tomatoes, wheat.Sulfuric acid manufacture, pulp and paper manufacture, carbon disulfide, rubber vulcanization, detergents, petroleum refining, dyes and chemicals, drugs and pharmaceuticals, explosives, rodent repellants, soil conditioner, coating for controlled-release fertilizers, nucleating reagent for photographic film, cement sealant, binder and asphalt extender in road paving (up to 40%), base material for low-temperature mortars.Through its major derivative, sulfuric acid, sulfur ranks as one of the more-important elements used as an industrial raw material. It is of prime importance to every sector of the world's industrial and fertilizer complexes. Sulfuric acid production is the major end use for sulfur, and consumption of sulfuric acid has been regarded as one of the best indexes of a nation's industrial development. More sulfuric acid is produced in the United States every year than any other chemical.A Claus sulfur recovery unit consists of a combustion furnace, waste heat boiler, sulfur condenser, and a series of catalytic stages each of which employs reheat, catalyst bed, and sulfur condenser. Typically, two or three catalytic stages are employed. The Claus process converts hydrogen sulfide to elemental sulfur via a two-step reaction. The first step involves controlled combustion of the feed gas to convert approximately one-third of the hydrogen sulfide to sulfur dioxide and noncatalytic reaction of unburned hydrogen sulfide with sulfur dioxide. In the second step, the Claus reaction, the hydrogen sulfide and sulfur dioxide react over a catalyst to produce sulfur and water. ... The amount of combustion air is tightly controlled to maximize sulfur recovery, ie, maintaining the appropriate reaction stoichiometry of 2:1 hydrogen sulfide to sulfur dioxide throughout downstream reactors. Typically, sulfur recoveries of up to 97% can be achieved.Two forms of sulfur of 99.5% purity or better are recognized in pharmacy: sublimed sulfur, also known as flowers of sulfur, and precipitated sulfur, also known as milk of sulfur, made by boiling sublimed sulfur with lime and precipitating with hydrochloric acid. Other sulfur preparations include: washed sulfur, made by treating sublimed sulfur with ammonia and washing with water to dissolve impurities, particularly arsenic; sulfurated lime, the active component of Vleminckx's lotion, made by boiling sublimed sulfur with lime, resulting in formation of calcium pentasulfide and calcium thiosulfate; and sulfurated potash (K2(Sx)), also known as liver of sulfur, made by heating sublimed sulfur with potassium carbonate.Crude sulfur contains small percentages of carbonaceous matter. The amount of impurity is usually determined by combustion.Precipitated sulfur: Powder: Topical: Cake: 3%, Buf Acne Cleansing Bar; 10%, Sulfur Soap; Gel: 4%, Xerac (with isopropyl alcohol 44%); Lotion: 5%, Liquimat (with alcohol 22%); Precipitated sulfur combinations: Topical: Cake: 2% with Salicyclic Acid 2%, Aveeno Cleansing Bar (with colloidal oatmeal); 10% with Salicyclic Acid 3%, Salicyclic Acid and Sulfur Soap; Cream: 8% with Resorcinol 2%, Acnomel (with alcohol 11%); Lotion: 3% with Salicyclic Acid 2%, Acno (with alcohol 25%); 4% with Salicyclic Acid 1.5%, Night Cast (with alcohol 33%); 5% with Resorcinol 2%, Rezamid (with alcohol 28.5%); 5% with Sulfacetamide Sodium 10%, Sulface-R (with parabens, propylene glycol, and zinc oxide); 8% with Resorcinol 2%, Night Cast Special Formula (with alcohol 31%); Shampoo: 2% with Coal Tar Soln 5% and Salicyclic Acid 1%, Vanseb-T (cream or lotion); 2% with Salicyclic 1%, Vanseb (cream or lotion); 5% with Sodium Salicyclate 0.5%, pHisoDan; Stick, 8% with Resorcinol 1%, Clearasil (with bentonite 4%)More than 85% of the sulfur consumed in the world is either converted to sulfuric acid or produced directly as such. Worldwide, well over half of the sulfuric acid is used in the manufacture of phosphatic fertilizers and ammonium sulfate for fertilizers.About 87% of sulfur was converted to sulfuric acid prior to end use.Ultra-low sulfur diesel (ULSD) is diesel fuel with 15 parts per million or lower sulfur content. The U.S. Environmental Protection Agency requires 80% of the highway diesel fuel refined in or imported into the United States (100% in California) to be ultra-low sulfur diesel. One hundred percent must be ULSD nationwide by 2010. Currently, the vast majority of ultra-low sulfur diesel is produced from petroleum. However, biodiesel (along with some emerging advanced fuels) is inherently ultra-low sulfur and could help meet ULSD requirements in the future. Ultra-low sulfur content in diesel fuel is beneficial because it enables use of advanced emission control technologies on light- and heavy-duty diesel vehicles. The combination of ULSD with advanced emission control technologies is sometimes called "clean diesel."Sulfur recovered as a by-product, involuntary sulfur, accounts for a larger portion of world supply than does mined or voluntary material. Sulfur is obtained from hydrogen sulfide, which evolves when natural gas, crude petroleum (qv), tar sands (qv), oil shales (qv), coal (qv), and geothermal brines are desulfurized. Other sources of sulfur include metal sulfides such as pyrites; sulfate materials, including gypsum; and elemental sulfur in native and volcanic deposits mined in the traditional manner.AOAC Method 952.25. Sulfur; Titrimetric carius combustion method (12) Official final action (not applicable in presence of phosphorus). Place weighed sample /greater or equal to 0.75 mg sulfur/ in combustion tube, add /fine crystals of/ sodium chloride 100% in excess of amt equivalent to sulfur sample, and ... /add 0.5 + or - 0.03 mL fuming nitric acid. Using blast lamp & holding at 30-40 deg angle, slowly rotate tube in flame until wall thickens, pull out, and seal off. Immediately place tube in furnace and heat 5 hr at 250 or 300 + or - 10 °C. Remove vented tube from furnaces and cut off constricted end./ Transfer contents of tube to 50 mL beaker, rinsing tube 4-6 times with 3-5 mL portions water. Evaporate to dryness on steam bath. Dissolve residue in 10 mL water, pour solution into titration cell, add 1 drop phenolphthalein, and make just alkaline with about 0.1 N sodium hydroxide, then acid with about 0.02 N hydrochloric acid, adding 1 drop excess. Add about 0.15 g of /tetrahydroxyquinone sulfate/ indicator, stir to dissolve ... using enough alcohol so that final soln contains about 50%. Titrate with standard barium chloride soln from 5 mL buret until stable color of soln immediately after stirring matches standard glass color filter. ... % sulfur= (mL barium chloride - mL blank) X normality X 16.032 X 100 mg/mg sample /Total sulfur/.AOAC Method 955.48. Sulfur; Gravimetric carius combustion method (13) Official final action (Applicable in presence of phosphorus). /Place weighed sample (greater or equal to 0.75 mg sulfur) in combustion tube, add fine crystals of sodium chloride 100% in excess of amt equivalent to sulfur sample, and add 0.5 + or - 0.03 mL fuming nitric acid. Using blast lamp & holding at 30-40 deg angle, slowly rotate tube in flame until wall thickens, pull out, and seal off. Immediately place tube in furnace and heat 5 hr at 250 or 300 + or - 10 °C. Remove vented tube from furnaces and cut off constricted end. Transfer contents of tube to 50 mL beaker, rinsing tube 4-6 times with 3-5 mL portions water. Evaporate to dryness on steam bath./ Dissolve residue ... in 3 mL water, pour into previously ignited and weighed (with filter stick) porcelain crucible. Place crucible on steam bath until soln is near boiling point. ... Slowly draw off soln, and rinse precipitate ... Place crucible and filter in larger crucible and dry in oven for 10 min at about 110 °C. Ignite in furnace 10 min at 700-750 °C ... cool on metal block 30 min or in desiccator 1 hr, and weigh. Determine blank on reagents. % sulfur= (wt of barium sulfate - blank) x 0.1374 X 100/wt sample /Total sulfur/.The major hazards encountered in the use and handling of sulfur stem from its toxicologic properties and flammability. Toxic by all routes (ie, inhalation, ingestion, and dermal contact), exposure to this pale yellow, crystalline substance may occur from the extraction of sulfur-bearing rock, its use in fertilizer, the production of sulfuric acid and other sulfur compounds, in wood pulping, in the vulcanization of rubber, and in the manufacture of matches, explosives, and dyes. Effects from exposure may include ulceration of the skin, conjunctivitis, inflammation of the nasal mucosa, shortness-of-breath, asthma, and tracheobronchitis. In activities and situations where over-exposure may occur, wear chemical protective clothing and a self-contained breathing apparatus. If exposure should occur, immediately irrigate eyes with copious amounts of tepid water for at least 15 minutes and wash skin extremely thoroughly with soap and water. Contaminated clothing should be removed and left at the work site for cleaning before reuse. Sulfur is an easily ignitable solid. In a powdered form it may form explosive mixtures with air, or in contact with oxidizing materials. Sulfur burns with a blue flame that may be difficult to see in daylight, and produces toxic sulfur dioxide gas. For fires involving sulfur, extinguish with dry chemical, sand, water spray (straight streams may scatter the material), fog, or standard foam. If water is used, apply from as far a distance as possible. Sulfur should be stored in a cool, well ventilated area, away from sources of ignition, physical damage, chlorates, nitrates, and other oxidizing materials. Sulfur may be shipped domestically via air, rail, road, and water. International shipments may require the label, "Flammable solid." Small dry spills of sulfur may be carefully shovelled into a clean, dry, covered container for recovery or later disposal. Large spills may be wetted down with water and diked for later disposal. Do not allow material to enter water sources or sewers.Vapors given off during melting of sulfur may contain sufficient hydrogen sulfide & carbon disulfide to permit ignition of air/vapor mixture on contact with hot surface; such ignition may result in transmission of flames to molten sulfur. ... Sulfur is poor conductor of electricity & tends to develop charges of static electricity during transport or processing; static discharge may lead to ignition of sulfur dust. Fires in heaps of sulfur are frequent & insidious since they may break out again even after original conflagration has ... Been extinguished.Environmental considerations: Water spill: Use natural barriers or oil spill control booms to limit spill travel. Use natural deep water pockets, excavated lagoons, or sand bag barriers to trap material at bottom. Remove trapped material with suction hoses.The most favorable course of action is to use an alternative chemical product with less inherent propensity for occupational harm/injury/toxicity or environmental contamination. Recycle any unused portion of the material for its approved use or return it to the manufacturer or supplier. Ultimate disposal of the chemical must consider: the material's impact on air quality; potential migration in soil or water; effects on animal and plant life; and conformance with environmental and public health regulations.The scientific literature for the use of contact lenses by industrial workers is inconsistent. The benefits or detrimental effects of wearing contact lenses depend not only upon the substance, but also on factors including the form of the substance, characteristics and duration of the exposure, the uses of other eye protection equipment, and the hygiene of the lenses. However, there may be individual substances whose irritating or corrosive properties are such that the wearing of contact lenses would be harmful to the eye. In those specific cases, contact lenses should not be worn. In any event, the usual eye protection equipment should be worn even when contact lenses are in place.SULFUR reacts violently with strong oxidizing agents causing fire and explosion hazards [Handling Chemicals Safely 1980 p. 871]. Reacts with iron to give pyrophoric compounds. Attacks copper, silver and mercury. Reacts with bromine trifluoride, even at 10°C [Mellor 2:113. 1946-47]. Ignites in fluorine gas at ordinary temperatures [Mellor 2:11-13 1946-47]. Reacts to incandescence with heated with thorium [Mellor 7:208 1946-47]. Can react with ammonia to form explosive sulfur nitride. Reacts with calcium phosphide incandescently at about 300°C. Reacts violently with phosphorus trioxide [Chem. Eng. News 27:2144 1949]. Mixtures with ammonium nitrate or with metal powders can be exploded by shock [Kirk and Othmer 8:644]. Combinations of finely divided sulfur with finely divided bromates, chlorates, or iodates of barium, calcium, magnesium, potassium, sodium, or zinc can explode with heat, friction, percussion, and sometimes light [Mellor 2 Supp.1:763. 1956]. A mixture with barium carbide heated to 150°C becomes incandescent. Reacts incandescently with calcium carbide or strontium carbide at 500°C. Attacks heated lithium, or heated selenium carbide with incandescence [Mellor 5:862 1946-47]. Reacts explosively if warmed with powdered zinc [Mellor 4:476. 1946-47]. Reacts vigorously with tin [Mellor 7:328. 1946-47]. A mixture with potassium nitrate and arsenic trisulfide is a known pyrotechnic formulation [Ellern 1968 p. 135]. Mixtures with any perchlorate can explode on impact [ACS 146:211-212]. A mixture of damp sulfur and calcium hypochlorite produces a brilliant crimson flash with scatter of molten sulfur [Chem. Eng. News 46(28):9 1968]. Takes fire spontaneously in chlorine dioxide and may produce an explosion [Mellor 2:289 (1946-47)]. Ignites if heated with chromic anhydride ignite and can explode, [Mellor 10:102 (1946-47)]. Even small percentages of hydrocarbons in contact with molten sulfur generate hydrogen sulfide and carbon disulfide, which may accumulate in explosive concentrations. Sulfur reacts with Group I metal nitrides to form flammable mixtures, evolving flammable and toxic NH3 and H2S gases if water is present (Mellor, 1940, Vol. 8, 99).Sulfur-plus-chlorate explosion is remarkably spontaneous in presence of copper ion or copper, e.g., in the form of bronze screen, even at room temp. ... Sulfur & chromic anhydride ignite when heated & can explode. ... Even small percentages of hydrocarbons in contact with molten sulfur generate hydrogen sulfide & carbon disulfide, which may accumulate in explosive concentration. ... Mixture of sulfur & lead chlorite will explode.An explosive reaction /sulfur & silver bromate/ occurs in the presence of water. A mixture of sulfur & silver chlorate ignites @ about 74 °C. ... When finely divided sulfur is ground with silver oxide, the mixture ignites. ... Solid sulfur will ignite if mixed with solid sodium chlorite & moistened.Lithium carbide burns in vapors of sulfur ... Mixture with mercurous oxide will ignite from light impact. Powdered nickel heated with sulfur ... Reacts with incandescence. Mixture of sulfur & potassium chlorate ignites at about 160-162 °C. ... Mixture of /sulfur, potassium nitrate & arsenic trisulfide/ is a known pyrotechnic formulation.Potassium perchlorate & sulfur/ mixture, used in flashcrackers, can be exploded by moderately strong impact. When powdered sulfur is heated with potassium permanganate, an explosion may occur. Mixture of silver nitrate & sulfur explodes when struck with hammer.As the federal pesticide law FIFRA directs, EPA is conducting a comprehensive review of older pesticides to consider their health and environmental effects and make decisions about their future use. Under this pesticide reregistration program, EPA examines health and safety data for pesticide active ingredients initially registered before November 1, 1984, and determines whether they are eligible for reregistration. In addition, all pesticides must meet the new safety standard of the Food Quality Protection Act of 1996. Sulfur is found on List A, which contains most food use pesticides and consists of the 194 chemical cases (or 350 individual active ingredients) for which EPA issued registration standards prior to FIFRA, as amended in 1988. Case No: 0031; Pesticide type: fungicide; Registration Standard Date: 12/19/82; Case Status: RED Approved 05/91; OPP has made a decision that some/all uses of the pesticide are eligible for reregistration, as reflected in a Reregistration Eligibility Decision (RED) document.; Active ingredient (AI): sulfur; AI Status: OPP has completed a Reregistration Eligibility Decision (RED) document for the case/AI.Sulfur accounts for 15% of the inner core of the earth and 0.052% of its crust. The total sulfur content of the earth is estimated to be about 18.2X10+15 tons. The world is rich in large and highly pure deposits of elemental sulfur from which commercial sulfur can be mined. Sulfur minerals include gypsum, epsomite, miralulite, pyrite and marcasite, sphalerite, chalcopyrite, cobaltitle, pyrrhalite, galena, arsenopyrite, and pentlandite. Elemental sulfur occurs in salt domes, volcanic deposits and some deposits of calcite, gypsum, and anhydrite. In every state, whether gas, liquid, or solid, elemental sulfur occurs in more than one allotropic form. Three are relevant in nature: -2 (sulfhydryl and sulfide), 0 (elemental sulfur), and +6 (sulfate). The global sulfur cycle involves an atmospheric flux of about (140-350)X10+6 tons/annum, with (40-60)X10+6 tons as anthropogenic sulfur, in the form of sulfur dioxide, sulfuric acid, and sulfate. The rest ((100-290)X10+6 tonns/annum) involves biological decay, sea spray, and volcanism. However, the increasing acid precipitation from industrial stack emissions has seriously disturbed the natural sulfur cycle. Sulfur also paricipates in microbial cycles. Numerous microorganisms and plants use sulfate as their sole source of sulfur, converting it to organic sulfhydryl compounds in the oxidation state of -2. Many microorganisms, mainly Thiobacillus sp., can produce sulfide which under aerobic conditions is oxidized to sulfur and sulfate either spontaneously or through biochemical processes.Sulfur accounts for 15% of the inner core of the earth and 0.052% of its crust. The total sulfur content of the earth is estimated to be about 18.2X10+15 tons. ... The global sulfur cycle involves an atmospheric flux of about (140-350)X10+6 tons/annum, /with (100-290)X10+6 tonns/annum involving/ ... biological decay, sea spray, and volcanism. Sulfur also paricipates in microbial cycles. The world is rich in large and highly pure deposits of elemental sulfur from which commercial sulfur can be mined.

Molecular Weight 32.07 g/mol    
XLogP3-AA 0.5    
Hydrogen Bond Donor Count 0    
Hydrogen Bond Acceptor Count 1    
Rotatable Bond Count 0    
Exact Mass 31.972071 g/mol    
Monoisotopic Mass 31.972071 g/mol    
Topological Polar Surface Area 1 Ų
Heavy Atom Count 1    
Formal Charge 0    
Complexity 0
Isotope Atom Count 0
Defined Atom Stereocenter Count    0 
Undefined Atom Stereocenter Count 0    
Defined Bond Stereocenter Count    0
Undefined Bond Stereocenter Count 0
Covalently-Bonded Unit Count 1
Compound Is Canonicalized Yes    

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