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J & K SCIENTIFIC LTD.
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| Products Intro: | Product Name:Sulfur, sublimed, 99.5%
CAS:7704-34-9
Purity:99.50% Package:2.5KG, 25GR |
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Meryer (Shanghai) Chemical Technology Co., Ltd.
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| Products Intro: | Product Name:Sulfur
CAS:7704-34-9
Purity:99.5% Package:500g Remarks:AAA125312 |
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3B Pharmachem (Wuhan) International Co.,Ltd.
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| Products Intro: | Product Name:Sulfur
CAS:7704-34-9
Purity:99% HPLC Package:1Mg ; 5Mg;10Mg ;100Mg;250Mg ;500Mg ;1g;2.5g ;5g ;10g |
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Alfa Aesar
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| Products Intro: | Product Name:Sulfur, flowers, 99%
CAS:7704-34-9
Package:100g Remarks:A17260 |
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| | Sulfur Chemical Properties |
| Melting point | 114 °C | | Boiling point | 445 °C | | density | 2.36 | | vapor density | 8.9 (vs air)
| | vapor pressure | 1 mm Hg ( 183.8 °C)
| | Fp | 168 °C
| | solubility | carbon disulfide: in accordance1g/5mL | | form | powder
| | color | Yellow | | Water Solubility | Insoluble | | Merck | 13,9059 / 13,9067 | | CAS DataBase Reference | 7704-34-9(CAS DataBase Reference) | | NIST Chemistry Reference | Sulfur atom(7704-34-9) | | EPA Substance Registry System | Sulfur(7704-34-9) |
| | Sulfur Usage And Synthesis |
| Description | Sulfur belongs to a nonmetallic chemical element (pure product: yellow crystalline solid) under the symbol S. It can actively react with many other elements. It exists in various kinds of forms and compound such as sulfide and sulfate minerals which can be found everywhere around the universe and earth. It is also a key element for all life as the major component of amino acids, vitamins and many other cofactors. Sulfur has applications in various kinds of fields. For example, one of its biggest applications is for the production of sulfuric acid for sulfate and phosphate fertilizers. It is also used for the manufacturing of insecticides, fungicides, and bactericides. In pharmaceutical, it can be used for the manufacturing of many kinds of sulfur-containing antibiotics. | | Chemical Properties | yellow powder | | History | Sulfur was known to the alchemists from ancient times as brimstone. Lavoisier in 1772 proved sulfur to be an element. The element derived its name from both the Sanskrit and Latin names Sulvere and Sulfurium, respectively. Sulfur is widely distributed in nature, in earth's crust, ocean, meteorites, the moon, sun, and certain stars. It also is found in volcanic gases, natural gases, petroleum crudes, and hot springs. It is found in practically all plant and animal life. Most natural sulfur is in iron sulfides in the deep earth mantle. The abundance of sulfur in earth’s crust is about 350 mg/kg. Its average concentration in seawater is estimated to be about 0.09%. Sulfur occurs in earth’s crust as elemental sulfur (often found in the vicinity of volcanoes), sulfides, and sulfates. The most important sulfur-containing ores are iron pyrite, FeS2; chalcopyrite, CuFeS2; sphalerite, ZnS; galena, PbS; cinnabar HgS; gypsum CaSO4•2H2O; anhydrite CaSO4; kieserite, MgSO4•H2O; celestite, SrSO4; barite, BaSO4; and. stibnite, Sb2S3.
| | Uses | Elemental sulfur is used for vulcanizing rubber; making black gunpowder; as a soil conditioner; as a fungicide; preparing a number of metal sulfides; and producing carbon disulfide. It also is used in matches; bleaching wood pulp, straw, silk, and wool; and in synthesis of many dyes. Pharmaceutical grade precipitated and sublimed sulfurs are used as scabicides and as antiseptics in lotions and ointments.
Important sulfur compounds include sulfuric acid, sulfur dioxide, hydrogen 890 SULFUR sulfide, sulfur trioxide, and a number of metal sulfides and metal oxo- salts such as sulfates, bisulfates, and sulfites. Numerous organic compounds contain sulfur, such as mercaptans, thiophenes, thiophenols, sulfate esters, sulfones, and carbon disulfide.
| | Production Methods | Elemental sulfur is recovered from its ore deposits found throughout the world. It is obtained commercially by the Frasch process, recovery from wells sunk into salt domes. Heated water under pressure is forced into the underground deposits to melt sulfur. Liquid sulfur is then brought to the surface. Sulfur is recovered by distillation. Often the ore is concentrated by froth flotation.
Elemental sulfur also is recovered as a by-product in processing natural gas and petroleum. Refining operations of natural gas and petroleum crude produce hydrogen sulfide, which also may occur naturally. Hydrogen sulfide is separated from hydrocarbon gases by absorption in an aqueous solution of alkaline solvent such as monoethanol amine. Hydrogen sulfide is concentrated in this solvent and gas is stripped out and oxidized by air at high temperature in the presence of a catalyst (Claus process).
Elemental sulfur also may be obtained by smelting sulfide ores with a reducing agent, such as coke or natural gas, or by reduction of sulfur dioxide.
| | Reactions | Sulfur forms two oxides, sulfur dioxide, SO2, and the trioxide, SO3. It burns in oxygen at about 250°C or in air above 260°C, forming sulfur dioxide. In excess oxygen the trioxide is obtained.
Sulfur reacts with hydrogen at 260 to 350°C forming hydrogen sulfide. The reaction is slow at this temperature and does not go to completion. The reaction is catalyzed by activated alumina.
Reactions with excess chlorine or fluorine yield sulfur tetrachloride, SCl4, or hexafluoride, SF6. These reactions occur under cold conditions.
Sulfur reacts with sulfur dioxide in an electric discharge to form disulfuroxide, S2O.
Sulfur reacts with aqueous sulfide to form polysulfides: S + Na2S → Na2S2
With aqueous solution of sulfite the product is thiosulfate:
S + SO32– → S2O32–
Thiosulfate also is obtained by heating sulfur with powdered sulfite:
S + Na2SO3 → Na2S2O3
When heated with alkali cyanide, thiocyanate salt is obtained:
S + KCN → KSCN
A similar reaction occurs in the aqueous phase in which thiocyanate is obtained by evaporation and crystallization.
Sulfur combines with alkali metals, copper, silver, and mercury on cold contact with the solid, forming sulfides. Reactions with magnesium, zinc, and cadmium occur to a small degree at ordinary temperatures, but rapidly on heating. Sulfur reacts with phosphorus, arsenic, antimony, bismuth, and silicon at their melting points and with other elements at elevated temperatures forming binary sulfides. Sulfides of tellurium, gold, platinum, and iridium are difficult to obtain even at elevated temperatures. Sulfur does not react with inert gases, nitrogen, and iodine.
| | General Description | 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. | | Air & Water Reactions | Flammable. Insoluble in water. | | Reactivity Profile | 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 gasses if water is present. (Mellor, 1940, Vol. 8, 99). | | Health Hazard | Can cause eye irritation; may rarely irritate skin. If recovered sulfur, refer to hydrogen sulfide.* | | References | https://en.wikipedia.org/wiki/Sulfur#Applications
http://geology.com/minerals/sulfur.shtml
http://www.wisegeek.org/what-is-sulfur.htm
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| | Sulfur Preparation Products And Raw materials |
| Raw materials | Acetic acid glacial-->Sodium carbonate-->Ammonia-->Carbon disulphide-->CARBON MONOXIDE-->HYDROGEN SULFIDE-->Sulphur-->Sodium hydrosulfide-->Titanium dioxide-->Phenolic epoxy resin-->Talc-->Bifenthrin-->Vanadium pentoxide -->4-Hydroxybenzenesulfonic acid-->PYRITE-->Triethylene glycol dimethacrylate-->Potassium sodium tartrate -->Heat exchanger-->Carbon monoxide and hydrogen mixtures | | Preparation Products | ETHYL 5-METHYL-4-OXO-3,4-DIHYDROTHIENO[2,3-D]-PYRIMIDINE-6-CARBOXYLATE-->5,6-DIMETHYLTHIENO[2,3-D]PYRIMIDIN-4(3H)-ONE-->ETHYL 2-AMINO-4-(4-METHOXYPHENYL)-3-THIOPHENECARBOXYLATE-->Ethylicin-->Sulfur Red Brown B3R-->Sulfur hexafluoride-->2-AMINO-5,6-DIHYDRO-4H-CYCLOPENTA[B]THIOPHENE-3-CARBONITRILE-->2-AMINO-6-METHYL-4,5,6,7-TETRAHYDRO-1-BENZOTHIOPHENE-3-CARBONITRILE-->1,2,3,5-TETRAHYDRO-8-THIA-5,7-DIAZA-CYCLOPENTA[A]INDENE-4-ONE-->ETHYL 2-AMINO-4,5-DIMETHYLTHIOPHENE-3-CARBOXYLATE-->5-AMINO-4-CYANO-3-METHYL-THIOPHENE-2-CARBOXYLIC ACID ETHYL ESTER-->4-Bromophenethyl alcohol-->2-AMINO-5-ISOPROPYL-THIOPHENE-3-CARBOXYLIC ACID ETHYL ESTER-->2-AMINO-4-ETHYL-5-METHYL-THIOPHENE-3-CARBOXYLIC ACID ETHYL ESTER-->2-AMINO-4,5,6,7-TETRAHYDRO-1-BENZOTHIOPHENE-3-CARBONITRILE-->2-AMINO-3-CYANO-4-METHYL-5-CARBMETHOXY THIOPHENE-->5-AMINO-3-METHYL-THIOPHENE-2,4-DICARBOXYLIC ACID DIMETHYL ESTER-->ETHYL 2-AMINO-4-METHYLTHIOPHENE-3-CARBOXYLATE-->2-AMINO-5-PHENYL-THIOPHENE-3-CARBOXYLIC ACID METHYL ESTER-->2-AMINO-5-TERT-BUTYL-THIOPHENE-3-CARBOXYLIC ACID ETHYL ESTER-->2-(2-PYRIDYL)BENZIMIDAZOLE-->1,3-DITHIOLE-2-THIONE-->2-AMINO-5-METHYL-THIOPHENE-3-CARBOXYLIC ACID ETHYL ESTER-->4,4'-Thiobis(6-tert-butyl-m-cresol)-->2-(4-Aminophenyl)-6-methyl-1,3-benzothiazole-7-sulfonic acid-->2-Thiopheneacetic acid-->5,6,7,8-TETRAHYDRO-3H-BENZO[4,5]THIENO[2,3-D]-PYRIMIDIN-4-ONE-->ETHYL 2-AMINO-5-PHENYLTHIOPHENE-3-CARBOXYLATE-->THIOPHENE-2-ACETAMIDE-->Isobutenyl sulfide-->ETHYL 2-AMINO-4,5,6,7-TETRAHYDROBENZO[B]THIOPHENE-3-CARBOXYLATE-->2-AMINO-5,6-DIHYDRO-4H-CYCLOPENTA[B]THIOPHENE-3-CARBOXYLIC ACID ETHYL ESTER-->Sulfur Yellow Brown 6G-->Anethole trithione-->SO^{2^} oxidation catalysts-->ammonium O,O-dimethyl thiophosphate -->PHENOXATHIIN |
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