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  • 7704-34-9 Structure
  • Basic information

    1. Product Name: Sulfur
    2. Synonyms: MICROTHIOL SPECIAL;RASULF;SULFUR;SULFUR, AAS STANDARD SOLUTION;Atomic sulfur;atomicsulfur;Bensulfoid;Biosulphur powder
    3. CAS NO:7704-34-9
    4. Molecular Formula: S8
    5. Molecular Weight: 256.52
    6. EINECS: 231-722-6
    7. Product Categories: Sulfur;Rubber Chemicals;Nonmetallic Element;Inorganics;FUNGICIDE;Essential Chemicals;Reagent Grade;Routine Reagents;AcaricidesMicro/Nanoelectronics;Electronic Chemicals;Pure Elements;InorganicsPesticides&Metabolites;AcaricidesPesticides;Alpha sort;Fungicides;Pesticides;Pesticides&Metabolites;Q-ZAlphabetic;S;SN - SZ;metal or element;rubber vulcanizing agent
    8. Mol File: 7704-34-9.mol
    9. Article Data: 219
  • Chemical Properties

    1. Melting Point: 114 °C
    2. Boiling Point: 445 °C
    3. Flash Point: 168 °C
    4. Appearance: Yellow/powder
    5. Density: 2.36
    6. Vapor Density: 8.9 (vs air)
    7. Vapor Pressure: 1 mm Hg ( 183.8 °C)
    8. Refractive Index: N/A
    9. Storage Temp.: N/A
    10. Solubility: carbon disulfide: in accordance1g/5mL
    11. Water Solubility: Insoluble
    12. Merck: 13,9059 / 13,9067
    13. CAS DataBase Reference: Sulfur(CAS DataBase Reference)
    14. NIST Chemistry Reference: Sulfur(7704-34-9)
    15. EPA Substance Registry System: Sulfur(7704-34-9)
  • Safety Data

    1. Hazard Codes: F,Xi
    2. Statements: 11-38
    3. Safety Statements: 16-26-46
    4. RIDADR: UN 1350 4.1/PG 3
    5. WGK Germany: 1
    6. RTECS: WS4250000
    7. TSCA: Yes
    8. HazardClass: 4.1
    9. PackingGroup: III
    10. Hazardous Substances Data: 7704-34-9(Hazardous Substances Data)

7704-34-9 Usage

Chemical Description

Sulfur is a chemical element.

Chemical Description

Sulfur is a yellow solid that is used in the production of sulfuric acid.

Chemical Description

Sulfur is a nonmetallic element that is often used in organic synthesis as a reducing agent or to promote cyclization reactions.

Chemical Description

Sulfur and chloranil are used in attempts to dehydrogenate some of the addition products, while bromine is used in the synthesis of tetrabromide of 1,4-diphenylbutadiene.

Chemical Description

Sulfur is used as a reagent in the reactions to form the sulfur-containing rings.

Description

Sulfur is a nonmetallic chemical element with the symbol S, known for its yellow crystalline solid form. It actively reacts with many other elements and exists in various forms and compounds such as sulfide and sulfate minerals, which are found everywhere around the universe and earth. Sulfur is a key element for all life, being a major component of amino acids, vitamins, and many other cofactors.

Uses

Used in Pharmaceutical Industry:
Sulfur is used as an ingredient in acne soaps and lotions for reducing oil-gland activity and dissolving the skin's surface layer of dry, dead cells. It is also used as a mild antiseptic in acne creams and lotions, stimulating healing when used on skin rashes. However, it may cause skin irritation and allergic skin reactions.
Used in Chemical Industry:
Sulfur is one of the four major commodities of the chemical industry, along with limestone, coal, and salt. It is primarily used to manufacture sulfuric acid (H2SO4), with forty million tons produced each year for various applications. Sulfur is also used in the production of fertilizers, lead-acid batteries, gunpowder, desiccants, matches, soaps, plastics, bleaching agents, rubber, road asphalt binders, insecticides, paint, dyes, and medical ointments, among many other uses.
Used in Agriculture:
Sulfur is a macronutrient required by plants in relatively large amounts. It is used to increase the acidity of soil and correct sulfur deficiency in plants. Sulfur is essential for the synthesis of amino acids, which are essential components of proteins. It also plays a role in chlorophyll synthesis and is part of ferridoxins, a type of non-heme iron-sulfur protein involved in the reduction of nitrite and sulfate and the assimilation of nitrogen by bacteria.
Used in Rubber Industry:
Elemental sulfur is used for vulcanizing rubber, a process that improves the elasticity, strength, and durability of rubber products.
Used in Mining and Explosives:
Sulfur is used in the production of black gunpowder, which is an explosive substance used in mining and other applications.
Used in Soil Conditioning and Fungicides:
Sulfur is used as a soil conditioner and as a fungicide to protect plants from fungal diseases.
Used in Metal Sulfides Production:
Sulfur is used in the preparation of a number of metal sulfides, which have various applications in different industries.
Used in Carbon Disulfide Production:
Sulfur is used in the production of carbon disulfide, which has various applications in the chemical industry.
Used in Matches and Bleaching:
Sulfur is used in the manufacturing of matches and for bleaching wood pulp, straw, silk, and wool.
Used in Dye Synthesis:
Sulfur is used in the synthesis of many dyes, contributing to the production of various colored products.
Used as Scabicides and Antiseptics:
Pharmaceutical grade precipitated and sublimed sulfurs are used as scabicides and as antiseptics in lotions and ointments, helping to treat skin conditions and prevent infections.

Isotopes

There are a total of 24 isotopes of sulfur; all but four of these are radioactive.The four stable isotopes and their contribution to sulfur’s total abundance on Earth areas follows: S-32 contributes 95.02% to the abundance of sulfur; S-33, just 0.75%; S-34,4.21%; and S-36, 0.02%.

Origin of Name

From the Sanskrit word sulvere and the Latin word sulphurim.

Characteristics

Sulfur exhibits a remarkable array of unique characteristics. Today, there are chemistsdevoting large portions of their careers to studying this unusual element. For example, whensulfur is melted, its viscosity increases, and it turns reddish-black as it is heated. Beyond200°C, the color begins to lighten, and it flows as a thinner liquid.Sulfur burns with a beautiful subdued blue flame. The old English name for sulfur was“brimstone,” which means “a stone that burns.” This is the origin of the term “fire and brimstone”when referring to great heat. Above 445°C, sulfur turns to a gas, which is dark orangeyellowbut which becomes lighter in color as the temperature rises.Sulfur is an oxidizing agent and has the ability to combine with most other elements toform compounds.

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.

History

Sulfur is found in meteorites. A dark area near the crater Aristarchus on the moon has been studied by R. W. Wood with ultraviolet light. This study suggests strongly that it is a sulfur deposit. Sulfur occurs native in the vicinity of volcanoes and hot springs. It is widely distributed in nature as iron pyrites, galena, sphalerite, cinnabar, stibnite, gypsum, Epsom salts, celestite, barite, etc. Sulfur is commercially recovered from wells sunk into the salt domes along the Gulf Coast of the U.S. It is obtained from these wells by the Frasch process, which forces heated water into the wells to melt the sulfur, which is then brought to the surface. Sulfur also occurs in natural gas and petroleum crudes and must be removed from these products. Formerly this was done chemically, which wasted the sulfur. New processes now permit recovery, and these sources promise to be very important. Large amounts of sulfur are being recovered from Alberta gas fields. Sulfur is a pale yellow, odorless, brittle solid that is insoluble in water but soluble in carbon disulfide. In every state, whether gas, liquid or solid, elemental sulfur occurs in more than one allotropic form or modification; these present a confusing multitude of forms whose relations are not yet fully understood. Amorphous or “plastic” sulfur is obtained by fast cooling of the crystalline form. X-ray studies indicate that amorphous sulfur may have a helical structure with eight atoms per spiral. Crystalline sulfur seems to be made of rings, each containing eight sulfur atoms that fit together to give a normal X-ray pattern. Twenty-one isotopes of sulfur are now recognized. Four occur in natural sulfur, none of which is radioactive. A finely divided form of sulfur, known as flowers of sulfur, is obtained by sublimation. Sulfur readily forms sulfides with many elements. Sulfur is a component of black gunpowder, and is used in the vulcanization of natural rubber and a fungicide. It is also used extensively is making phosphatic fertilizers. A tremendous tonnage is used to produce sulfuric acid, the most important manufactured chemical. It is used in making sulfite paper and other papers, as a fumigant, and in the bleaching of dried fruits. The element is a good electrical insulator. Organic compounds containing sulfur are very important. Calcium sulfate, ammonium sulfate, carbon disulfide, sulfur dioxide, and hydrogen sulfide are but a few of the many other important compounds of sulfur. Sulfur is essential to life. It is a minor constituent of fats, body fluids, and skeletal minerals. Carbon disulfide, hydrogen sulfide, and sulfur dioxide should be handled carefully. Hydrogen sulfide in small concentrations can be metabolized, but in higher concentrations it can quickly cause death by respiratory paralysis. It is insidious in that it quickly deadens the sense of smell. Sulfur dioxide is a dangerous component in atmospheric pollution. Sulfur (99.999%) costs about $575/kg.

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.

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).

Hazard

Many of the sulfur compounds are toxic but essential for life. The gas from elemental sulfurand from most of the compounds of sulfur is poisonous when inhaled and deadly wheningested. This is the reason that sulfur compounds are effective for rat and mice exterminationas well an ingredient of insecticides. Sulfa drugs (sulfanilamide and sufadiazine), althoughtoxic, were used as medical antibiotics during World War II before the development of penicillin.They are still used today in veterinary medicine.

Health Hazard

Can cause eye irritation; may rarely irritate skin. If recovered sulfur, refer to hydrogen sulfide.*

Flammability and Explosibility

Nonflammable

Safety Profile

Poison by ingestion, intravenous, and intraperitoneal routes. A human eye irritant. A fungcide. Chronic inhalation can cause irritation of mucous membranes. Combustible when exposed to heat or flame or by chemical reaction with oxidzers. Explosive in the form of dust when exposed to flame. Can react violently with halogens, carbides, halogenates, halogenites, zinc, uranium, tin, sodium, lithium, nickel, palladium, phosphorus, potassium, indum, calcium, boron, aluminum, (aluminum + niobium pentoxide), ammonia, ammonium nitrate, ammonium perchlorate, BrF5, BrF3, (Ca + VO + H20), Ca(OCl)2, Cad%, Cs3N, charcoal, (Cu + chlorates), ClO2, Cl0, ClF3, CrO3, Cr(OCl)2, hydrocarbons, IF5,IO5, Pb02, Hg(NO3)2, HgO, Hg20, NO2, P2O3, (KNO3 + As2S3), K3N, KMn04, AgNO3, Ag20, NaH, (NaNO3 + charcoal), (Na + SnI4), SCl2, T12O3, F2. Can react with oxidzing materials. To fight fire, use water or special mixtures of dry chemical. When heated it burns and emits highly toxic fumes of SOX. See also NUISANCE DUSTS.

Purification Methods

Murphy, Clabaugh & Gilchrist [J Res Nat Bur Stand 64A 355 1960] have obtained sulfur of about 99.999% purity by the following procedure: Roll sulfur was melted and filtered through a coarse-porosity glass filter funnel into a 2L round-bottomed Pyrex flask with two necks. Conc H2SO4 (300mL) was added to the sulfur (2.5kg), and the mixture was heated to 150o, stirring continuously for 2hours. Over the next 6hours, conc HNO3 was added in about 2mL portions at 10-15minutes intervals to the heated mixture. It was then allowed to cool to room temperature and the acid was poured off. The sulfur was rinsed several times with distilled water, then remelted, cooled, and rinsed several times with distilled water again, this process being repeated four or five times to remove most of the acid entrapped in the sulfur. An air-cooled reflux tube (ca 40cm long) was attached to one of the necks of the flask, and a gas delivery tube (the lower end about 2.5cm above the bottom of the flask) was inserted into the other. While the sulfur was boiled under reflux, a stream of helium or N2 was passed through to remove any water, HNO3 or H2SO4, as vapours. After 4hours, the sulfur was cooled so that the reflux tube could be replaced by a bent air-cooled condenser. The sulfur was then distilled, rejecting the first and the final 100mL portions, and transferred in 200mL portions to 400mL glass cylinder ampoules (which were placed on their sides during solidification). After adding about 80mL of water, displacing the air with N2, the ampoule was cooled, and the water was titrated with 0.02M NaOH, the process being repeated until the acid content was negligible. Finally, entrapped water was removed by alternate evacuation to 10mm Hg and refilling with N2 while the sulfur was kept molten. The ampoules were then sealed. Other purifications include crystallisation from CS2 (which is less satisfactory because the sulfur retains appreciable amounts of organic material), *benzene or *benzene/acetone, followed by melting and degassing. It has also been boiled with 1% MgO, then decanted, and dried under a vacuum at 40o for 2days over P2O5. [For the purification of S6, “recrystallised S8” and “Bacon-Fanelli sulfur” see Bartlett et al. J Am Chem Soc 83 103, 109 1961.]

References

https://en.wikipedia.org/wiki/Sulfur#Applications http://geology.com/minerals/sulfur.shtml http://www.wisegeek.org/what-is-sulfur.htm

Check Digit Verification of cas no

The CAS Registry Mumber 7704-34-9 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 7,7,0 and 4 respectively; the second part has 2 digits, 3 and 4 respectively.
Calculate Digit Verification of CAS Registry Number 7704-34:
(6*7)+(5*7)+(4*0)+(3*4)+(2*3)+(1*4)=99
99 % 10 = 9
So 7704-34-9 is a valid CAS Registry Number.
InChI:InChI=1/S

7704-34-9SDS

SAFETY DATA SHEETS

According to Globally Harmonized System of Classification and Labelling of Chemicals (GHS) - Sixth revised edition

Version: 1.0

Creation Date: Aug 16, 2017

Revision Date: Aug 16, 2017

1.Identification

1.1 GHS Product identifier

Product name sulfur atom

1.2 Other means of identification

Product number -
Other names sulfur

1.3 Recommended use of the chemical and restrictions on use

Identified uses For industry use only.
Uses advised against no data available

1.4 Supplier's details

1.5 Emergency phone number

Emergency phone number -
Service hours Monday to Friday, 9am-5pm (Standard time zone: UTC/GMT +8 hours).

More Details:7704-34-9 SDS

7704-34-9Synthetic route

sulfur dioxide
7446-09-5

sulfur dioxide

water
7732-18-5

water

A

sulfuric acid
7664-93-9

sulfuric acid

B

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
at 170-180°C; in very dilute soln. complete decompn. in 2 h, incomplete decompn. in concd. solns.;A n/a
B 100%
byproducts: H2S4O6;
sodium thiosulfate In water 100°C;
carbon monoxide
201230-82-2

carbon monoxide

sulfur dioxide
7446-09-5

sulfur dioxide

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
With catalyst: CeO2.Co3O4 284-465°C, metal oxide mixture catalysts activity: CuCo2O4;100%
With catalyst: CuCo2O4 284-465°C, metal oxide mixture catalysts activity: CuCo2O4;100%
With catalyst: LaCoO3 284-465°C, metal oxide mixture catalysts activity: CuCo2O4;100%
vanadium sulfate

vanadium sulfate

A

hydrogen
1333-74-0

hydrogen

B

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
1690°C complete decompn.;A 100%
B n/a
red heat;A 7%
B n/a
400°C;
barium dithionate

barium dithionate

A

barium sulfate

barium sulfate

B

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
With water In water byproducts: H2SO4; 6-8 h at 150-180°C;A 100%
B n/a
With H2O In water byproducts: H2SO4; 6-8 h at 150-180°C;A 100%
B n/a
With water In water byproducts: H2SO4, SO2; incomplete decompn.;
With H2O In water byproducts: H2SO4, SO2; incomplete decompn.;
tungsten(IV) sulfide

tungsten(IV) sulfide

A

sulfur
7704-34-9

sulfur

B

tungsten
7440-33-7

tungsten

Conditions
ConditionsYield
2000°C, fast react.;A n/a
B 100%
2000°C, fast react.;A n/a
B 100%
1200°C, 2 h;A n/a
B 60%
1200°C, 2 h;A n/a
B 60%
cadmium(II) dithionate

cadmium(II) dithionate

A

cadmium sulfate

cadmium sulfate

B

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
With water byproducts: H2SO4; 150-180°C under N2;A 100%
B n/a
With H2O byproducts: H2SO4; 150-180°C under N2;A 100%
B n/a
ammonium thiosulfate

ammonium thiosulfate

hydrogen sulfide
7783-06-4

hydrogen sulfide

A

water
7732-18-5

water

B

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
In water Kinetics; Reduction of (NH4)2S2O3 (c=0.4 mole/liter) by H2S in aq. soln. (50°C, pH=5, p(H2S)=0.08 MPa) in presence of Si-based catalyst.; Gravimetrical determination of S.;A n/a
B 99.7%
In water Kinetics; Reduction of (NH4)2S2O3 (c=1.0 mole/liter) by H2S in aq. soln. (50°C, pH=5, p(H2S)=0.08 MPa) in presence of Si-based catalyst.; Gravimetrical determination of S.;A n/a
B 99.87%
In water Kinetics; Reduction of (NH4)2S2O3 (c=1.0 mole/liter) by H2S in aq. soln. (50°C, pH=5, p(H2S)=0.08 MPa).; Gravimetrical determination of S.;A n/a
B 76.1%
In water Kinetics; Reduction of (NH4)2S2O3 (c=0.4 mole/liter) by H2S in aq. soln. (50°C, pH=5, p(H2S)=0.08 MPa).; Gravimetrical determination of S.;A n/a
B 71.5%
hydrogen sulfide
7783-06-4

hydrogen sulfide

sulfur dioxide
7446-09-5

sulfur dioxide

A

water
7732-18-5

water

B

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
In hydrogenchloride 20°C;satd. solns.; molar ratio 2 : 1; 15 % HCl soln., ,30 min;; S coagulated by addn. of gelatine or Al2(SO4)3;A n/a
B 99.7%
In hydrogenchloride 20°C;satd. solns.; molar ratio 2 : 1; 15 % HCl soln., ,30 min;; S coagulated by addn. of gelatine or Al2(SO4)3;A n/a
B 99.7%
In hydrogenchloride 20°C; satd. solns.; molar ratio 2 : 1; 3.5 % HCl soln.;; S coagulated by addn. of gelatine or Al2(SO4)3;;A n/a
B 93.5%
sulfur dioxide
7446-09-5

sulfur dioxide

A

sulfuric acid
7664-93-9

sulfuric acid

B

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
In not given Electrolysis; Pt anode, graphite cathode, area of the electrodes 30 cm^2, 1 A, 20 min, 0.208 mg/l SO2 soln.;A 98.16%
B 70.87%
In not given Electrolysis; Pt anode, graphite cathode, area of the electrodes 30 cm^2, 1 A, 20 min, 0.420 mg/l SO2 soln.;A 98.52%
B 74.28%
In not given Electrolysis; Pt anode, graphite cathode, area of the electrodes 30 cm^2, 1 A, 20 min, 1.123 mg/l SO2 soln.;A 98.86%
B 74.2%
hydrgensulfide(1-)

hydrgensulfide(1-)

hydrogen sulfite

hydrogen sulfite

A

Sulfate
14808-79-8

Sulfate

B

thiosulphate ion
14383-50-7

thiosulphate ion

C

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
In water byproducts: H2O; at ambient temp., molar ratio HS(1-) : HSO3(1-) = 1 : 2 must be adjusted as exactly as possible;; only small amts. of S and sulfate form;;A n/a
B 98%
C n/a
In water byproducts: H2O; at ambient temp., molar ratio HS(1-) : HSO3(1-) = 1 : 2 must be adjusted as exactly as possible;; only small amts. of S and sulfate form;;A n/a
B 98%
C n/a
2,2,4,4,6,6-hexamethyl-1,3,5,2,4,6-trithiatristanninane
16892-64-1

2,2,4,4,6,6-hexamethyl-1,3,5,2,4,6-trithiatristanninane

N-chloro-p-chlorobenzenesulfonamide sodium salt
30066-82-1

N-chloro-p-chlorobenzenesulfonamide sodium salt

A

CH3OSn(CH3)2S(NSO2C6H4Cl)Sn(CH3)2SSn(CH3)2NHSO2C6H4Cl
206008-10-8

CH3OSn(CH3)2S(NSO2C6H4Cl)Sn(CH3)2SSn(CH3)2NHSO2C6H4Cl

B

sulfur
7704-34-9

sulfur

C

sodium chloride
7647-14-5

sodium chloride

Conditions
ConditionsYield
In methanol soln. of N-compd. addn. to soln. of Sn compd. (vacuum, stirring), heating (50°C, 30 min); mixture cooling (ice bath), ppt. filtration off and extracting with water to remove NaCl and with acetone to remove S, alcoholic filtrate vacuumevapn., residue treating with diethyl ether, soln. decanting and vacuum evapn.; elem. anal.;A 92%
B 33%
C 98%
bis(tetraethylammonium)-bis[di-(thiophenolato)-(μ-sulfido)ferrate(III)]

bis(tetraethylammonium)-bis[di-(thiophenolato)-(μ-sulfido)ferrate(III)]

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

A

(NEt4)[Fe(NO)2(thiophenol)2(-2H)]
106709-47-1

(NEt4)[Fe(NO)2(thiophenol)2(-2H)]

B

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
In acetonitrile at 20℃; for 1.5h; Inert atmosphere; Schlenk technique;A 81%
B 98%
hydrogen sulfide
7783-06-4

hydrogen sulfide

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
With catalyst: bauxite; H2SO4, SO3, oleum or HSO3Cl In gas byproducts: H2O; two steps: 300°C and 200°C;97%
With catalyst: bauxite; H2SO4, SO3, oleum or HSO3Cl In neat (no solvent, gas phase) byproducts: H2O; two steps: 300°C and 200°C;97%
With oxygen at 180℃; for 30h; Catalytic behavior; Activation energy; Reagent/catalyst; Temperature; Flow reactor;95%
hydrgensulfide(1-)

hydrgensulfide(1-)

hydrogen cation

hydrogen cation

sulfite(2-)
14265-45-3

sulfite(2-)

hydrogen sulfite

hydrogen sulfite

A

water
7732-18-5

water

B

thiosulphate ion
14383-50-7

thiosulphate ion

C

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
In not given equimolar amts. of HSO3(1-) and SO3(2-);A n/a
B 96%
C 0%
In not given equimolar amts. of HSO3(1-) and SO3(2-);A n/a
B 96%
C 0%
sulfuryl dichloride
7791-25-5

sulfuryl dichloride

cadmium(II) sulphide

cadmium(II) sulphide

A

sulfur dioxide
7446-09-5

sulfur dioxide

B

sulfur
7704-34-9

sulfur

C

cadmium(II) chloride
10108-64-2

cadmium(II) chloride

Conditions
ConditionsYield
3-4 h at 350°C in a sealed bombe tube;A n/a
B n/a
C 95%
3-4 h at 350°C in a sealed bombe tube;A n/a
B n/a
C 95%
16 h at 250°C in a sealed bombe tube;A n/a
B n/a
C 94%
carbon monoxide
201230-82-2

carbon monoxide

sulfur dioxide
7446-09-5

sulfur dioxide

A

carbon oxide sulfide
463-58-1

carbon oxide sulfide

B

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
With catalyst: La2O3-TiO2 highest activity with 1:1 La:Ti ratio; 500°C, 1 atm, in the presence of N2;A <1
B 95%
With catalyst: Fe-Al2O3 byproducts: CO2; highest SO2 reduction with 40 % Fe in the catalyst, maximum COS yield at 400°C;
With catalyst: Cu-Al2O3 H2O vapour diminishes catalyst activity;
carbon monoxide
201230-82-2

carbon monoxide

sulfur dioxide
7446-09-5

sulfur dioxide

A

carbon dioxide
124-38-9

carbon dioxide

B

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
La-doped ceria above 550°C;A n/a
B 95%
cerium(IV) oxide catalyst exposition to SO2/CO/He mixt. at space velocity 10000 ml/(h*g catalyst) and temp. increase rate 10 K/min; gas chromy.;
Ca-doped cerium oxide catalyst exposition to SO2/CO/He mixt. at space velocity 10000 ml/(h*g catalyst) and temp. increase rate 10 K/min; gas chromy.;
chloroauric acid

chloroauric acid

Sodium thiosulfate pentahydrate

Sodium thiosulfate pentahydrate

A

gold(I) sulfide

gold(I) sulfide

B

Na3Au(thiosulfate)2*2water

Na3Au(thiosulfate)2*2water

C

gold (I) hydroxide

gold (I) hydroxide

D

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
With sodium hydroxide; nitric acid In water 0.1 mol H{AuCl4}; 40% NaOH soln.; excess of 0.4 mol Na2S2O3*5H2O; 4 m HNO3 soln.; stirring; filtration; dissolving in alc. and H2O; decompn. with alc.; evapn.; drying in vac. dessicator above H2SO4 in dark 1 d;A n/a
B 95%
C n/a
D n/a
With NaOH; HNO3 In water 0.1 mol H{AuCl4}; 40% NaOH soln.; excess of 0.4 mol Na2S2O3*5H2O; 4 m HNO3 soln.; stirring; filtration; dissolving in alc. and H2O; decompn. with alc.; evapn.; drying in vac. dessicator above H2SO4 in dark 1 d;A n/a
B 95%
C n/a
D n/a
manganese(II) sulfide

manganese(II) sulfide

ammonium tetrathionate

ammonium tetrathionate

A

ammonium thiosulfate

ammonium thiosulfate

B

manganese sulfite

manganese sulfite

C

manganese thiosulfate

manganese thiosulfate

D

hydrogen sulfide
7783-06-4

hydrogen sulfide

E

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
21 hours;A n/a
B n/a
C 95%
D n/a
E n/a
21 hours;A n/a
B n/a
C 95%
D n/a
E n/a
1/2 hours;A n/a
B n/a
C 56%
D n/a
E n/a
1/2 hours;A n/a
B n/a
C 56%
D n/a
E n/a
pyrite

pyrite

A

sulfur
7704-34-9

sulfur

B

iron(II) chloride

iron(II) chloride

Conditions
ConditionsYield
With chlorine at 600°C;A 94.7%
B n/a
With Cl2 at 600°C;A 94.7%
B n/a
sulfur dioxide
7446-09-5

sulfur dioxide

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
With pyrographite90%
With hydrogen sulfide In further solvent(s) in glycol with NaOOCCH2CH2COONa;82%
With hydrogen sulfide In further solvent(s) in glycol with p-H2NC6H4COOK;73%
hydrogen sulfide
7783-06-4

hydrogen sulfide

A

sulfur
7704-34-9

sulfur

B

sodium thiosulfate

sodium thiosulfate

Conditions
ConditionsYield
With phosphate buffer; oxygen In water Kinetics; byproducts: H2O; at pH=8.4-9.0, temp. 25°C, O2 pressure 101 kPa, H2S concn. (2.4-7.2)E-2 M; catalyst Co(II)phthalocyanine(SO3Na)4+MnCl2; not isolated, detd. by iodometry, lead indicator paper, spectrophotometry;A 90%
B n/a
With phosphate buffer; oxygen; cobalt(II) phthalocyaninetetrasulfonate sodium salt In water Kinetics; byproducts: H2O; at pH=8.0-10.2, temp. 25°C, O2 pressure 101 kPa, H2S concn. (2.4-7.2)E-2 M; not isolated, detd. by iodometry, lead indicator paper, spectrophotometry;A 60%
B 40%
With phosphate buffer; oxygen; sodium salt of cobalt disulfophthalocyanine In water Kinetics; byproducts: H2O; at pH=8.0-10.2, temp. 25°C, O2 pressure 101 kPa, H2S concn. (2.4-7.2)E-2 M; not isolated, detd. by iodometry, lead indicator paper, spectrophotometry;A 60%
B 40%
With phosphate buffer; oxygen; manganese(II) sulfate In water Kinetics; byproducts: H2O; at pH=11.3, temp. 25°C, O2 pressure 101 kPa, H2S concn. (2.4-7.2)E-2 M; not isolated, detd. by iodometry, lead indicator paper, spectrophotometry;
With phosphate buffer; oxygen In water Kinetics; byproducts: H2O; at pH=11.3-11.85, temp. 25°C, O2 pressure 101 kPa, H2S concn. (2.4-7.2)E-2 M; catalyst Co(II)phthalocyanine(SO3Na)4+MnSO4; not isolated, detd. by iodometry, lead indicator paper, spectrophotometry;
ammonium bisulfite

ammonium bisulfite

A

trithionate
15579-17-6

trithionate

B

Sulfate
14808-79-8

Sulfate

C

dithionate

dithionate

D

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
In water in concd. soln. in closed tube for 4 years by light;A <1
B 90%
C 0%
D n/a
sodium hydrogensulfite

sodium hydrogensulfite

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
selenium In not given 70-80°C for about 24 h;90%
In not given standing for a longtime;
potassium pentathionate In not given 70°C in closed pot;
selenium In not given 70-80°C for about 30 h;
In not given in closed tube at 100°C for 22 h or at 150°C for 7 h;0%
dimethoxy disulfide
28752-21-8

dimethoxy disulfide

A

iodine
7553-56-2

iodine

B

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
With hydrogenchloride byproducts: H2O, H2S, SO2; in presence of KI;A 90%
B n/a
With HCl byproducts: H2O, H2S, SO2; in presence of KI;A 90%
B n/a
bis(tetraethylammonium)-bis[di-(thiophenolato)-(μ-sulfido)ferrate(III)]

bis(tetraethylammonium)-bis[di-(thiophenolato)-(μ-sulfido)ferrate(III)]

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

A

(NEt4)[Fe(NO)2(thiophenol)2(-2H)]
106709-47-1

(NEt4)[Fe(NO)2(thiophenol)2(-2H)]

B

hydrogen sulfide
7783-06-4

hydrogen sulfide

C

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
With ethanethiol In acetonitrile at 20℃; for 1h; Reagent/catalyst; Inert atmosphere; Schlenk technique;A 83%
B 88%
C 6.8%
magnesium sulfate
7487-88-9

magnesium sulfate

A

magnesium oxide

magnesium oxide

B

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
With acetylene In neat (no solvent) redn. with acetylene in a stream of CO2 at 700°C;; MgO containes coal;;A n/a
B 87.5%
With benzene In neat (no solvent) redn. with benzene in a stream of CO2 at 700°C;; MgO containes coal;;A n/a
B 19.2%
tetrabutylammonium hexasulfide
85533-96-6

tetrabutylammonium hexasulfide

tetramethlyammonium chloride
75-57-0

tetramethlyammonium chloride

silver nitrate

silver nitrate

A

n{Ag(S5)(1-)}(Me4N(1+))
126032-36-8

n{Ag(S5)(1-)}(Me4N(1+))

B

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
In methanol; acetonitrile oxygen exclusion; treatment of (Bu4N)2S6 with MeCN and methanolic Me4NCl, addn. of AgNO3 in acetonitrile (stirring); cooling (-20°C, 24 h), sulphur removal, standing (room temp.) crystals collection, washing (MeCN), drying (vac.); elem. anal.;A 83%
B n/a
rongalite
149-44-0

rongalite

A

trithioformaldehyde
36069-03-1

trithioformaldehyde

B

sulfur dioxide
7446-09-5

sulfur dioxide

C

Sulfate
14808-79-8

Sulfate

D

sulphurous acid
7782-99-2

sulphurous acid

E

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
With hydrogenchloride In not given byproducts: H2O, polythionic acids; digesting with HCl-soln.;A n/a
B 82%
C 0%
D n/a
E 82%
With HCl In not given byproducts: H2O, polythionic acids; digesting with HCl-soln.;A n/a
B 82%
C 0%
D n/a
E 82%
sodium sulfide

sodium sulfide

sulphurous acid
7782-99-2

sulphurous acid

A

water
7732-18-5

water

B

sulfur
7704-34-9

sulfur

C

sodium thiosulfate

sodium thiosulfate

Conditions
ConditionsYield
In water pure SO2 is introduced into concd. Na2S soln. at 60°C;;A n/a
B n/a
C 80%
In water at 20°C, aq. SO2 soln., diluted Na2S soln.;
bismuth
7440-69-9

bismuth

sulfur
7704-34-9

sulfur

bismuth(III) sulfide

bismuth(III) sulfide

Conditions
ConditionsYield
In neat (no solvent) under dry N2 atm. in vac. glovebox; mixt. of Bi and S was transferred inquartz tube, with was flame sealed under vac.; tube was heated to 650.d egree.C for 48 h; stayed at 650°C for 2 ds; cooled to 50°Cin 10 h; ground into powder;100%
In melt by melting at possible min. temp.;
In melt addition of S to molten Bi at 600-700°C;; Bi content 1 - 2 %;;
antimony
7440-36-0

antimony

sulfur
7704-34-9

sulfur

antimony(III) sulfide

antimony(III) sulfide

Conditions
ConditionsYield
In melt melting of Sb and S at 450-500 °C gives complete reaction; slow cooling;;100%
heating;
mixt. fusing (evac. quartz ampoule); vac. sublimation;
sulfur
7704-34-9

sulfur

sodium nitrite
7632-00-0

sodium nitrite

sodium thiosulfate

sodium thiosulfate

Conditions
ConditionsYield
In N,N-dimethyl-formamide byproducts: N2O; at about 80°C, under N2 or CO2, cooling, separation of Na2S2O3;; washing with acetone, analytically pure;;100%
In further solvent(s) byproducts: N2O; solvent: dimethyl acetamide, at about 80°C, under N2 or CO2, cooling, separation of Na2S2O3;; washing with acetone, analytically pure;;100%
sulfur
7704-34-9

sulfur

phosphorus trichloride
7719-12-2, 52843-90-0

phosphorus trichloride

trichlorothiophosphine
3982-91-0

trichlorothiophosphine

Conditions
ConditionsYield
With disulfur dichloride; iron(III) chloride In neat (no solvent) addn. of a mixt. of 140 g PCl3 and 1.7 g S2Cl2 drop by drop to a hot mixt. of 160 g PSCl3, 2 g anhydrous FeCl3 and 38 g S on stirring and refluxing (4.5 h); refluxing for 1 h, distg. off PSCl3;;100%
In neat (no solvent) react. molten S with PCl3 at 124-126 °C at ambient pressure; use of a catalyst formed on melting S with active carbon and boiling in PSCl3 at 200 °C;;
disulfur dichloride In not given react. with S2Cl2 as catalyst;;
bis(perfluorophenyl) selenide
973-18-2

bis(perfluorophenyl) selenide

sulfur
7704-34-9

sulfur

pentafluorophenyl sulfide
1043-50-1

pentafluorophenyl sulfide

Conditions
ConditionsYield
at 230°C;100%
at 230°C;100%
bismuth
7440-69-9

bismuth

potassium
7440-09-7

potassium

sulfur
7704-34-9

sulfur

potassium metathiobismuthite

potassium metathiobismuthite

Conditions
ConditionsYield
In neat (no solvent)100%
differential thermal anal.;100%
bromine
7726-95-6

bromine

sulfur
7704-34-9

sulfur

molybdenum
7439-98-7

molybdenum

Mo3(12+)*S(2-)*3S2(2-)*4Br(1-)=Mo3S7Br4

Mo3(12+)*S(2-)*3S2(2-)*4Br(1-)=Mo3S7Br4

Conditions
ConditionsYield
In neat (no solvent) reactants placing into Mo-glass ampule, cooling (liquid N2), evacuation,sealing, gradual increasing temperature and heating (280°C, 14 h ; 400°C, 40 h), cooling, excess Br2 removing; remaining solid washing (CHCl3), vacuum drying (50°C, 6 h); elem.anal.;100%
chromium chloride hexahydrate

chromium chloride hexahydrate

tetraphenylphosphonium bromide
2751-90-8

tetraphenylphosphonium bromide

sulfur
7704-34-9

sulfur

ethylenediamine
107-15-3

ethylenediamine

[(C6H5)4P](1+)*[Cr(NH2CH2CH2NH2)(S5)2](1-)=[(C6H5)4P][Cr(NH2CH2CH2NH2)(S5)2]
236386-04-2

[(C6H5)4P](1+)*[Cr(NH2CH2CH2NH2)(S5)2](1-)=[(C6H5)4P][Cr(NH2CH2CH2NH2)(S5)2]

Conditions
ConditionsYield
In water stoichiometric amts., 10% en in H2O, heating (398 K, 7 d);100%
nickel
7440-02-0

nickel

sulfur
7704-34-9

sulfur

1,2-diaminopropan
78-90-0, 10424-38-1

1,2-diaminopropan

[Ni(1,2-diaminopropane)3]2Sn2S6*2H2O

[Ni(1,2-diaminopropane)3]2Sn2S6*2H2O

Conditions
ConditionsYield
In further solvent(s) High Pressure; prepd. under solvothermal conditions; reactants weighted in ratio of 1 Ni:1 Sn:3 S, heated in sealed Teflon-lined steel autoclave in pure 1,2-diaminopropane for 7 d at 140°C; elem. anal.;100%
2-phenyl-4,5-[1,2(1,2-dicarba-closo-dodecaborano)]-1,3-diselena-2-phospha-cyclopentane
1017605-86-5

2-phenyl-4,5-[1,2(1,2-dicarba-closo-dodecaborano)]-1,3-diselena-2-phospha-cyclopentane

sulfur
7704-34-9

sulfur

2-phenyl-2-thio-4,5-[1,2(1,2-dicarba-closo-dodecaborano)]-1,3-diselena-2-λ5-phospha-cyclopentane
1017605-87-6

2-phenyl-2-thio-4,5-[1,2(1,2-dicarba-closo-dodecaborano)]-1,3-diselena-2-λ5-phospha-cyclopentane

Conditions
ConditionsYield
In dichloromethane-d2 S added to B-compound in CD2Cl2; mixt. stirred overnight; crystallized from CH2Cl2 at room temp.;100%
bis[1,3-dihydro-1-methyl-3-(1-methylethyl)-2H-imidazol-2-ylidene]iodocopper

bis[1,3-dihydro-1-methyl-3-(1-methylethyl)-2H-imidazol-2-ylidene]iodocopper

sulfur
7704-34-9

sulfur

1,3-dihydro-1-methyl-3-(1-methylethyl)-2H-imidazol-2-thione
61640-29-7

1,3-dihydro-1-methyl-3-(1-methylethyl)-2H-imidazol-2-thione

Conditions
ConditionsYield
In chloroform at 20℃; for 4h; Inert atmosphere;100%
bis(1-[2,6-bis(1-methylethyl)phenyl]-1,3-dihydro-3-methyl-2-H-imidazol-2-ylidene)copper(1+) hexafluorophosphate(1-) (1:1)

bis(1-[2,6-bis(1-methylethyl)phenyl]-1,3-dihydro-3-methyl-2-H-imidazol-2-ylidene)copper(1+) hexafluorophosphate(1-) (1:1)

sulfur
7704-34-9

sulfur

1,3-dihydro-1-[2,6-bis(1-methylethyl)phenyl]-3-methyl-2H-imidazol-2.thione
1184635-07-1

1,3-dihydro-1-[2,6-bis(1-methylethyl)phenyl]-3-methyl-2H-imidazol-2.thione

Conditions
ConditionsYield
In chloroform at 20℃; for 16h; Inert atmosphere;100%
lanthanum(III) oxide

lanthanum(III) oxide

tungsten(VI) oxide

tungsten(VI) oxide

cobalt
7440-48-4

cobalt

sulfur
7704-34-9

sulfur

tungsten
7440-33-7

tungsten

La3CoS3(6+)*WO6(6-)=La3CoWS3O6

La3CoS3(6+)*WO6(6-)=La3CoWS3O6

Conditions
ConditionsYield
In melt stoich. amts. of La2O3, S, W, WO3, Co mixed with KCl flux; sealed in carbon coated SiO2 ampoule under vac.; heated from 200 to 400°C in 24 h; held for 48 h; heated to 950°C in 12 h; held for 120 h; cooled to room temp. within 24 h; soaked in H2O overnight; washed with H2O; detn. by EDX, XRD;100%
tellurium

tellurium

cesium azide
22750-57-8

cesium azide

sulfur
7704-34-9

sulfur

cesium thiotellurate(II)

cesium thiotellurate(II)

Conditions
ConditionsYield
In neat (no solvent) at 500℃; for 96h;100%
tellurium

tellurium

cesium azide
22750-57-8

cesium azide

sulfur
7704-34-9

sulfur

cesium thiotellurate(IV)

cesium thiotellurate(IV)

Conditions
ConditionsYield
In neat (no solvent) at 500℃; for 96h;100%
sodium sulfide

sodium sulfide

uranium

uranium

tetraphosphorus decasulfide
15857-57-5

tetraphosphorus decasulfide

sulfur
7704-34-9

sulfur

P2S7(4-)*U(4+)

P2S7(4-)*U(4+)

Conditions
ConditionsYield
In neat (no solvent) at 130 - 700℃; for 348h; Sealed tube;100%
uranium

uranium

tetraphosphorus decasulfide
15857-57-5

tetraphosphorus decasulfide

sulfur
7704-34-9

sulfur

P2S6(4-)*U(4+)

P2S6(4-)*U(4+)

Conditions
ConditionsYield
In neat (no solvent) at 130 - 700℃; for 348h; Sealed tube;100%
uranium

uranium

tetraphosphorus decasulfide
15857-57-5

tetraphosphorus decasulfide

sulfur
7704-34-9

sulfur

P2S7(4-)*U(4+)

P2S7(4-)*U(4+)

Conditions
ConditionsYield
In neat (no solvent) at 130 - 700℃; for 348h; Sealed tube;100%
C33H38GeN2OSeSi

C33H38GeN2OSeSi

sulfur
7704-34-9

sulfur

C33H38GeN2OSSi

C33H38GeN2OSSi

Conditions
ConditionsYield
In tetrahydrofuran at 20℃; for 10h;100%
C33H38GeN2OSi

C33H38GeN2OSi

sulfur
7704-34-9

sulfur

C33H38GeN2OSSi

C33H38GeN2OSSi

Conditions
ConditionsYield
In tetrahydrofuran at 20℃; for 2h;100%
bismuth
7440-69-9

bismuth

lithium sulfide

lithium sulfide

sulfur
7704-34-9

sulfur

Li0.97Sn2.06Bi4.97S10

Li0.97Sn2.06Bi4.97S10

Conditions
ConditionsYield
Stage #1: bismuth; tin; lithium sulfide; sulfur at 800℃; under 0.00150015 Torr; for 10h; Inert atmosphere; Glovebox; Sealed tube;
Stage #2: at 800℃; for 26h;
100%
yttrium(III) oxysulfide

yttrium(III) oxysulfide

terbium dioxosulfide

terbium dioxosulfide

sulfur
7704-34-9

sulfur

silicon
7440-21-3

silicon

(Y0.98Tb0.02)4S3(Si2O7)

(Y0.98Tb0.02)4S3(Si2O7)

Conditions
ConditionsYield
With cesium chloride at 1100℃; for 12h; Milling; Sealed tube;100%
yttrium(III) oxysulfide

yttrium(III) oxysulfide

terbium dioxosulfide

terbium dioxosulfide

sulfur
7704-34-9

sulfur

silicon
7440-21-3

silicon

(Y0.96Tb0.04)4S3(Si2O7)

(Y0.96Tb0.04)4S3(Si2O7)

Conditions
ConditionsYield
With cesium chloride at 1100℃; for 12h; Milling; Sealed tube;100%
yttrium(III) oxysulfide

yttrium(III) oxysulfide

europium oxysulfide

europium oxysulfide

sulfur
7704-34-9

sulfur

silicon
7440-21-3

silicon

(Y0.99Eu0.01)4S3(Si2O7)

(Y0.99Eu0.01)4S3(Si2O7)

Conditions
ConditionsYield
With cesium chloride at 1100℃; for 12h; Milling; Sealed tube;100%

7704-34-9Relevant articles and documents

Steele, B. D.,Bagster, L. S.

, p. 2607 (1910)

EFFECT OF PREADSORBED SULFUR ON NITRIC OXIDE REDUCTION ON POROUS PLATINUM BLACK ELECTRODES.

Foral,Langer

, p. 257 - 263 (1988)

Sulfur can be deposited on porous platinum black gas diffusion cathodes to influence the course of the electrogenerative reduction of nitric oxide. Polarization (performance) curves and reactor selectivity data are compared for untreated cathodes and thos

Donath, E.

, p. 141 - 143 (1901)

Kinetic regularities of recovery of metals from raw materials of industrial origin

Velikanova,Semchenko,Khentov

, p. 1470 - 1475 (2011)

Kinetics of recovery of metals from the wastes and poor ores, which contain oxide and sulfide minerals of copper, vanadium, and silver with an azomethine solution in organic solvent was studied. The optimal parameters of the recovery were suggested.

The Dissociation Rate of S2 Produced from COS Pyrolysis

Higashihara, Tetsuo,Saito, Ko,Murakami, Ichiro

, p. 15 - 18 (1980)

The disappearance rate of S2, which was produced from the pyrolysis of COS, was measured behind incident shock waves by monitoring the UV emission in the temperature range of 4500-6000 K and in the pressure range of 0.32-0.5 atm.It was found that two proc

Infrared studies of the adsorption and surface reactions of hydrogen sulfide and sulfur dioxide on some aluminas and zeolites

Deo,Lana, I.G.Dalla,Habgood

, p. 270 - 281 (1971)

Adsorption of hydrogen sulfide, sulfur dioxide, and their mixtures on four different catalysts has been studied by infrared spectroscopy of the catalyst surfaces. The four catalysts, which show a wide range of acidity and are all active for the Claus reaction (2H2S + SO2 → 3S + 2H2O), were γ-alumina (the main constituent of commercial bauxite catalysts), γ-alumina doped with NaOH, sodium Y zeolite, and hydrogen Y zeolite. All catalysts showed physical adsorption of both reactants with strong hydrogen bonding to surface OH groups. This would suggest that the role of the catalyst is primarily to bring the reactants together in suitable orientation. On the other hand, γ-alumina shows, on heating with SO2, a chemisorbed SO2 species which may be a reaction intermediate. The NaOH-treated γ-alumina shows a second chemisorbed SO2 species which is irreversibly adsorbed and thus may be a catalyst poison.

Wright, L. T.

, p. 156 - 156 (1883)

Matthews, E.

, (1926)

Dunnicliff, H. B.,Nijhawan, S. D.

, (1926)

Use of cobalt(II) phthalocyanine sulfonates in gas purification to remove hydrogen sulfide

Faddeenkova,Kundo

, p. 1946 - 1950 (2003)

Experiments on liquid-phase oxidation of H2S with oxygen in the presence of catalysts, cobalt phthalocyanine sulfonates [CoPc(SO 3Na)n], were performed on a laboratory static installation in order to find conditions under which a stationary oxidation mode can be established at pH ≥ 8. The influence exerted by additional introduction of a soluble salt of Mn2+ (MnSO4, MnCl2) into the reaction mixture at various pH values was studied.

Carter, S. R.,Butler, J. A. V.

, p. 2370 - 2370 (1923)

Carter, S. R.,Butler, J. A. V.

, p. 2380 - 2380 (1923)

Wardlaw, W.,Carter, S. R.,Clews, F. H.

, p. 1241 - 1241 (1920)

Sato, Tetsuya,Kinugawa, Tohru,Arikwawa, Tatsuo,Kawasaki, Masahiro

, p. 173 - 182 (1992)

Corrosion mechanism of nickel in hot, concentrated H2SO4

Kish,Ives,Rodda

, p. 3637 - 3646 (2000)

Electrochemical techniques, complemented by weight change and ex situ X-ray spectroscopic measurements, were employed to characterize the corrosion of nickel in concentrated H2SO4 solutions. By use of a rotating cylinder electrode, it was found that corrosion is a mass-transport controlled process with the convective diffusion of nickel cations from a saturated NiSO4 layer as its rate-determining step. The oxidizing nature of the acid solution leads to the formation of additional corrosion products including metastable NiS, and elemental sulfur along with NiSO4, none of which is protective. When present on the surface, NiS establishes a galvanic interaction with the uncovered metal, significantly polarizing the anodic metal dissolution reaction. Since corrosion is mass-transport controlled, the resultant corrosion rate of the metal is unaffected during the galvanic-induced polarization.

The synthesis and characterization of Pb5S2I6 whiskers and tubules

Yang, Qing,Tang, Kaibin,Wang, Chunrui,Zuo, Jian,Qian, Yitai

, p. 670 - 674 (2003)

Pb5S2I6 whiskers and tubules were synthesized from the reaction among lead chloride, thiourea, and excess sodium iodide under hydrothermal conditions at 200 °C for 20-40 h. XRD, SEM, XPS, ICP-AES, and TEM characterized the final products. Most products are whiskers with structure of 3-4 mm in length, 0.5-2.0 μm in diameter for a singular one. Meanwhile, about 10% tubules are produced in the process. The tubules are 3-6 mm in length, 8-20 μm in diameter, and 1-3 μm in thickness. Nanowhiskers were also produced in the route at 180-200 °C for 8-10 h. Raman spectra show that the Pb5S2I6 crystals have complex vibrational modes of PbS and PbI2.

Iwasawa, Y.,Ogasawara, S.

, p. 132 - 142 (1977)

A facile in situ sulfur deposition route to obtain carbon-wrapped sulfur composite cathodes for lithium-sulfur batteries

Su, Yu-Sheng,Manthiram, Arumugam

, p. 272 - 278 (2012)

An in situ sulfur deposition route has been developed for synthesizing sulfur-carbon composites as cathode materials for lithium-sulfur batteries. This facile synthesis method involves the precipitation of elemental sulfur at the interspaces between carbon nanoparticles in aqueous solution at room temperature. The product has been characterized by X-ray diffraction, scanning electron microscopy, transmission electron microscopy, charge-discharge measurements, and electrochemical impedance spectroscopy. The sulfur-carbon composite cathode with 75 wt.% active material thus obtained exhibits a remarkably high first discharge capacity of 1116 mAh g-1 with good cycle performance, maintaining 777 mAh g-1 after 50 cycles. The significantly improved electrochemical performance of the sulfur-carbon composite cathode is attributed to the carbon-wrapped sulfur network structure, which suppresses the loss of active material during charging/discharging and the migration of the polysulfide ions to the anode (i.e., shuttling effect). The integrity of the cathode structure during cycling is reflected in low impedance values observed after cycling. This facile in situ sulfur deposition route represents a low-cost approach to obtain high-performance sulfur-carbon composite cathodes for rechargeable Li-S batteries.

Thermodynamics of copper sulfides. II. Heat capacity and thermodynamic properties of synthetic covellite, CuS, from 5 to 780.5 K. Enthalpy of decomposition

Westrum, Edgar F.,Stoelen, Svein,Groenvold, Fredrik

, p. 1199 - 1208 (1987)

The heat capacity of CuS has been measured by adiabatic shield calorimetry from 5 to 840 K.The heat capacity increases regularly up to about 750 K and then more strongly as the decomposition temperature (780.5 K) of covellite into high-digenite and sulfur is approached.The molar enthalpy and molar entropy of decomposition are 2149.3R*K and 2.755R.Above 780.5 K the uptake of sulfur in the high-digenite causes a further rise in the heat capacity.The low-temperature values increase more strongly than expected from the Debye relation with a Debye temperature estimated from the intermediate-temperature behavior.This phenomenon as well as a small bump in the heat capacity around 55 K are discussed.The resulting molar enthalpy and molar entropy at 298.15 and 825 K are 1136.6R*K, 8.101R, and 6744.2R*K, 17.393R, respectively.

A Novel Reaction of Metal Sulphides with the Mixed Non-aqueous System Dimethyl Sulphoxide-Sulphur Dioxide

Harrison, W. David,Gill, J. Bernard,Goodall, David C.

, p. 728 - 729 (1988)

Several synthetic and naturally occuring metal sulphides react with the system dimethyl sulphoxide-sulphur dioxide to give metal hydrogen sulphates or sulphates, in contrast with the reaction of sulphides with aqueous sulphur dioxide, which yields mainly thiosulphate.

Bellissent, R.,Descotes, L.,Boue, F.

, (1990)

Gibbs, W.

, p. 387 - 402 (1864)

Murthy, A. R. V.

, p. 388 - 401 (1952)

Structural determination of the S-passivated InP(100)-(1x1) surface by dynamical low-energy electron-diffraction analysis

Warren, O. L.,Anderson, G. W.,Hanf, M. C.,Griffiths, K.,Norton, P. R.

, (1995)

We have determined the optimum geometry of the S-passivated InP(100)-(1x1) surface by dynamical low-energy electron-diffraction analysis. S atoms bond to In by occupying the bridge site that continues the zinc-blendestacking sequence of the substrate. Oth

Skrabal

, p. 107 - 107 (1924)

High temperature H2S selective oxidation on a copper-substituted hexaaluminate catalyst: A facile process for treating low concentration acid gas

Hao, Zhengping,Jiang, Guoxia,Li, Ganggang,Xu, Xin,Zhang, Fenglian

supporting information, (2021/09/22)

H2S selective catalytic oxidation technology is a prospective way for the treatment of low concentration acid gas with simple process operation and low investment. However, undesirable results such as large formation of SO2 and catalyst deactivation inevitably occur, due to the temperature rise of fixed reaction bed caused by the exothermic reaction. Catalyst with high activity in wide operating temperature window, especially in high temperature range, is urgently needed. In this paper, a series of copper-substituted hexaaluminate catalysts (LaCux, x = 0, 0.5, 1, 1.5, 2, 2.5) were prepared and investigated for the H2S selective oxidation reaction at high temperature conditions (300-550°C). The LaCu1 catalyst exhibited excellent catalytic performance and great stability, which was attributed to the best reductive properties and proper pore structure. Besides, two facile deep processing paths were proposed to eliminate the remaining H2S and SO2 in the tail gas.

Synergistic effect of Bi-doped exfoliated MoS2 nanosheets on their bactericidal and dye degradation potential

Qumar,Ikram,Imran,Haider,Ul-Hamid,Haider,Riaz,Ali

, p. 5362 - 5377 (2020/05/08)

Nanosheets incorporated with biological reducing agents are widely used to minimize the toxic effects of chemicals. Biologically amalgamated metal oxide nanomaterials have crucial importance in nanotechnology. In this study, bare and bismuth (Bi)-doped molybdenum disulfide (MoS2) nanosheets were synthesized via a hydrothermal method. Different Bi weight ratios of 2.5, 5, 7.5 and 10% were incorporated in a fixed amount of MoS2 to evaluate its catalytic and antimicrobial activities. Doped nanosheets were characterized using XRD, FTIR and UV-vis spectroscopy, FESEM, HRTEM, Raman, PL, DSC/TGA, EDX, XRF and XPS analysis. The XRD spectra confirmed that the doped nanosheets exhibit a hexagonal structure and their crystallite size increases gradually upon doping. The morphology and interlayer d-spacing of doped MoS2 were determined by FESEM and HRTEM. The presence of functional groups in the doped nanosheets was confirmed using FTIR, PL and Raman analysis. The absorption intensity increased and the corresponding measured band gap energy decreased with doping. The thermal stability and weight loss behaviour of the prepared samples were studied using DSC/TGA. The doped MoS2 nanosheets showed a higher catalytic potential compared to undoped MoS2. The doped Bi nanosheets exhibited higher antimicrobial activity against Gram-positive Staphylococcus aureus (S. aureus) and Gram-negative Escherichia coli (E. coli) at different concentrations of Bi (0.075 and 0.1), showing a tendency to counter the emerging drug resistance against pathogenic bacterial diseases. Consequently, significant inhibition zones were recorded against (MDR) S. aureus ranging from 2.25 to 3.3 mm and 3.25 to 5.05 mm at low and high concentrations of doped-Bi nanosheets and against Gram-negative E. coli ranging from 1 to 1.45 mm at high concentrations. In conclusion, the Bi-doped MoS2 nanocomposite has exhibited significant potential for use in industrial dye degradation applications. Its antibacterial properties can also mitigate health risks associated with the presence of several well-known pathogens in the environment.

Physicochemical studies on the desulfurization process of organosulfur compounds occur in crude oil by metallo-complexation method

Alhadhrami,Al-Ghamry, Mosad A.,Atta, Aly H.,El-Shenawy, Ahmed I.,Refat, Moamen S.,Al-Omar, Mohamed A.,Naglah, Ahmed M.

, p. 94 - 97 (2017/02/13)

All over the world researchers in accelerating to development the new and modern methods of desulfurization process to overcome the presence of residual sulfur compounds in the crude oil, which has harmful effects and undesirable. Out of these important r