June 24th ┊ 🦈 Shark Tank’s Kevin O’Leary is Bullish on This

If you have ever watched Shark Tank, you know Kevin O’Leary (Mr. Wоnderful) is very protective of his moneу. [Grand Event]( Having Troubles Viewing? [Check it Online]( - June 24, 2023 - [Visit Our Website]( [Business team]( Hi Trader, If you have ever watched Shark Tank, you know Kevin O’Leary (Mr. Wоnderful) is very protective of his moneу. In fact, he expects to multiply his investments by at least 10x when he gets in... The company I discusses in this video is exactly what Mr. Wоnderful looks for. In fact, not onlу did Kevin O’Leary invest his monеy in it… [he also put his own personal team to work in the company.]( That’s how excited he is about this oppоrtunity. And I'm calling this oppоrtunity part of “the greatest wealth transfer in history.” To learn more, clіck hеre nоw to watch this video. Sincerely, Bryan Perry Editor, Micro-Cap Stock Trader P.S. I personally interviewed Mr. Wondеrful, the CEO of this organization and key members of the team. After our discussion, I walked away more convinced than ever that this company is one of the bеst ways to stake a claim in this megatrend. [Cliсk hеre nоw to watch Kevin O’Leary and I discuss this oppоrtunity.]( [Clіck Video]( ur (also spelled sulphur in British English) is a chemical element with the symbol S and atomic number 16. It is abundant, multivalent and nonmetallic. Under normal conditions, sulfur atoms fom cyclic octatomic molecules with a chemical formula S8. Elemental sulfur is a bright yellow, crystalline solid at room temperature. Sulfur is the tenth most abundant element by mass in the universe and the fifth most on Earth. Though sometimes found in pure, native fom, sulfur on Earth usually occurs as sulfide and sulfate minerals. Being abundant in native frm, sulfur was known in ancient times, being mentioned for its uses in ancient India, ancient Greece, China, and ancient Egypt. Historically and in literature sulfur is also called brimstone,[5] which means "burning stone".[6] Tday, almost ll elemental sulfur is produced as a byproduct of removing sulfur-containing contaminants from natural gas and petroleum.[7][8] The greatest commercial use of the element is the production of sulfuric acid for sulfate and phosphate fertilizers, and other chemical processes. Sulfur is used in matches, insecticides, and fungicides. Many sulfur compounds are odoriferous, and the smells of odorized natural gas, skunk scent, grapefruit, and garlic are due to organosulfur compounds. Hydrogen sulfide gives the characteristic odor to rotting eggs and other biological processes. Sulfur is an essential element for ll lfe, but almost always in the frm of organosulfur compounds or metal sulfides. Amino acids (two proteinogenic: cysteine and methionine, and many other non-coded: cystine, taurine, etc.) and two vitamins (biotin and thiamine) are organosulfur compounds crucial for ife. Many cofactors also contain sulfur, including glutathione, and iron–sulfur proteins. Disulfides, S–S bonds, confer mechanical strength and insolubility of the (among others) protein keratin, found in outer skin, hair, and feathers. Sulfur is one of the core chemical elements needed for biochemical functioning and is an elemental macronutrient for al living organisms. Characteristics As a solid, sulfur is a characteristic lemon yellow; when burned, sulfur melts into a blood-red liquid and emits a blue flame. Physical properties Sulfur forms several polyatomic molecules. The est-known allotrope is octasulfur, cyclo-S8. The point group of cyclo-S8 is D4d and its dipole moment is 0 D.[9] Octasulfur is a soft, bright-yellow solid that is odorless, but impure samples have an odor similar to that of matches.[10] It melts at 115.21 °C (239.38 °F), boils at 444.6 °C (832.3 °F)[5] and sublimes more or less between 20 °C (68 °F) and 50 °C (122 °F).[11] At 95.2 °C (203.4 °F), below its melting temperature, cyclo-octasulfur changes from α-octasulfur to the β-polymorph.[12] The structure of the S8 ring is virtually unchanged by this phase change, which affects the intermolecular interactions. Between its melting and boiling temperatures, octasulfur changes its allotrope again, turning from β-octasulfur to γ-sulfur, again accompanied by a lower density but increased viscosity due to the formation of polymers.[12] At higher temperatures, the viscosity decreases as depolymerization occurs. Molten sulfur assumes a dark red color above 20. The density of sulfur is about 2 g/cm3, depending on the allotrope; ll of the stable allotropes are excellent electrical insulators. Sulfur is insoluble in water but soluble in carbon disulfide and, to a lesser extent, in other nonpolar organic solvents, such as benzene and toluene. Chemical properties Under normal conditions, sulfur hydrolyzes very slowly to mainly fom hydrogen sulfide and sulfuric acid: 4 The reaction involves adsorption of protons onto S 8 clusters, followed by disproportionation into the reaction products.[13] The second, fourth and sixth ionization energies of sulfur are 2252 kJ/mol−1, 4556 kJ/mol−1 and 8495.8 kJ/mol−1,respectively. A composition of products of sulfur's reactions with oxidants (and its oxidation state) depends on that whether releasing out of a reaction energy overcomes these thresholds. Applying catalysts and / or supply of outer energy may vary sulfur's oxidation state and a composition of reaction products. While reaction between sulfur and oxygen at normal conditions gives sulfur dioxide (oxidation state +4), formation of sulfur trioxide (oxidation state +6) requires temperature 400 – 600 °C and presence of a catalyst. In reactions with elements of lesser electronegativity, it reacts as an oxidant and forms sulfides, where it has oxidation state –2. Sulfur reacts with nearly ll other elements with the exception of the noble gases, even with the notoriously unreactive metal iridium (yielding iridium disulfide).[14] Some of those reactions need elevated temperatures.[15] Allotropes Main article: Allotropes of sulfur The structure of the cyclooctasulfur molecule, S8 Sulfur forms over 30 solid allotropes, more than any other element.[16] Besides S8, several other rings are known.[17] Removing one atom from the crown gives S7, which is more of a deep yellow than the S8. HPLC analysis of "elemental sulfur" reveals an equilibrium mixture of mainly S8, but with S7 and small amounts of S6.[18] Larger rings have been prepared, including S12 and S18.[19][20] Amorphous or "plastic" sulfur is produced by rapid cooling of molten sulfur—for example, by pouring it into cold water. X-ray crystallography studies show that the amorphous fom may have a helical structure with eight atoms per turn. The long coiled polymeric molecules make the brownish substance elastic, and in bulk this frm has the feel of crude rubber. This fom is metastable at room temperature and gradually reverts to crystalline molecular allotrope, which is no longer elastic. This process happens within a matter of hours to days, but can be rapidly catalyzed. Isotopes Main article: Isotopes of sulfur This section needs additional citations for verification. Pease help improve this article by adding citations to reliable sources in this section. Unsourced material may be challenged and removed. (February 2022) (Learn how and when to reme of 87 days, the radioactive isotopes of sulfur have half-lives less than 3 hours. The preponderance of sulfur-32 is explained by its production in the so-called alpha-process (one of the main classes of nuclear fusion reactions) in exploding stars. Other stable sulfur isotopes are produced in the bypass processes related with argon-34, and their composition depends on a type of a stellar explosion. For example, there is more sulfur-33 come from novae, than from supernovae.[23] On the planet Earth the sulfur isotopic composition was determined by the Sun. Though it is assumed that the distribution of different sulfur isotopes should be more of less equal, it has been found that proportions of two most abundant sulfur isotopes sulfur-32 and sulfur-34 varies in different samples. Assaying of these isotopes ratio (δ34S) in the samples allows to make suggestions about their chemical history, and with support of other methods, it allows to age-date the samples, estimate temperature of equilibrium between ore and water, determine pH and oxygen fugacity, identify the activity of sulfate-reducing bacteria in the time of formation of the sampe, or suggest the main sources of sulfur in ecosystems.[24] However, discussions about what is the real reason of the δ34S shifts, biological activity or postdeposital alteration, go on.[25] For example, when sulfide minerals are precipitated, isotopic equilibration among solids and liquid may cause small differences in the δ34S values of co-genetic minerals. The differences between minerals can be used to estimate the temperature of equilibration. The δ13C and δ34S of coexisting carbonate minerals and sulfides can be used to determine the pH and oxygen fugacity of the ore-bearing fluid during ore formation. Scientists measure the sulfur isotopes of minerals in rocks and sediments to study the redox conditions in the oceans in the past. Sulfate-reducing bacteria in marine sediment fractionate sulfur isotopes as they take in sulfate and produce sulfide. Prior to 2010s, it was thought that sulfate reduction could fractionate sulfur isotopes up to 46 permil[26] and fractionation larger than 46 permil recorded in sediments must be due to disproportionation of sulfur compounds in the sediment. This view has changed since the 2010s as experiments show that sulfate-reducing bacteria can fractionation to 66 permil.[27] As substrates for disproportionation are liited by the product of sulfate reduction, the isotopic effect of disproportionation should be less than 16 permil in most sedimentary settings.[28] In most forest ecosystems, sulfate is derived mostly from the atmosphere; weathering of ore minerals and evaporites contribute some sulfur. Sulfur with a distinctive isotopic composition has been used to identify pollution sources, and enriched sulfur has been added as a tracer in hydrologic studies. Differences in the natural abundances can be used in systems where there is sufficient variation in the 34S of ecosystem components. Rocky Mountain lakes thought to be dominated by atmospheric sources of sulfate have been found to have characteristic 34S values from lakes believed to be dominated by watershed sources of sulfate. The radioactive sulfur-35 is formed in cosmic ray spallation of the atmospheric 40Ar. This fact may be used for proving the presence of recent (not more than 1 year) atmospheric sediments in various things. This isotope may be obtained artificially by different ways. In practice, the reaction 35Cl + n → 35S + p is used by irradiating potassium chloride with neutrons.[29] The isotope sulfur-35 is used in various sulfur-containing compounds as a radioactive tracer for many biological studies, for example, the Hershey-Chase experiment. Because of its weak beta activity, S-35 compounds are relatively safe as long as they are not ingested or absorbed by the body.[30] Natural occurrence Sulfur vat from which railroad cars are loaded, Freeport Sulphur Co., Hoskins Mound, Texas (1943) Most of the yellow and orange hues of Io are due to elemental sulfur and sulfur compounds deposited by active volcanoes. Sulfur extraction, East Java A man carrying sulfur blocks from Kawah Ijen, a volcano in East Java, Indonesia, 2009 32S is created inside massive stars, at a depth where the temperature exceeds 2.5×109 K, by the fusion of one nucleus of silicon plus one nucleus of helium.[31] As this nuclear reaction is part of the alpha process that produces elements in abundance, sulfur is the 10th most common element in the universe. Sulfur, usually as sulfide, is present in many types of meteorites. Ordinary chondrites contain on average 2.1 sulfur, and carbonaceous chondrites may contain as much as 6.. It is normally present as troilite (FeS), but there are exceptions, with carbonaceous chondrites containing fre sulfur, sulfates and other sulfur compounds.[32] The distinctive colors of Jupiter's volcanic moon Io are attributed to various forms of molten, solid, and gaseous sulfur.[33] It is the fifth most common element by mass in the Earth. Elemental sulfur can be found near hot springs and volcanic regions in many parts of the world, especially along the Pacific Ring of Fire; such volcanic deposits are currently mined in Indonesia, Chile, and Japan. These deposits are polycrystalline, with the largest documented single crystal measuring 22×16×11 cm.[34] Historically, Sicily was a major source of sulfur in the Industrial Revolution.[35] Lakes of molten sulfur up to ~200 m in diameter have been found on the sea floor, associated with submarine volcanoes, at depths where the boiling point of water is higher than the melting point of sulfur.[36] Native sulfur is synthesised by anaerobic bacteria acting on sulfate minerals such as gypsum in salt domes.[37][38] Significant deposits in salt domes occur along the coast of the Gulf of Mexico, and in evaporites in eastern Europe and western Asia. Native sulfur may be produced by geological processes alone. Fossil-based sulfur deposits from salt domes were once the basis for commercial production in the United States, Russia, Turkmenistan, and Ukraine.[39] Currently, commercial production is still carried out in the Osiek mine in Poland. Such sources are nw of secondary commercial importance, and most are no longer worked. Common naturally occurring sulfur compounds include the sulfide minerals, such as pyrite (iron sulfide), cinnabar (mercury sulfide), galena (lead sulfide), sphalerite (zinc sulfide), and stibnite (antimony sulfide); and the sulfate minerals, such as gypsum (calcium sulfate), alunite (potassium aluminium sulfate), and barite (barium sulfate). On Earth, just as upon Jupiter's moon Io, elemental sulfur occurs naturally in volcanic emissions, including emissions from hydrothermal vents. The main industrial source of sulfur is no petroleum and natural gas.[7] Compounds Main article: Sulfur compounds Common oxidation states of sulfur range from −2 to +6. Sulfur forms stable compounds with ll elements except the noble gases. Electron transfer reactions Lapis lazuli owes its blue color to a trisulfur radical anion (S− 3) Sulfur polycations, S82+, S42+ and S162+ are produced when sulfur is reacted with oxidising agents in a strongly acidic soluion.[40] The colored solutions produced by dissolving sulfur in oleum were first reported as early as 1804 by C.F. Bucholz, but the cause of the color and the structure of the polycations involved was oly determined in the late 1960s. S82+ is deep blue, S42+ is yellow and S162+ is red.[12] Reduction of sulfur gives various polysulfides with the formula Sx2-, many of which have been obtained crystalline frm. Illustrative is the production of sodium tetrasulfide: 4 Na + S8 → 2 Na2S4 Some of these dianions dissociate to give radical anions, such as S3− gives the blue color of the rock lapis lazuli. Two parallel sulfur chains grown inside a single-wall carbon nanotube (CNT, a). Zig-zag (b) and straight (c) S chains inside double-wall CNTs[41] This reaction highlights a distinctive property of sulfur: its ability to catenate (bind to itself by formation of chains). Protonation of these polysulfide anions produces the polysulfanes, H2Sx where x= 2, 3, and 4.[42] Ultimately, reduction of sulfur produces sulfide salts: 16 Na + S8 → 8 Na2S The interconversion of these species is exploited in the sodium–sulfur battery. Hydrogenation Treatment of sulfur with hydrogen gives hydrogen sulfide. When dissolved in water, hydrogen sulfide is mildly acidic:[5] H2S ⇌ HS− + H+ Hydrogen sulfide gas and the hydrosulfide anion are extremely toxic to mammals, due to their inhibition of the oxygen-carrying capacity of hemoglobin and certain cytochromes in a manner analogous to cyanide and azide (see below, under precautions). Combustion The two principal sulfur oxides are obtained by burning sulfur: S + O2 → SO2 (sulfur dioxide) 2 SO2 + O2 → 2 SO3 (sulfur trioxide) Many other sulfur oxides are observed including the sulfur-rich oxides include sulfur monoxide, disulfur monoxide, disulfur dioxides, and higher oxides containing peroxo groups. Halogenation Sulfur reacts with fluorine to give the highly reactive sulfur tetrafluoride and the highly inert sulfur hexafluoride.[43] Whereas fluorine gives S(IV) and S(VI) compounds, chlorine gives S(II) and S(I) derivatives. Thus, sulfur dichloride, disulfur dichloride, and higher chlorosulfanes arise from the chlorination of sulfur. Sulfuryl chloride and chlorosulfuric acid are derivatives of sulfuric acid; thionyl chloride (SOCl2) is a common reagent in organic synthesis.[44] Pseudohalides Sulfur oxidizes cyanide and sulfite to give thiocyanate and thiosulfate, respectively. Metal sulfides Sulfur reacts with many metals. Electropositive metals give polysulfide salts. Copper, zinc, silver are attacked by sulfur, see tarnishing. Although many metal sulfides are known, most are prepared by high temperature reactions of the elements.[45] Geoscientists also study the isotopes of metal sulfides in rocks and sediment to study environmental conditions in the Earth's past.[46] Organic compounds Main article: Organosulfur compounds Illustrative organosulfur compounds Allicin, a chemical compound in garlic Allicin, a chemical compound in garlic (R)-cysteine, an amino acid containing a thiol group (R)-cysteine, an amino acid containing a thiol group Methionine, an amino acid containing a thioether Methionine, an amino acid containing a thioether Diphenyl disulfide, a representative disulfide Diphenyl disulfide, a representative disulfide Perfluorooctanesulfonic acid, a surfactant Perfluorooctanesulfonic acid, a surfactant Dibenzothiophene, a component of crude oil Dibenzothiophene, a component of crude oil Penicillin, an antibiotic where "R" is the variable group Penicillin, an antibiotic where "R" is the variable group Some of the main classes of sulfur-containing organic compounds include the following:[47] Thiols or mercaptans (so called because they capture mercury as chelators) are the sulfur analogs of alcohols; treatment of thiols with base gives thiolate ions. Thioethers are the sulfur analogs of ethers. Sulfonium ions have three groups attached to a cationic sulfur center. Dimethylsulfoniopropionate (DMSP) is one such compound, important in the marine organic sulfur cycle. Sulfoxides and sulfones are thioethers with one and two oxygen atoms attached to the sulfur atom, respectively. The simplest sulfoxide, dimethyl sulfoxide, is a common solvent; a common sulfone is sulfolane. Sulfonic acids are used in many detergents. Compounds with carbon–sulfur multiple bonds are uncommon, an exception being carbon disulfide, a volatile colorless liquid that is structurally similar to carbon dioxide. It is used as a reagent to make the polymer rayon and many organosulfur compounds. Unlike carbon monoxide, carbon monosulfide is stable nly as an extremely dilute gas, found between solar systems.[48] Organosulfur compounds are responsible for some of the unpleasant odors of decaying organic matter. They are widely known as the odorant in domestic natural gas, garlic odor, and skunk spray. Not al organic sulfur compounds smell unpleasant at ll concentrations: the sulfur-containing monoterpenoid (grapefruit mercaptan) in small concentrations is the characteristic scent of grapefruit, but has a generic thiol odor at larger concentrations. Sulfur mustard, a potent vesicant, was used in World War I as a disabling agent.[49] Sulfur–sulfur bonds are a structural component used to stiffen rubber, similar to the disulfide bridges that rigidify proteins (see biological below). In the most common type of industrial "curing" or hardening and strengthening of natural rubber, elemental sulfur is heated with the rubber to the point that chemical reactions fom disulfide bridges between isoprene units of the polymer. This process, patented in 1843, made rubber a major industrial product, especially in automobile tires. Because of the heat and sulfur, the process was named vulcanization, after the Roman god of the forge and volcanism. History Antiquity Pharmaceutical container for sulfur from the first half of the 20th century. From the Museo del Objeto del Objeto collection Being abundantly available in native frm, sulfur was known in ancient times and is referred to in the Torah (Genesis). English translations of the Christian Bible commonly referred to burning sulfur as "brimstone", giving rise to the term "fire-and-brimstone" sermons, in which listeners are reminded of the fate of eternal damnation that await the unbelieving and unrepentant. It is from this part of the Bible[50] that Hell is implied to "smell of sulfur" (likely due to its association with volcanic activity). According to the Ebers Papyrus, a sulfur ointment was used in ancient Egypt to treat granular eyelids. Sulfur was used for fumigation in preclassical Greece;[51] this is mentioned in the Odyssey.[52] Pliny the Elder discusses sulfur in book 35 of his Natural History, saying that its best-known source is the island of Melos. He mentions its use for fumigation, mdicine, and bleaching cloth.[53] A natural fom of sulfur known as shiliuhuan) was known in China since the 6th century BC and found in Hanzhong.[54] By the 3rd century, the Chinese had discovered that sulfur could be extracted from pyrite.[54] Chinese Daoists were interested in sulfur's flammability and its reactivity with certain metals, yet its earliest practical uses were found in traditional Chinese meicine.[54] The Wujing Zongyao of 1044 AD described various formulas for Chinese black powder, which is a mixture of potassium nitrate (KNO 3), charcoal, and sulfur.[55] Sulfur Brimstone Alchemical signs for sulfur, or the combustible elements, and brimstone, an older/archaic nme for sulfur.[56] Indian alchemists, practitioners of the "science of chemicals" (Sanskrit: रसशास्त्र, romanized: rasaśāstra), wrote extensively about the use of sulfur in alchemical operations with mercury, from the eighth century AD onwards.[57] In the rasaśāstra tradition, sulfur is called "the smelly" (गन्धक, gandhaka). Early European alchemists gave sulfur a unique alchemical symbol, a triangle atop a cross (🜍). (This is sometimes confused with the astronomical crossed-spear symbol ⚴ for 2 Pallas.) The variation known as brimstone has a symbol combining a two-barred cross atop a lemniscate (🜏). In traditional skin treatment, elemental sulfur was used (mainly in creams) to alleviate such conditions as scabies, ringworm, psoriasis, eczema, and acne. The mechanism of acion is unknown—though elemental sulfur does oxidize slowly to sulfurous acid, which is (through the ation of sulfite) a mild reducing and antibacterial agent.[58][59][60] Modern times Above: Sicilian kiln used to obtain sulfur from volcanic rock (diagram from a 1906 chemistry book) Right: Tody sulfur is known to have antifungal, antibacterial, and keratolytic activity; in the past it was used against acne vulgaris, rosacea, seborrheic dermatitis, dandruff, pityriasis versicolor, scabies, and warts.[61] This 1881 advertisement baselessly clais efficacy against rheumatism, gout, baldness, and graying of hair. Sulfur appears in a column of fixed (non-acidic) alkali in a chemical table of 1718.[62] Antoine Lavoisier used sulfur in combustion experiments, writing of some of these in 1777.[63] Sulfur deposits in Sicily were the dominant source for more than a century. By the late 18th century, about 2,000 tonnes per yar of sulfur were imported into Marseille, France, for the production of sulfuric acid for use in the Leblanc process. In industrializing Britain, with the repeal of tariffs on salt in 1824, demand for sulfur from Sicily surged upward. The increasing British control and exploitation of the mining, refining, and transportation of the sulfur, coupled with the failure of this lucrative export to transform Sicily's backward and impoverished economy, led to the Sulfur Crisis of 1840, when King Ferdinand II gave a monopoly of the sulfur industry to a French firm, violating an earlier 1816 trade agreement with Britain. A peaceful soluton was eventually negotiated by France.[64][65] In 1867, elemental sulfur was discovered in underground deposits in Louisiana and Texas. The highly successful Frasch process was developed to extract this resource.[66] In the late 18th century, furniture makers used molten sulfur to produce decorative inlays.[67] Molten sulfur is sometimes still used for setting steel bolts into drilled concrete holes where high shock resistance is desired for floor-mounted equipment attachment points. Pure powdered sulfur was used as a medicinal tonic and laxative.[39] With the advent of the contact process, the majority of sulfur tody is used to make sulfuric acid for a wide range of uses, particularly fertilizer.[68] In recent times, the main source of sulfur has become petroleum and natural gas. This is due to the requirement to remoe sulfur from fuels in ordr to prevent acid rain, and has resulted in a surplus of sulfur.[7] Spelling and etymology Sulfur is derived from the Latin word sulpur, which was Hellenized to sulphur in the erroneous belief that the Latin word came from Greek. This spelling was later reinterpreted as representing an /f/ sound and resulted in the spelling sulfur, which appears in Latin toward the end of the Classical period. The true Ancient Greek word for sulfur, θεῖον, theîon (from earlier θέειον, théeion), is the source of the international chemical prefix thio-. The Modern Standard Greek word for sulfur is θείο, theío. In 12th-century Anglo-French, it was sulfre. In the 14th century, the erroneously Hellenized Latin -ph- was restored in Middle English sulphre. By the 15th century, both full Latin spelling variants sulfur and sulphur became common in English. The parallel f~ph spellings continued in Britain until the 19th century, when the word was standardized as sulphur.[69] On the other hand, sulfur was the frm chosen in the United States, whereas Canada uses both. The IUPAC adopted the spelling sulfur in 1990 or 1971, depending on the source cited,[70] as did the Nomenclature Committee of the Royal Society of Chemistry in 1992, restoring the spelling sulfur to Britain.[71] Oxford Dictionaries note that "in chemistry and other technical uses ... the -f- spelling is ow the standard fom for this and related words in British as well as US contexts, and is increasingly used in general contexts as well."[72] Production Traditional sulfur mining at Ijen Volcano, East Java, Indonesia. This image shows the dangerous and rugged conditions the miners face, including toxic smoke and high drops, as well as their lack of protective equipment. The pipes over which they are standing are for condensing sulfur vapors. Sulfur may be found by itself and historically was usually obtained in this fom; pyrite has also been a source of sulfur.[73] In volcanic regions in Sicily, in ancient times, it was found on the surface of the Earth, and the "Sicilian process" was used: sulfur deposits were piled and stacked in brick kilns built on sloping hillsides, with airspaces between them. Then, some sulfur was pulverized, spread over the stacked ore and ignited, causing the fee sulfur to melt down the hills. Eventually the surface-borne deposits played out, and miners excavated veins that ultimately dotted the Sicilian landscape with labyrinthine mines. Mining was unmechanized and labor-intensive, with pickmen freeing the ore from the rock, and mine-boys or carusi carrying baskets of ore to the surface, often through a mile or more of tunnels. Once the ore was at the surface, it was reduced and extracted in smelting ovens. The conditions in Sicilian sulfur mines were horrific, prompting Booker T. Washington to write "I am not prepared just no to say to what extent I believe in a physical hell in the next world, but a sulfur mine in Sicily is about the nearest thing to hell that I expect to see in this lie."[74] Sulfur recovered from hydrocarbons in Alberta, stockpiled for shipment in North Vancouver, British Columbia Elemental sulfur was extracted from salt domes (in which it sometimes occurs in nearly pure fom) until the late 20th century. Sulfur is nw produced as a side product of other industrial processes such as in oil refining, in which sulfur is undesired. As a mineral, native sulfur under salt domes is thought to be a fossil mineral resource, produced by the ction of anaerobic bacteria on sulfate deposits. It was removed from such salt-dome mines mainly by the Frasch process.[39] In this method, superheated water was pumped into a native sulfur deposit to melt the sulfur, and then compressed air returned the 99.5 pure melted product to the surface. Throughout the 20th century this procedure produced elemental sulfur that required no further purification. Due to a liited nuber of such sulfur deposits and the high cst of working them, this process for mining sulfur has not been employed in a major way anywhere in the world since 2002.[75][76] Toay, sulfur is produced from petroleum, natural gas, and related fossil resources, from which it is obtained mainly as hydrogen sulfide.[7] Organosulfur compounds, undesirable impurities in petroleum, may be upgraded by subjecting them to hydrodesulfurization, which cleaves the C–S bonds:[75][76] The resulting hydrogen sulfide from this process, and also as it occurs in natural gas, is converted into elemental sulfur by the Claus process. This process entails oxidation of some hydrogen sulfide to sulfur dioxide and then the comproportionation of the two:[75][76] Production and prce (US market) of elemental sulfur Owing to the high sulfur content of the Athabasca Oil Sands, stockpiles of elemental sulfur from this process ow exist throughout Alberta, Canada.[77] Another way of storing sulfur is as a binder for concrete, the resulting product having many desirable properties (see sulfur concrete).[78] Sulfur is still mined from surface deposits in poorer nations with volcanoes, such as Indonesia, and worker conditions have not improved much since Booker T. Washington's days.[79] The world production of sulfur in 2011 amounted to 69 milion tonnes (Mt), with more than 15 countries contributing more than 1 Mt each. Countries producing more than 5 Mt are China (9.6), the United States (8.8), Canada (7.1) and Russia (7.1).[80] Production has been slowly increasing from 1900 to 2010; the prce was unstable in the 1980s and around 2010.[81] [Grand EE nаme] Grand Event brought to you by Inception Media, LLC. This editorial email with educational news was sent to {EMAIL}. To stоp receiving mаrketing communication from us [unsubsсribe hеre](. Feel frеe to contact us toll freе Domestic/International: [+17072979173](tel:+17072979173) Mon–Fri, 9am–5pm ET, or email us support@grandexpoevent.com Inception Media, LLC. Аll rights reserved 600 N Broad St Ste 5 PMB 1 Middletown, DE 19709 Plеase add our email address to your contact book (or mark as important) to guаrantee that our emails continue to reach your inbox. Inception Media, LLC appreciates your comments and inquiries. Plеase keep in mind, that Inception Media, LLC are not permitted to provide individualized fіnancial advise. 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