Balanced Chemical Equations - Formulae And Equations

Which formula equation represents the burning of sulfur to produce sulfur dioxide? What is the formula equation for the reaction between sulfuric acid and dissolved sodium hydroxide if all products and reactants are in the aqueous or liquid phase?Sulfur is not considered corrosive to the usual construction materials. Because sulfur ointment is messy, malodorous, tends to stain, and can produce an irritant dermatitis, its use Following dermal application of radioactive sulfur to the backs of 4 subjects for 8 hours, radioactivity was detectable in...4:16 understand how sulfur dioxide and oxides of nitrogen oxides contribute to acid rain. 4:17 describe how long-chain alkanes are converted to alkenes and shorter-chain alkanes by catalytic cracking (using silica or alumina as the catalyst and a temperature in the range of 600-700⁰C).Sulfur (in traditional lay Commonwealth English: sulphur) is a chemical element with the symbol S and atomic number 16. It is abundant, multivalent and nonmetallic. Under normal conditions, sulfur atoms form cyclic octatomic molecules with a chemical formula S8.Questions related to Sulfur Dioxide. How much sulfur dioxide is produced in Kg's when 1 litre of Diesel is burnt by vehicles? It is possible that the effect of Sulfur dioxide has something to do with changing the viscosity of the DOPC film at the interface.

Sulfur | S - PubChem | 2.2Molecular Formula

Sulfur dioxide produced weak increases in micronuclei after activation in a plant assay Sulfur dioxide is a common combustion product from the burning of coal or oil products and as a Without the catalyst, the oxidation reaction given in Equation (20.2) is too slow for the process to be profitable.The formula equation which represents the burning of sulfur to produce sulfur dioxide is: S + O₂ → SO₂. Sulfur in the pressure of oxygen produces sulfur dioxide gas. The balanced chemical reaction is shown below as:- The enthalpy change of the reaction is ΔH = -297 kJ/mol.Hydrogen sulfide Sulfurous acid Peroxymonosulfuric acid Sulfur trioxide Oleum. Sulfuric acid is a constituent of acid rain, being formed by atmospheric oxidation of sulfur dioxide in the presence of water - i.e. oxidation of sulfurous acid. In the first step, sulfur is burned to produce sulfur dioxide.The balanced reaction that describes the reaction between sulfur and oxygen to produce sulfur dioxide is expressed S (s) + O2 (g) = SO2 (g). In many manufacturing plants, sulfur dioxide is furhter reacted to oxygen to form sulfur trioxide then added with water to produce sulfuric acid.

4:15 explain how the combustion of some... | TutorMyself Chemistry

Sulfur dioxide. Properties of oxides. Oxides is a complex chemical substances that represent simple chemical compounds of the elements with oxygen. Burning coal is forming two oxides: carbon monoxide and carbon dioxide 2C+O2→2CO - formation of carbon monoxide.Sulfur, nonmetallic chemical element, one of the most reactive of the elements. Pure sulfur is a tasteless, odorless, brittle solid that is pale yellow in color, a poor conductor Millions of tons of sulfur are produced each year, mostly for the manufacture of sulfuric acid , which is widely used in industry.When burned, sulfur produces a blue flame and sulfur dioxide gas — a common pollutant, according to the Environmental Protection Agency. Sulfur dioxide in the atmosphere comes mostly from fossil-fuel power plants and is one of the primary causes of acid rain. The gas is also a lung irritant.Which Formula Equation Represents The Burning Of Sulfur To Produce Sulfur Dioxide?What volume of hydrogen at 42 °C and 149 kPa can be burned in a fuel cell using 296 L of oxygen gas measured under the same conditions?

Jump to navigation Jump to seek For different uses, see SO2.

Sulfur dioxide Names IUPAC identify Sulfur dioxide Other names Sulfurous anhydride Sulfur(IV) oxide Identifiers CAS Number 7446-09-5 3D type (JSmol) Interactive image Beilstein Reference 3535237 ChEBI CHEBI:18422 ChEMBL ChEMBL1235997 ChemSpider 1087 ECHA InfoCard 100.028.359 EC Number 231-195-2 E quantity E220 (preservatives) Gmelin Reference 1443 KEGG D05961 MeSH Sulfur+dioxide PubChem CID 1119 RTECS number WS4550000 UNII 0UZA3422Q4 UN number 1079, 2037 CompTox Dashboard (EPA) DTXSID6029672 InChI InChI=1S/O2S/c1-3-2 Key: RAHZWNYVWXNFOC-UHFFFAOYSA-N InChI=1/O2S/c1-3-2Key: RAHZWNYVWXNFOC-UHFFFAOYAT SMILES O=S=O Properties Chemical formula SO2 Molar mass 64.066 g mol−1 Appearance Colorless fuel Odor Pungent; similar to a just-struck fit[1]Density 2.6288 kg m−3Melting point −72 °C; −98 °F; 201 Okay Boiling point −10 °C (14 °F; 263 Okay) Solubility in water 94 g/L[2]bureaucracy sulfurous acid Vapor drive 237.2 okayPa Acidity (pKa) 1.81 Basicity (pKb) 12.19 Magnetic susceptibility (χ) −18.2·10−6 cm3/mol Viscosity 12.82 μPa·s[3]Structure Point group C2vCoordination geometry Digonal Molecular form Dihedral Dipole second 1.sixty two D Thermochemistry Std molarentropy (So298) 248.223 J Okay−1 mol−1Std enthalpy offormation (ΔfH⦵298) −296.81 kJ mol−1Hazards GHS pictograms GHS Signal word Danger GHS danger statements H314, H331[4]NFPA 704 (fire diamond) 3 0 0 Lethal dose or concentration (LD, LC): LC50 (median concentration) 3000 ppm (mouse, 30 min)2520 ppm (rat, 1 hr)[6]LCLo (lowest revealed) 993 ppm (rat, 20 min)611 ppm (rat, Five hr)764 ppm (mouse, 20 min)1000 ppm (human, 10 min)3000 ppm (human, Five min)[6]NIOSH (US health exposure limits): PEL (Permissible) TWA Five ppm (13 mg/m3)[5]REL (Recommended) TWA 2 ppm (5 mg/m3) ST 5 ppm (Thirteen mg/m3)[5]IDLH (Immediate risk) 100 ppm[5]Related compounds Related sulfur oxides Sulfur monoxideSulfur trioxide Related compounds Ozone

Selenium dioxideSulfurous acidTellurium dioxide

Except the place in a different way famous, data are given for fabrics of their usual state (at 25 °C [77 °F], 100 okayPa). check (what's ?) Infobox references

Sulfur dioxide (IUPAC-recommended spelling) or sulphur dioxide (traditional Commonwealth English) is the chemical compound with the formula SO2. It is a toxic gas answerable for the odor of burnt matches. It is released naturally by way of volcanic process and is produced as a spinoff of copper extraction and the burning of fossil fuels infected with sulfur compounds. Sulfur dioxide has a pungent smell like nitric acid.

Structure and bonding

SO2 is a unethical molecule with C2vsymmetry point workforce. A valence bond concept means taking into consideration just s and p orbitals would describe the bonding in terms of resonance between two resonance structures.

Two resonance constructions of sulfur dioxide

The sulfur–oxygen bond has a bond order of 1.5. There is fortify for this easy way that does not invoke d orbital participation.[7] In terms of electron-counting formalism, the sulfur atom has an oxidation state of +4 and a formal charge of +1.

Occurrence

The blue auroral glows of Io's higher atmosphere are led to by way of volcanic sulfur dioxide.

Sulfur dioxide is located on Earth and exists in very small concentrations and in the atmosphere at about 1 ppm.[8][9]

On other planets, sulfur dioxide will also be found in more than a few concentrations, the most significant being the atmosphere of Venus, where it's the third-most significant atmospheric fuel at 150 ppm. There, it condenses to form clouds, and is a key component of chemical reactions in the planet's setting and contributes to international warming.[10] It has been implicated as a key agent in the warming of early Mars, with estimates of concentrations in the lower surroundings as top as A hundred ppm,[11] although it most effective exists in trace quantities. On each Venus and Mars, as on Earth, its number one source is assumed to be volcanic. The setting of Io, a herbal satellite tv for pc of Jupiter, is 90% sulfur dioxide[12] and trace quantities are concept to additionally exist in the setting of Jupiter.

As an ice, it's thought to exist in abundance on the Galilean moons—as subliming ice or frost on the trailing hemisphere of Io,[13] and in the crust and mantle of Europa, Ganymede, and Callisto, most likely also in liquid shape and readily reacting with water.[14]

Production

Sulfur dioxide is primarily produced for sulfuric acid manufacture (see contact procedure). In the United States in 1979, 23.6 million tonnes (26,014,547 US quick lots) of sulfur dioxide had been used on this method, when compared with A hundred and fifty thousand tonnes (165,347 US quick lots) used for different functions. Most sulfur dioxide is produced by way of the combustion of elemental sulfur. Some sulfur dioxide may be produced by means of roasting pyrite and other sulfide ores in air.[15]

">Play media An experiment showing burning of sulfur in oxygen. A flow-chamber joined to a gas washing bottle (filled with a solution of methyl orange) is being used. The product is sulfur dioxide (SO2) with some traces of sulfur trioxide (SO3). The "smoke" that exits the fuel washing bottle is, in reality, a sulfuric acid fog generated in a response. Combustion routes

Sulfur dioxide is the product of the burning of sulfur or of burning materials that include sulfur:

S + O2 → SO2, ΔH = −297 kJ/mol

To support combustion, liquified sulfur (140–150 °C, 284-302 °F) is sprayed via an atomizing nozzle to generate tremendous drops of sulfur with a big floor house. The response is exothermic, and the combustion produces temperatures of 1000–1600 °C (1832–2912 °F). The significant quantity of warmth produced is recovered by means of steam era that can subsequently be transformed to electricity.[15]

The combustion of hydrogen sulfide and organosulfur compounds proceeds in a similar fashion. For instance:

2 H2S + 3 O2 → 2 H2O + 2 SO2

The roasting of sulfide ores corresponding to pyrite, sphalerite, and cinnabar (mercury sulfide) also releases SO2:[16]

4 FeS2 + 11 O2 → 2 Fe2O3 + 8 SO2 2 ZnS + Three O2 → 2 ZnO + 2 SO2 HgS + O2 → Hg + SO2 4 FeS + 7O2 → 2 Fe2O3 + 4 SO2

A mixture of those reactions is answerable for the greatest supply of sulfur dioxide, volcanic eruptions. These occasions can release thousands and thousands of tonnes of SO2.

Reduction of higher oxides

Sulfur dioxide may also be a byproduct in the manufacture of calcium silicate cement; CaSO4 is heated with coke and sand in this procedure:

2 CaSO4 + 2 SiO2 + C → 2 CaSiO3 + 2 SO2 + CO2

Until the Nineteen Seventies, business amounts of sulfuric acid and cement had been produced by means of this procedure in Whitehaven, England. Upon being mixed with shale or marl, and roasted, the sulfate liberated sulfur dioxide gas, utilized in sulfuric acid production, the response additionally produced calcium silicate, a precursor in cement manufacturing.[17]

On a laboratory scale, the action of hot concentrated sulfuric acid on copper turnings produces sulfur dioxide.

Cu + 2 H2SO4 → CuSO4 + SO2 + 2 H2OFrom sulfites

Sulfites results through the action of aqueous base on sulfur dioxide:

SO2 + 2 NaOH → Na2SO3 + H2O

The opposite response occurs upon acidification:

H+ + HSO3− → SO2 + H2O

Reactions

Featuring sulfur in the +4 oxidation state, sulfur dioxide is a decreasing agent. It is oxidized through halogens to give the sulfuryl halides, such as sulfuryl chloride:

SO2 + Cl2 → SO2Cl2

Sulfur dioxide is the oxidising agent in the Claus procedure, which is performed on a large scale in oil refineries. Here, sulfur dioxide is diminished by hydrogen sulfide to give elemental sulfur:

SO2 + 2 H2S → 3 S + 2 H2O

The sequential oxidation of sulfur dioxide followed by its hydration is utilized in the manufacturing of sulfuric acid.

2 SO2 + 2 H2O + O2 → 2 H2SO4Laboratory reactions

Sulfur dioxide is one of the few commonplace acidic yet decreasing gases. It turns wet litmus pink (being acidic), then white (due to its bleaching effect). It may be known by way of effervescent it through a dichromate answer, turning the resolution from orange to inexperienced (Cr3+ (aq)). It too can scale back ferric ions to ferrous.[18]

Sulfur dioxide can react with sure 1,3-dienes in a cheletropic reaction to form cyclic sulfones. This reaction is exploited on an commercial scale for the synthesis of sulfolane, which is crucial solvent in the petrochemical trade.

Sulfur dioxide can bind to metal ions as a ligand to shape steel sulfur dioxide complexes, normally where the transition metal is in oxidation state Zero or +1. Many different bonding modes (geometries) are identified, however usually, the ligand is monodentate, attached to the steel through sulfur, which will also be both planar and pyramidal η1.[19] As a η1-SO2 (S-bonded planar) ligand sulfur dioxide purposes as a Lewis base the use of the lone pair on S. SO2 purposes as a Lewis acids in its η1-SO2 (S-bonded pyramidal) bonding mode with metals and in its 1:1 adducts with Lewis bases equivalent to dimethylacetamide and trimethyl amine. When bonding to Lewis bases the acid parameters of SO2 are EA = 0.51 and EA = 1.56.

Uses

The overarching, dominant use of sulfur dioxide is in the production of sulfuric acid.[15]

Precursor to sulfuric acid

Sulfur dioxide is an intermediate in the manufacturing of sulfuric acid, being transformed to sulfur trioxide, and then to oleum, which is made into sulfuric acid. Sulfur dioxide for this objective is made when sulfur combines with oxygen. The way of changing sulfur dioxide to sulfuric acid is called the touch procedure. Several billion kilograms are produced every year for this goal.

As a preservative

Sulfur dioxide is sometimes used as a preservative for dried apricots, dried figs, and different dried culmination, owing to its antimicrobial homes and talent to save you oxidation,[20] and is called E220[21] when used in this approach in Europe. As a preservative, it maintains the colourful appearance of the fruit and prevents rotting. It may be added to sulfured molasses.

Sulfur dioxide used to be first utilized in winemaking via the Romans, after they discovered that burning sulfur candles inside empty wine vessels assists in keeping them recent and loose from vinegar smell.[22]

It remains to be the most important compound in winemaking, and is measured in parts per million (ppm) in wine. It is present even in so-called unsulfurated wine at concentrations of up to 10 mg/L.[23] It serves as an antibiotic and antioxidant, protecting wine from spoilage by means of bacteria and oxidation - a phenomenon that leads to the browning of the wine and a loss of cultivar explicit flavors.[24][25] Its antimicrobial motion also is helping reduce risky acidity. Wines containing sulfur dioxide are typically categorised with "containing sulfites".

Sulfur dioxide exists in wine in loose and certain paperwork, and the combos are referred to as general SO2. Binding, for example to the carbonyl staff of acetaldehyde, varies with the wine in question. The unfastened shape exists in equilibrium between molecular SO2 (as a dissolved gas) and bisulfite ion, which is in flip in equilibrium with sulfite ion. These equilibria rely on the pH of the wine. Lower pH shifts the equilibrium against molecular (gaseous) SO2, which is the lively form, whilst at higher pH extra SO2 is found in the inactive sulfite and bisulfite paperwork. The molecular SO2 is active as an antimicrobial and antioxidant, and this may be the shape which is also perceived as a stinky smell at prime levels. Wines with total SO2 concentrations underneath 10 ppm don't require "contains sulfites" on the label by means of US and EU laws. The upper limit of overall SO2 allowed in wine in the US is 350 ppm; in the EU it is One hundred sixty ppm for crimson wines and 210 ppm for white and rosé wines. In low concentrations, SO2 is mostly undetectable in wine, but at free SO2 concentrations over 50 ppm, SO2 turns into evident in the scent and taste of wine.

SO2 may be an important compound in vineyard sanitation. Wineries and equipment must be kept clean, and because bleach can't be used in a vineyard due to the risk of cork taint,[26] a combination of SO2, water, and citric acid is frequently used to blank and sanitize apparatus. Ozone (O3) is now used broadly for sanitizing in wineries due to its efficacy, and because it does now not impact the wine or maximum equipment.[27]

As a decreasing agent

Sulfur dioxide could also be a excellent reductant. In the presence of water, sulfur dioxide is in a position to decolorize components. Specifically, this is a useful decreasing bleach for papers and gentle fabrics corresponding to garments. This bleaching impact usually does no longer ultimate very lengthy. Oxygen in the surroundings reoxidizes the lowered dyes, restoring the colour. In municipal wastewater remedy, sulfur dioxide is used to treat chlorinated wastewater prior to release. Sulfur dioxide reduces free and blended chlorine to chloride.[28]

Sulfur dioxide is somewhat soluble in water, and through both IR and Raman spectroscopy; the hypothetical sulfurous acid, H2SO3, is not provide to any extent. However, such answers do show spectra of the hydrogen sulfite ion, HSO3−, through reaction with water, and it is in fact the exact reducing agent present:

SO2 + H2O ⇌ HSO3− + H+Biochemical and biomedical roles

Sulfur dioxide or its conjugate base bisulfite is produced biologically as an intermediate in each sulfate-reducing organisms and in sulfur-oxidizing micro organism, as smartly. The function of sulfur dioxide in mammalian biology isn't but smartly understood.[29] Sulfur dioxide blocks nerve indicators from the pulmonary stretch receptors and abolishes the Hering–Breuer inflation reflex.

It is considered that endogenous sulfur dioxide plays an important physiological role in regulating cardiac and blood vessel serve as, and aberrant or poor sulfur dioxide metabolism can give a contribution to several other cardiovascular illnesses, comparable to arterial hypertension, atherosclerosis, pulmonary arterial high blood pressure, and stenocardia.[30]

It was shown that in kids with pulmonary arterial high blood pressure due to congenital middle illnesses the stage of homocysteine is higher and the level of endogenous sulfur dioxide is lower than in standard regulate children. Moreover, these biochemical parameters strongly correlated to the severity of pulmonary arterial high blood pressure. Authors considered homocysteine to be one of helpful biochemical markers of disease severity and sulfur dioxide metabolism to be one of doable healing objectives in those sufferers.[31]

Endogenous sulfur dioxide also has been shown to decrease the proliferation fee of endothelial easy muscle cells in blood vessels, by way of reducing the MAPK process and activating adenylyl cyclase and protein kinase A.[32] Smooth muscle cell proliferation is one of necessary mechanisms of hypertensive remodeling of blood vessels and their stenosis, so it is a very powerful pathogenetic mechanism in arterial high blood pressure and atherosclerosis.

Endogenous sulfur dioxide in low concentrations reasons endothelium-dependent vasodilation. In upper concentrations it causes endothelium-independent vasodilation and has a unfavorable inotropic impact on cardiac output function, thus effectively reducing blood force and myocardial oxygen consumption. The vasodilating and bronchodilating results of sulfur dioxide are mediated via ATP-dependent calcium channels and L-type ("dihydropyridine") calcium channels. Endogenous sulfur dioxide is also a potent antiinflammatory, antioxidant and cytoprotective agent. It lowers blood pressure and slows hypertensive transforming of blood vessels, particularly thickening of their intima. It also regulates lipid metabolism.[33]

Endogenous sulfur dioxide also diminishes myocardial injury, brought about through isoproterenol adrenergic hyperstimulation, and strengthens the myocardial antioxidant protection reserve.[34]

As a reagent and solvent in the laboratory

Sulfur dioxide is a versatile inert solvent extensively used for dissolving extremely oxidizing salts. It is also used now and again as a source of the sulfonyl crew in organic synthesis. Treatment of aryl diazonium salts with sulfur dioxide and cuprous chloride yields the corresponding aryl sulfonyl chloride, for instance:[35]

As a end result of its very low Lewis basicity, it's steadily used as a low-temperature solvent/diluent for superacids like Magic acid (FSO3H/SbF5), taking into account extremely reactive species like tert-butyl cation to be noticed spectroscopically at low temperature (although tertiary carbocations do react with SO2 above about –30 °C, or even less reactive solvents like SO2ClF will have to be used at these higher temperatures).[36]

Aspirational programs As a refrigerant

Being easily condensed and possessing a high warmth of evaporation, sulfur dioxide is a candidate subject material for refrigerants. Prior to the construction of chlorofluorocarbons, sulfur dioxide used to be used as a refrigerant in house refrigerators.

Climate engineering

Injections of sulfur dioxide in the stratosphere has been proposed in climate engineering. The cooling effect would be equivalent to what has been seen after the huge explosive 1991 eruption of Mount Pinatubo. However this manner of geoengineering would have unsure regional penalties on rainfall patterns, as an example in monsoon areas.[37]

As an air pollutant

Further information: Stratospheric sulfur aerosols A collection of estimates of past and long run anthropogenic global sulfur dioxide emissions. The Cofala et al. estimates are for sensitivity research on SO2 emission insurance policies, CLE: Current Legislation, MFR: Maximum Feasible Reductions. RCPs (Representative Concentration Pathways) are used in CMIP5 simulations for contemporary (2013–2014) IPCC 5th overview document.

Sulfur dioxide is a noticeable element in the environment, particularly following volcanic eruptions.[38] According to the United States Environmental Protection Agency,[39] the amount of sulfur dioxide launched in the U.S. in line with 12 months was once:

Year SO21970 31,161,000 quick lots (28.3 Mt) 1980 25,905,000 quick heaps (23.5 Mt) 1990 23,678,000 quick lots (21.5 Mt) 1996 18,859,000 brief lots (17.1 Mt) 1997 19,363,000 brief tons (17.6 Mt) 1998 19,491,000 quick lots (17.7 Mt) 1999 18,867,000 quick tons (17.1 Mt)

Sulfur dioxide is a major air pollutant and has vital impacts upon human well being.[40] In addition, the focus of sulfur dioxide in the atmosphere can influence the habitat suitability for plant communities, in addition to animal lifestyles.[41] Sulfur dioxide emissions are a precursor to acid rain and atmospheric particulates. Due in large part to the US EPA's Acid Rain Program, the U.S. has had a 33% decrease in emissions between 1983 and 2002. This growth resulted partly from flue-gas desulfurization, a generation that enables SO2 to be chemically certain in power crops burning sulfur-containing coal or oil. In explicit, calcium oxide (lime) reacts with sulfur dioxide to form calcium sulfite:

CaO + SO2 → CaSO3

Aerobic oxidation of the CaSO3 gives CaSO4, anhydrite. Most gypsum offered in Europe comes from flue-gas desulfurization.

Sulfur will also be got rid of from coal right through burning by the usage of limestone as a mattress subject material in fluidized bed combustion.[42]

Sulfur may also be got rid of from fuels sooner than burning, fighting formation of SO2 when the fuel is burnt. The Claus process is used in refineries to produce sulfur as a byproduct. The Stretford process has also been used to remove sulfur from gas. Redox processes using iron oxides can also be used, as an example, Lo-Cat[43] or Sulferox.[44]

Fuel components equivalent to calcium components and magnesium carboxylate may be used in marine engines to decrease the emission of sulfur dioxide gases into the surroundings.[45]

As of 2006, China was the international's largest sulfur dioxide polluter, with 2005 emissions estimated to be 25,490,000 brief tons (23.1 Mt). This quantity represents a 27% build up since 2000, and is more or less similar with U.S. emissions in 1980.[46]

A sulfur dioxide plume from Halemaʻumaʻu, which glows at night

Sulfur dioxide in the international on April 15, 2017. Note that sulfur dioxide moves through the environment with prevailing winds and thus local sulfur dioxide distributions range day to day with weather patterns and seasonality.

Safety

US Geological Survey volunteer tests for sulfur dioxide after the 2018 lower Puna eruption Inhalation

Incidental exposure to sulfur dioxide is routine, e.g. the smoke from matches, coal, and sulfur-containing fuels.

Sulfur dioxide is mildly poisonous and can be hazardous in top concentrations.[47] Long-term exposure to low concentrations may be problematic. A 2011 systematic review concluded that publicity to sulfur dioxide is associated with preterm birth.[48]

U.S. laws

In 2008, the American Conference of Governmental Industrial Hygienists lowered the non permanent exposure limit to 0.25 parts per million (ppm). In the US, the OSHA set the PEL at 5 ppm (Thirteen mg/m3) time-weighted reasonable. Also in the US, NIOSH set the IDLH at One hundred ppm.[49] In 2010, the EPA "revised the primary SO2NAAQS by establishing a new one-hour standard at a level of 75 parts per billion (ppb). EPA revoked the two existing primary standards because they would not provide additional public health protection given a one-hour standard at 75 ppb."[40]

Ingestion

In the United States, the Center for Science in the Public Interest lists the two meals preservatives, sulfur dioxide and sodium bisulfite, as being safe for human consumption excluding for certain asthmatic people who could also be delicate to them, particularly in large amounts.[50] Symptoms of sensitivity to sulfiting brokers, together with sulfur dioxide, manifest as potentially life-threatening trouble respiring inside of minutes of ingestion.[51]

See additionally

Bunker gasoline National Ambient Air Quality Standards Sulfur trioxide Sulfur–iodine cycle

References

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External links

Wikimedia Commons has media comparable to sulfur dioxide.Global map of sulfur dioxide distribution United States Environmental Protection Agency Sulfur Dioxide web page International Chemical Safety Card 0074 IARC Monographs. "Sulfur Dioxide and some Sulfites, Bisulfites and Metabisulfites". vol. 54. 1992. p. 131. NIOSH Pocket Guide to Chemical Hazards CDC – Sulfure Dioxide – NIOSH Workplace Safety and Health Topic Sulfur Dioxide, Molecule of the MonthvteOxidesCombined oxidation states Antimony tetroxide (Sb2O4) Cobalt(II,III) oxide (Co3O4) Lead(II,IV) oxide (Pb3O4) Manganese(II,III) oxide (Mn3O4) Iron(II,III) oxide (Fe3O4) Silver(I,III) oxide (Ag2O2) Triuranium octoxide (U3O8) Carbon suboxide (C3O2) Mellitic anhydride (C12O9) Praseodymium(III,IV) oxide (Pr6O11) Terbium(III,IV) oxide (Tb4O7) Dichlorine pentoxide (Cl2O5)+1 oxidation state Copper(I) oxide (Cu2O) Caesium oxide (Cs2O) Dicarbon monoxide (C2O) Dichlorine monoxide (Cl2O) Gallium(I) oxide (Ga2O) Lithium oxide (Li2O) Potassium oxide (K2O) Rubidium oxide (Rb2O) Silver oxide (Ag2O) Thallium(I) oxide (Tl2O) Sodium oxide (Na2O) Water (hydrogen oxide) (H2O)+2 oxidation state Aluminium(II) oxide (AlO) Barium oxide (BaO) Beryllium oxide (BeO) Cadmium oxide (CdO) Calcium oxide (CaO) Carbon monoxide (CO) Chromium(II) oxide (CrO) Cobalt(II) oxide (CoO) Copper(II) oxide (CuO) Dinitrogen dioxide (N2O2) Germanium monoxide (GeO) Iron(II) oxide (FeO) Lead(II) oxide (PbO) Magnesium oxide (MgO) Manganese(II) oxide (MnO) Mercury(II) oxide (HgO) Nickel(II) oxide (NiO) Nitric oxide (NO) Palladium(II) oxide (PdO) Silicon monoxide (SiO) Strontium oxide (SrO) Sulfur monoxide (SO) Disulfur dioxide (S2O2) Thorium monoxide (ThO) Tin(II) oxide (SnO) Titanium(II) oxide (TiO) Vanadium(II) oxide (VO) Zinc oxide (ZnO)+3 oxidation state Actinium(III) oxide (Ac2O3) Aluminium oxide (Al2O3) Antimony trioxide (Sb2O3) Arsenic trioxide (As2O3) Bismuth(III) oxide (Bi2O3) Boron trioxide (B2O3) Cerium(III) oxide (Ce2O3) Chromium(III) oxide (Cr2O3) Cobalt(III) oxide (Co2O3) Dinitrogen trioxide (N2O3) Dysprosium(III) oxide (Dy2O3) Erbium(III) oxide (Er2O3) Europium(III) oxide (Eu2O3) Gadolinium(III) oxide (Gd2O3) Gallium(III) oxide (Ga2O3) Holmium(III) oxide (Ho2O3) Indium(III) oxide (In2O3) Iron(III) oxide (Fe2O3) Lanthanum oxide (La2O3) Lutetium(III) oxide (Lu2O3) Manganese(III) oxide (Mn2O3) Neodymium(III) oxide (Nd2O3) Nickel(III) oxide (Ni2O3) Phosphorus monoxide (PO) Phosphorus trioxide (P4O6) Praseodymium(III) oxide (Pr2O3) Promethium(III) oxide (Pm2O3) Rhodium(III) oxide (Rh2O3) Samarium(III) oxide (Sm2O3) Scandium oxide (Sc2O3) Terbium(III) oxide (Tb2O3) Thallium(III) oxide (Tl2O3) Thulium(III) oxide (Tm2O3) Titanium(III) oxide (Ti2O3) Tungsten(III) oxide (W2O3) Vanadium(III) oxide (V2O3) Ytterbium(III) oxide (Yb2O3) Yttrium(III) oxide (Y2O3)+4 oxidation state Americium dioxide (AmO2) Carbon dioxide (CO2) Carbon trioxide (CO3) Cerium(IV) oxide (CeO2) Chlorine dioxide (ClO2) Chromium(IV) oxide (CrO2) Dinitrogen tetroxide (N2O4) Germanium dioxide (GeO2) Hafnium(IV) oxide (HfO2) Lead dioxide (PbO2) Manganese dioxide (MnO2) Neptunium(IV) oxide (NpO2) Nitrogen dioxide (NO2) Osmium dioxide (OsO2) Plutonium(IV) oxide (PuO2) Praseodymium(IV) oxide (PrO2) Protactinium(IV) oxide (PaO2) Rhodium(IV) oxide (RhO2) Ruthenium(IV) oxide (RuO2) Selenium dioxide (SeO2) Silicon dioxide (SiO2) Sulfur dioxide (SO2) Tellurium dioxide (TeO2) Terbium(IV) oxide (TbO2) Thorium dioxide (ThO2) Tin dioxide (SnO2) Titanium dioxide (TiO2) Tungsten(IV) oxide (WO2) Uranium dioxide (UO2) Vanadium(IV) oxide (VO2) Zirconium dioxide (ZrO2)+5 oxidation state Antimony pentoxide (Sb2O5) Arsenic pentoxide (As2O5) Dinitrogen pentoxide (N2O5) Niobium pentoxide (Nb2O5) Phosphorus pentoxide (P2O5) Protactinium(V) oxide (Pa2O5) Tantalum pentoxide (Ta2O5) Vanadium(V) oxide (V2O5)+6 oxidation state Chromium trioxide (CrO3) Molybdenum trioxide (MoO3) Rhenium trioxide (ReO3) Selenium trioxide (SeO3) Sulfur trioxide (SO3) Tellurium trioxide (TeO3) Tungsten trioxide (WO3) Uranium trioxide (UO3) Xenon trioxide (XeO3)+7 oxidation state Dichlorine heptoxide (Cl2O7) Manganese heptoxide (Mn2O7) Rhenium(VII) oxide (Re2O7) Technetium(VII) oxide (Tc2O7)+8 oxidation state Osmium tetroxide (OsO4) Ruthenium tetroxide (RuO4) Xenon tetroxide (XeO4) Iridium tetroxide (IrO4)Related Oxocarbon Suboxide Oxyanion Ozonide Peroxide Superoxide OxypnictideOxides are sorted via oxidation state. Category:Oxides vteMolecules detected in outer spaceMoleculesDiatomic Aluminium monochloride Aluminium monofluoride Aluminium(II) oxide Argonium Cyapho radical Carbon monosulfide Carbon monoxide Cyano radical Diatomic carbon Fluoromethylidynium Helium hydride ion Hydrogen chloride Hydrogen fluoride Hydrogen (molecular) Hydroxyl radical Iron(II) oxide Magnesium monohydride Methylidyne radical Nitric oxide Nitrogen (molecular) Imidogen Sulfur mononitride Oxygen (molecular) Phosphorus monoxide phosphorus mononitride Potassium chloride Silicon carbide Silicon monoxide Silicon monosulfide Sodium chloride Sodium iodide Sulfur monohydride Sulfur monoxide Titanium(II) oxide

Triatomic Aluminium(I) hydroxide Aluminium isocyanide Amino radical Carbon dioxide Carbonyl sulfide CCP radical Chloronium Diazenylium Dicarbon monoxide Disilicon carbide Ethynyl radical Formyl radical Hydrogen cyanide (HCN) Hydrogen isocyanide (HNC) Hydrogen sulfide Hydroperoxyl Iron cyanide Isoformyl Magnesium cyanide Magnesium isocyanide Methylene radical N2H+ Nitrous oxide Nitroxyl Ozone Phosphaethyne Potassium cyanide Protonated molecular hydrogen Sodium cyanide Sodium hydroxide Silicon carbonitride c-Silicon dicarbide SiNC Sulfur dioxide Thioformyl Thioxoethenylidene Titanium dioxide Tricarbon WaterFouratoms Acetylene Ammonia Cyanic acid Cyanoethynyl Cyclopropynylidyne Formaldehyde Fulminic acid HCCN Hydrogen peroxide Hydromagnesium isocyanide Isocyanic acid Isothiocyanic acid Ketenyl Methylene amidogen Methyl radical Propynylidyne Protonated carbon dioxide Protonated hydrogen cyanide Silicon tricarbide Thioformaldehyde Tricarbon monoxide Tricarbon monosulfide Thiocyanic acidFiveatoms Ammonium ion Butadiynyl Carbodiimide Cyanamide Cyanoacetylene Cyanoformaldehyde Cyanomethyl Cyclopropenylidene Formic acid Isocyanoacetylene Ketene Methane Methoxy radical Methylenimine Propadienylidene Protonated formaldehyde Protonated formaldehyde Silane Silicon-carbide clusterSixatoms Acetonitrile Cyanobutadiynyl radical E-Cyanomethanimine Cyclopropenone Diacetylene Ethylene Formamide HC4N Ketenimine Methanethiol Methanol Methyl isocyanide Pentynylidyne Propynal Protonated cyanoacetyleneSevenatoms Acetaldehyde Acrylonitrile Vinyl cyanide Cyanodiacetylene Ethylene oxide Glycolonitrile Hexatriynyl radical Methylacetylene Methylamine Methyl isocyanate Vinyl alcoholEightatoms Acetic acid Aminoacetonitrile Cyanoallene Ethanimine Glycolaldehyde Heptatrienyl radical Hexapentaenylidene Methylcyanoacetylene Methyl formate PropenalNineatoms Acetamide Cyanohexatriyne Cyanotriacetylene Dimethyl ether Ethanol Methyldiacetylene Octatetraynyl radical Propene PropionitrileTenatomsor more Acetone Benzene Benzonitrile Buckminsterfullerene (C60, C60+, fullerene, buckyball) C70 fullerene Cyanodecapentayne Cyanopentaacetylene Cyanotetra-acetylene Ethylene glycol Ethyl formate Methyl acetate Methyl-cyano-diacetylene Methyltriacetylene Propanal n-Propyl cyanide PyrimidineDeuteratedmolecules Ammonia Ammonium ion Formaldehyde Formyl radical Heavy water Hydrogen cyanide Hydrogen deuteride Hydrogen isocyanide Methylacetylene N2D+ Trihydrogen cationUnconfirmed Anthracene Dihydroxyacetone Ethyl methyl ether Glycine Graphene Hemolithin (possibly 1st extraterrestrial protein discovered) H2NCO+ Linear C5 Naphthalene cation Phosphine Pyrene SilylidineRelated Abiogenesis Astrobiology Astrochemistry Atomic and molecular astrophysics Chemical formula Circumstellar envelope Cosmic dust Cosmic ray Cosmochemistry Diffuse interstellar band Earliest known existence forms Extraterrestrial lifestyles Extraterrestrial liquid water Forbidden mechanism Homochirality Intergalactic dust Interplanetary medium Interstellar medium Photodissociation area Iron–sulfur global principle Kerogen Molecules in stars Nexus for Exoplanet System Science Organic compound Outer space PAH global speculation Panspermia Polycyclic aromatic hydrocarbon (PAH) RNA world hypothesis Spectroscopy Tholin Category:Astrochemistry Astronomy portal Chemistry portal vteSulfur compoundsSulfides and disulfides Al2S3 As2S2 As2S3 As2S5 As4S4 Au2S Au2S3 B2S3 BaS BeS Bi2S3 CS2 C3S2 C6S6 CaS CdS CeS CoS Cr2S3 CSSe CSTe CuFeS2 CuS D2S Dy2S3 Er2S3 EuS FeS2 GaS H2S HfS2 HgS In2S3 K2S LaS LiS MgS MoS3 NaHS Na2S NH4HS NiS P4Sx PbS PbS2 PSCl3 PSI3 PtS ReS2 Re2S7 SiS SrS TlS VS SeS2 S2U WS2 Sb2S3 Sb2S5 Sb4S3O3 Sm2S3 Y2S3 ZrS2Sulfur halides S2Br2 SBr2 S2Cl2 SCl2 SCl4 SF4 S2F10 SF6 SI2Sulfur oxides and oxyhalides SO2 SO3 SOBr2 SOCl2 SOF2 H2SO3 H2SO4 H2S2O7 H2SO5Sulfites CdSO3 K2SO3Sulfates Ag2SO4 CaSO4 Cs2O4S Er2(SO4)3 Eu2(SO4)3 HgSO4 K2SO4 KAl(SO4)2 NaAl(SO4)2 RaSO4 SnSO4 SrSO4 Ti(SO4)2 Tm2(SO4)3 Yb2(SO4)3 Zr(SO4)2 Thiocyanates HSCN KSCN Co(SCN)2Organosulfur compounds C2H4S C2H6S3 C4H4S C32H66S2 CHCl3S C2H3SNChemical formulation Authority keep watch over GND: 4180392-9 MA: 2780447027 NDL: 00568537 Retrieved from "https://en.wikipedia.org/w/index.php?title=Sulfur_dioxide&oldid=1013164764"