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|Product Name:||Sulfur Dioxide||Purity:||99.9%|
|Density:||2.6288 Kg M−3||Application:||Reagent And Solvent In The Laboratory|
|Melting Point:||−72 °||Boiling Point:||−10 °C|
Laboratory Reagent Solvent Sulphur Dioxide Gas With Pungent Odor
Sulfite results from the reaction of aqueous base and sulfur dioxide. The reverse reaction involves acidification of sodium metabisulfite.
Treatment of basic solutions with sulfur dioxide affords sulfite salts.
Featuring sulfur in the +4 oxidation state, sulfur dioxide is a reducing agent. It is oxidized by halogens to give the sulfuryl halides, such as sulfuryl chloride.
Sulfur dioxide is the oxidising agent in the Claus process, which is conducted on a large scale in oil refineries. Here, sulfur dioxide is reduced by hydrogen sulfide to give elemental sulfur.
The sequential oxidation of sulfur dioxide followed by its hydration is used in the production of sulfuric acid.
1. Physical properties
|Hazardous class for transort||2.3|
2. Typical technical data (COA)
|Specification||Unit||Certified Concentration||Newradar SO2|
|Cylinder Size||Filling Weight (kg)||
|Precursor to sulfuric acid||Sulfur dioxide is an intermediate in the production of sulfuric acid, being converted to sulfur trioxide, and then to oleum, which is made into sulfuric acid. Sulfur dioxide for this purpose is made when sulfur combines with oxygen. The method of converting sulfur dioxide to sulfuric acid is called the contact process. Several billion kilograms are produced annually for this purpose|
|As a preservative||Sulfur dioxide is sometimes used as a preservative for dried apricots, dried figs, and other dried fruits, owing to its antimicrobial properties, and is called when used in this way in Europe. As a preservative, it maintains the colorful appearance of the fruit and prevents rotting. It is also added to sulfured molasses|
|In winemaking||Sulfur dioxide was used by the Romans in winemaking, when they discovered that burning sulfur candles inside empty wine vessels keeps them fresh and free from vinegar smell|
|As a reducing agent||Sulfur dioxide is also a good reductant. In the presence
of water, sulfur dioxide is able to decolorize substances. Specifically, it is a
useful reducing bleach for papers and delicate materials such as clothes
|Biochemical and biomedical roles||Sulfur dioxide is toxic in large amounts. It or its conjugate base bisulfite is produced biologically as an intermediate in both sulfate-reducing organisms and in sulfur-oxidizing bacteria, as well. The role of sulfur dioxide in mammalian biology is not yet well understood|
|As a refrigerant||Being easily condensed and possessing a high heat of
evaporation, sulfur dioxide is a candidate material for refrigerants. Prior to the
development of chlorofluorocarbons, sulfur dioxide was used as a
refrigerant in home refrigerators
|As a reagent and solvent in the laboratory||Sulfur dioxide is a versatile inert solvent widely used for dissolving highly oxidizing salts. It is also used occasionally as a source of the sulfonyl group in organic synthesis|
|Proposed use in climate engineering||Injections of sulfur dioxide in the
stratosphere has been proposed in climate engineering
|As an air pollutant||Sulfur dioxide is a noticeable component in the atmosphere, especially following volcanic eruptions.|