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|Product Name:||Sulfur Dioxide||Purity:||99.9%|
|Density:||2.6288 Kg M−3||Application:||Winemaking, Precursor To Sulfuric Acid|
|Cylinder Volume:||40L, 80L, 100L, 400L, 800L And 926L||Valve:||QF-10|
Pungent Industrial Gases Liquid Sulfur Dioxide SO2 Reducing Agent
Sulfur dioxide is the chemical compound with the formula SO2. At standard atmosphere, it is a toxic gas with a pungent, irritating smell. The triple point is 197.69 K and 1.67 kPa. It is released naturally by volcanic activity.
The significant amount of heat produced is recovered by steam generation that can subsequently be converted to electricity.
A combination of these reactions is responsible for the largest source of sulfur dioxide, volcanic eruptions. These events can release millions of tonnes of SO2.
Sulfur dioxide can also be a byproduct in the manufacture of calcium silicate cement; CaSO4 is heated with coke and sand. On a laboratory scale, the action of hot concentrated sulfuric acid on copper turnings produces sulfur dioxide.
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.|