Product Category: Sulfur Dioxide

Name/Chemical Formula: Sulfur Dioxide/SO2
Packaging Specifications: 4L, 8L, 40L
Purity (%) and Impurities (ppm): 99.9%
Impurities (ppm): O2 + N2 < 100, H2O < 10, Others < 200

Packaging

Packaged in 40L steel cylinders, and can also be repackaged into 4-10L gas cylinders according to customer requirements.

Applications

Manufacturing inorganic sulfides, organic synthesis, fumigants, pesticides, preservatives for fruits and vegetables, disinfectant bactericides, bleaching agents, paper industry, tanning, refrigerants, petroleum refining, magnesium smelting, preservatives, calibration gases, online instrumentation.

Physical and Chemical Properties

A colorless gas with a pungent, suffocating, and irritating odor. Highly liquefiable, non-flammable in air, and does not support combustion.

Precautions

Keep tightly closed and provide adequate local exhaust and general ventilation. Operators must receive specialized training and strictly adhere to operating procedures. It is recommended that operators wear self-priming filter-type gas masks (full facepiece), polyethylene chemical protective clothing, and rubber gloves. Keep away from flammable and combustible materials. Prevent gas leakage into the workplace air. Avoid contact with oxidizers and reducing agents. Handle with care during transportation to prevent damage to cylinders and attachments. Equip with emergency leak handling equipment. Store in a cool, well-ventilated warehouse. Keep away from fire and heat sources. Storage temperature should not exceed 30°C. Separate from flammable/combustible materials, oxidizers, reducing agents, and food chemicals. Avoid mixed storage. The storage area should be equipped with emergency leak handling equipment.

Sulfur dioxide (chemical formula: SO2) is the most common sulfur oxide. It is a colorless gas with a strong, irritating odor and is one of the major air pollutants. It is emitted during volcanic eruptions and is also produced in many industrial processes. Since coal and petroleum often contain sulfur compounds, burning them generates sulfur dioxide. When sulfur dioxide dissolves in water, it forms sulfurous acid (a major component of acid rain). Further oxidation of SO2, usually in the presence of a catalyst such as nitrogen dioxide, produces sulfuric acid. This is one of the reasons for environmental concerns regarding the use of these fuels as energy sources.