sulfur oxide (IV) has a name, also officially used in Chemistry - sulfur dioxide, in addition, this substance is also called sulfur dioxide or sulfur dioxide.Sulfur oxide (IV) in normal conditions - is a gas that has no color, with a distinctive, unpleasant odor that resembles the smell of the match at the time of the fire.
gas is liquefied when the pressure increases, the temperature may not differ from normal room.The substance is soluble in water to form sulfurous acid unstable.The solubility of sulfur dioxide in water at a temperature of 20 C 11,5 grams of agent per 100 grams of water.Interestingly, when the temperature rises, the level of solubility of the compound decreases.Besides water, sulfur dioxide is soluble in ethanol and sulfuric acid.The nature of the sulfur dioxide, whose formula is SO2, is one of the elements constituting the volcanic gas.
industrial production of sulfur dioxide based on the direct burning of sulfur may also be prepared by firing the gas sulfides, especially such as pyrite.
sulfide gas is produced and by laboratory methods.To this reacted exposure to sulfites strong acids.As the basic substance used in laboratories and hydrosulfites.This response takes the form of the equation: Na2SO3 + H2SO4 → Na2SO4 + H2SO3.The result of the reaction, as can be seen from the equation, is sulfuric acid, which because of its instability immediately decomposes to sulfur dioxide and water.
Less material is used for a method in which impact on the less active metals with dilute sulfuric acid, and the reaction should occur upon heating of the working solution.
basic chemical properties of sulfur dioxide as follows.
Sulphur dioxide is absorbed in the ultraviolet range of the spectrum.It is classified as an acidic oxide.As already indicated, the sulfur dioxide is soluble in water in a reversible chemical reaction.
Upon entry into the reaction gas are obtained with alkali sulfites In general, if we characterize the reactivity of the gas, it is necessary to recognize rather high.During reactions most commonly manifested recovery properties of matter and the level of oxidation of the sulfur in the reaction, it becomes higher.
oxidative properties of sulfur dioxide exhibits during the reactions accompanied by strong reducing agents.For example, in the industrial sector for the production of sulfur method is used, warped her recovery carbon monoxide (II).
sulfur oxide (IV) in the chemical industry mainly used to produce sulfuric acid.In general, its use is very broad and ambiguous.The fact that sulfur dioxide is toxic.When inhaled, it can get poisoning symptoms are sore throat, runny nose, cough.If inhaled sulfur dioxide damage brings the greater the higher the concentration of the substance was.At high concentrations can occur severe consequences, up to the choking, speech disorders, and pulmonary edema.
sulfur oxide (IV) is used in the food industry, in particular it is present in beverages slaboalkogolnyh preservative.In the textile industry it is used as a constituent element of means for bleaching a variety of materials that can not be bleached with chlorine compounds.
in industry and research laboratories sulfur oxide (IV) serves as an indispensable solvent, but in this case it should be remembered that gas can contain impurities of water and SO3, which mogtst affect the purity and correctness during the reaction in the presence ofdioxide.Therefore, in these cases, the gas is purified by passing through a filter containing concentrated H2SO4, always in a closed vessel.
Due to the extensive use of sulfur dioxide acts as one of the main air pollutants.Especially dangerous emissions produced from the burning of our usual energy - coal, natural gas and oil.As a rule, most of the harmful effects is through precipitation, because of rainwater - the final product is the presence of the substance in aerosol form.
Currently, the highest concentration of this gas is observed in the northern hemisphere, especially over the United States, Ukraine, Western Europe and in the western regions of Russia.
