sulfur trioxide oor Spaans
sulfur trioxide
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(inorganic chemistry) A corrosive liquid, SO <sub>3</sub> , which forms sulfuric acid on contact with water; made commercially by the oxidation of sulfur dioxide.
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anhídrido sulfúrico
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Oleums can be described by the formula ySO3.H2O where y is the total molar sulfur trioxide content.
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This requires care to prevent overheating and evaporation of sulfur trioxide.
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Sulfur trioxide is very reactive and representative reactions are given in scheme 16.95.
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Thus, sulfur(VI) oxide (sulfur trioxide; SO3) is more acidic than sulfur(IV) oxide (sulfur dioxide; SO2).
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At or above 340 °C, sulfuric acid, sulfur trioxide, and water coexist in significant equilibrium concentrations.
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Sulfur trioxide, SO3, is produced in enormous quantities each year for use in the synthesis of sulfuric acid.
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Examples of molecules with trigonal planar geometry include boron trifluoride (BF3), formaldehyde (H2CO), phosgene (COCl2), and sulfur trioxide (SO3).
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When a high-sulfur fuel is burned, the sulfur is converted to sulfur dioxide (SO2) and sulfur trioxide (SO3).
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Sulfamic acid is produced industrially by treating urea with a mixture of sulfur trioxide and sulfuric acid (or oleum).
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They can also be described by the formula H2SO4.xSO3 where x is now defined as the molar free sulfur trioxide content.
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Chlordecone has been produced by reacting hexachlorocyclopentadiene and sulfur trioxide under heat and pressure in the presence of antimony pentachloride as a catalyst
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Chlordecone has been produced by reacting hexachlorocyclopentadiene and sulfur trioxide under heat and pressure in the presence of antimony pentachloride as a catalyst.
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Examples include nitric acid (from ammonia), sulfuric acid (from sulfur dioxide to sulfur trioxide by the contact process), terephthalic acid from p-xylene, and acrylonitrile from propane and ammonia.
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Oleum (Latin oleum, meaning oil), or fuming sulfuric acid, is a solution of various compositions of sulfur trioxide in sulfuric acid, or sometimes more specifically to disulfuric acid (also known as pyrosulfuric acid).
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The lead chamber process for sulfuric acid production was abandoned partly because it could not produce sulfur trioxide or concentrated sulfuric acid directly due to corrosion of the lead, and absorption of NO2 gas.
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Resistivity of the fly ash can be changed by decreasing the temperature in the ESP or by conditioning the particles upstream of the ESP with sulfur trioxide (SO3), sulfuric acid (H2SO4), water, sodium, or ammonia (NH3).
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Due to its effectiveness in converting sulfur dioxide into sulfur trioxide, and thereby sulfuric acid, special care must be taken with the operating temperatures and placement of a power plant's SCR unit when firing sulfur-containing fuels.
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It can also be used to break down mineral salts such as sulfates (SO2− 4) through thermolysis, in this case producing sulfur dioxide (SO2) or sulfur trioxide (SO3) gas which can be dissolved in water to obtain sulfuric acid.
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The majority of sulfur trioxide made in this way is converted into sulfuric acid not by the direct addition of water, with which it forms a fine mist, but by absorption in concentrated sulfuric acid and dilution with water of the produced oleum.
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Vanadium(V) oxide serves the crucial purpose of catalysing the mildly exothermic oxidation of sulfur dioxide to sulfur trioxide by air in the contact process: 2 SO2 + O2 ⇌ 2 SO3 The discovery of this simple reaction, for which V2O5 is the most effective catalyst, allowed sulfuric acid to become the cheap commodity chemical it is today.
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Adding chromium trioxide ( Cr03 ) to dilute sulfuric acid achieves the same result
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It is a precursor of the trioxide (SO3), used to make SULFURIC ACID.
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Molecular chromic acid could in principle be made by adding chromium trioxide to water (cf. manufacture of sulfuric acid).
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