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'''Oleum''' ([[Latin]] ''oleum'' = "oil"), or '''fuming sulfuric acid''' refers to a solution of various compositions of [[sulfur trioxide]] in [[sulfuric acid]] or sometimes more specifically to [[disulfuric acid]] (also known as pyrosulfuric acid). | '''Oleum''' ([[Latin]] ''oleum'' = "oil"), or '''fuming sulfuric acid''' refers to a solution of various compositions of [[sulfur trioxide]] in [[sulfuric acid]] or sometimes more specifically to [[disulfuric acid]] (also known as pyrosulfuric acid). | ||
| − | Oleums can be described by the formula ''y''SO<sub>3</sub>.H<sub>2</sub>O where y is the total molar sulfur trioxide content. The value of ''y'' can be varied, to include different oleums. | + | Oleums can be described by the formula ''y''SO<sub>3</sub>.H<sub>2</sub>O where ''y'' is the total molar sulfur trioxide content. The value of ''y'' can be varied, to include different oleums. |
| − | They can also be described by the formula H<sub>2</sub>SO<sub>4</sub> | + | They can also be described by the formula H<sub>2</sub>SO<sub>4</sub>·''x''SO<sub>3</sub> where ''x'' is now defined as the molar free sulfur trioxide content. Oleum is generally assayed according to the free SO<sub>3</sub> content by weight. |
| − | A value for ''x'' of 1 gives us the [[empirical formula]] H<sub>2</sub>S<sub>2</sub>O<sub>7</sub> for disulfuric (pyrosulfuric) acid. Pure disulfuric acid itself is a solid at room temperature, melting at 36 °C and rarely used either in the laboratory or industrial processes. | + | A value for ''x'' of 1 gives us the [[empirical formula]] H<sub>2</sub>S<sub>2</sub>O<sub>7</sub> for disulfuric (pyrosulfuric) acid. Pure disulfuric acid itself is a solid at room temperature, melting at 36 °C and rarely used either in the laboratory or industrial processes. |
==Production== | ==Production== | ||
| − | Oleum is produced in the [[contact process]], where [[sulfur]] is oxidized to [[sulfur trioxide]] which is subsequently dissolved in concentrated sulfuric acid. | + | Oleum is produced in the [[contact process]], where [[sulfur]] is oxidized to [[sulfur trioxide]] which is subsequently dissolved in concentrated sulfuric acid. Sulfuric acid itself is regenerated by dilution of part of the oleum. |
| − | 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 | + | 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 SO<sub>2</sub> gas. Until this process was made obsolete by the [[contact process]], oleum had to be obtained through indirect methods. Historically, the biggest production of oleum came from the [[distillation]] of [[iron sulfate]]s at [[Nordhausen]] in the [[Harz Mountains]] in central [[Germany]], from which the historical name Nordhausen sulfuric acid is derived. |
==Applications== | ==Applications== | ||
===Sulfuric acid production=== | ===Sulfuric acid production=== | ||
| − | Oleum is an important intermediate in the manufacture of sulfuric acid due to its high [[enthalpy]] of [[hydration reaction|hydration]]. When SO<sub>3</sub> is added to water, rather than simply dissolving, it tends to form a fine mist of sulfuric acid, which is difficult to manage. However, SO<sub>3</sub> added to concentrated sulfuric acid readily dissolves, forming oleum which can then be diluted with water to produce additional concentrated sulfuric acid.<ref>Considine | + | Oleum is an important intermediate in the manufacture of sulfuric acid due to its high [[enthalpy]] of [[hydration reaction|hydration]]. When SO<sub>3</sub> is added to water, rather than simply dissolving, it tends to form a fine mist of sulfuric acid, which is difficult to manage. However, SO<sub>3</sub> added to concentrated sulfuric acid readily dissolves, forming oleum which can then be diluted with water to produce additional concentrated sulfuric acid.<ref>{{citation | last = Considine | first = Douglas M. | title = Chemical and Process Technology Encyclopedia | publisher = McGraw-Hill | location = New York | year = 1974 | pages = 1070–71}}.</ref> |
===As an intermediate for transportation=== | ===As an intermediate for transportation=== | ||
Oleum is a useful form for transporting sulfuric acid compounds, typically in rail tankcars, between oil refineries (which produce various sulfur compounds as a byproduct of refining) and industrial consumers. | Oleum is a useful form for transporting sulfuric acid compounds, typically in rail tankcars, between oil refineries (which produce various sulfur compounds as a byproduct of refining) and industrial consumers. | ||
| − | Certain compositions of oleum are solid at room temperature, and thus is safer to ship than when liquid. Solid oleum can then be converted into liquid at the destination through steam heating or dilution or concentration. This requires some care to prevent overheating and evaporation of sulfur trioxide. To extract it from a tank car requires careful heating using steam conduits within the tank car. Great care must be taken to avoid overheating, as this can increase the internal pressure within the tank car to a value exceeding the limit of the tank's [[safety valve]]. | + | Certain compositions of oleum are solid at room temperature, and thus is safer to ship than when liquid. Solid oleum can then be converted into liquid at the destination through steam heating or dilution or concentration. This requires some care to prevent overheating and evaporation of sulfur trioxide. To extract it from a tank car requires careful heating using steam conduits within the tank car. Great care must be taken to avoid overheating, as this can increase the internal pressure within the tank car to a value exceeding the limit of the tank's [[safety valve]]. In [[Richmond, California]] in 1993 a significant release occurred due to overheating, causing a release of sulfur trioxide that absorbed moisture from the atmosphere, creating a mist of micrometre-sized sulfuric acid particles that formed an inhalation health hazard.<ref>{{citation | url = http://www.cchealth.org/groups/hazmat/accident_history.php | webpage = Major Accidents at Chemical/Refinery Plants in Contra Costa County}}.</ref><ref>{{citation | last1 = Baskett | first1 = R. L. | last2 = Vogt | first2 = P. J. | author3 = Schalk III | last4 = Pobanz | first4 = B. M. | title = ARAC Dispersion Modeling of the July 26, 1993 Oleum Tank Car Spill in Richmond, California | id = UCRL-ID-116012 | date = February 3, 1994}}.</ref> This mist produced adverse health effects on residents and workers over a wide area.<ref>{{citation | url = http://www.epicode.com/epiwebcase.html | webpage = CASE STUDY - Richmond, California Oleum Release}}.</ref> |
===Organic chemistry=== | ===Organic chemistry=== | ||
| Line 24: | Line 24: | ||
===Explosives manufacture=== | ===Explosives manufacture=== | ||
| − | Oleum is used in the manufacture of many [[ | + | Oleum is used in the manufacture of many [[explosive]]s, with the notable exception of [[nitrocellulose]].<ref>{{citation | last = Urbanski | first = Tadeusz | title = Chemistry and Technology of Explosives | publisher = Pergamon | location = Oxford | year = 1965 | volume = 2 | page = 329}}.</ref> The chemical requirements for explosives manufacture often call for anhydrous mixtures containing [[nitric acid]] and [[sulfuric acid]]. Ordinary commercial grade nitric acid consists of the constant boiling [[azeotrope]] of nitric acid and water, and contains 68% nitric acid. Mixtures of ordinary nitric acid in sulfuric acid therefore contain substantial amounts of water and are unsuitable for processes such as occur in the manufacture of [[trinitrotoluene]]. |
| − | Anhydrous nitric acid, referred to as [[white fuming nitric acid]], can be used to prepare water-free [[nitration]] mixtures, and this method is used in laboratory scale operations where the cost of material is not of primary importance. Fuming nitric acid is very hazardous to handle and transport, because it is extremely corrosive and volatile. For industrial use, such strong [[nitration]] mixtures are prepared by mixing oleum with ordinary commercial nitric acid so that the free sulfur trioxide in the oleum consumes the water in the nitric acid.<ref>Urbanski | + | Anhydrous nitric acid, referred to as [[white fuming nitric acid]], can be used to prepare water-free [[nitration]] mixtures, and this method is used in laboratory scale operations where the cost of material is not of primary importance. Fuming nitric acid is very hazardous to handle and transport, because it is extremely corrosive and volatile. For industrial use, such strong [[nitration]] mixtures are prepared by mixing oleum with ordinary commercial nitric acid so that the free sulfur trioxide in the oleum consumes the water in the nitric acid.<ref>{{citation | last = Urbanski | first = Tadeusz | title = Chemistry and Technology of Explosives | publisher = Pergamon | location = Oxford | year = 1965 | volume = 1 | page = 347–49}}.</ref> |
==Reactions== | ==Reactions== | ||
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==References== | ==References== | ||
| − | + | {{reflist}} | |
[[Category:Sulfur oxoacids]] | [[Category:Sulfur oxoacids]] | ||
{{Imported from Wikipedia|name=Oleum|id=305677437}} | {{Imported from Wikipedia|name=Oleum|id=305677437}} | ||
Revision as of 18:26, 23 August 2009
Oleum (Latin oleum = "oil"), or fuming sulfuric acid refers to a solution of various compositions of sulfur trioxide in sulfuric acid or sometimes more specifically to disulfuric acid (also known as pyrosulfuric acid).
Oleums can be described by the formula ySO3.H2O where y is the total molar sulfur trioxide content. The value of y can be varied, to include different oleums. They can also be described by the formula H2SO4·xSO3 where x is now defined as the molar free sulfur trioxide content. Oleum is generally assayed according to the free SO3 content by weight.
A value for x of 1 gives us the empirical formula H2S2O7 for disulfuric (pyrosulfuric) acid. Pure disulfuric acid itself is a solid at room temperature, melting at 36 °C and rarely used either in the laboratory or industrial processes.
Contents
Production
Oleum is produced in the contact process, where sulfur is oxidized to sulfur trioxide which is subsequently dissolved in concentrated sulfuric acid. Sulfuric acid itself is regenerated by dilution of part of the oleum.
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 SO2 gas. Until this process was made obsolete by the contact process, oleum had to be obtained through indirect methods. Historically, the biggest production of oleum came from the distillation of iron sulfates at Nordhausen in the Harz Mountains in central Germany, from which the historical name Nordhausen sulfuric acid is derived.
Applications
Sulfuric acid production
Oleum is an important intermediate in the manufacture of sulfuric acid due to its high enthalpy of hydration. When SO3 is added to water, rather than simply dissolving, it tends to form a fine mist of sulfuric acid, which is difficult to manage. However, SO3 added to concentrated sulfuric acid readily dissolves, forming oleum which can then be diluted with water to produce additional concentrated sulfuric acid.[1]
As an intermediate for transportation
Oleum is a useful form for transporting sulfuric acid compounds, typically in rail tankcars, between oil refineries (which produce various sulfur compounds as a byproduct of refining) and industrial consumers.
Certain compositions of oleum are solid at room temperature, and thus is safer to ship than when liquid. Solid oleum can then be converted into liquid at the destination through steam heating or dilution or concentration. This requires some care to prevent overheating and evaporation of sulfur trioxide. To extract it from a tank car requires careful heating using steam conduits within the tank car. Great care must be taken to avoid overheating, as this can increase the internal pressure within the tank car to a value exceeding the limit of the tank's safety valve. In Richmond, California in 1993 a significant release occurred due to overheating, causing a release of sulfur trioxide that absorbed moisture from the atmosphere, creating a mist of micrometre-sized sulfuric acid particles that formed an inhalation health hazard.[2][3] This mist produced adverse health effects on residents and workers over a wide area.[4]
Organic chemistry
Oleum is a harsh reagent, and is highly corrosive. One important use of oleum as a reagent is the secondary nitration of nitrobenzene. The first nitration can occur with nitric acid in sulfuric acid, but this deactivates the ring towards further electrophilic substitution. A stronger reagent, oleum, is needed to introduce the second nitro group onto the aromatic ring.
Explosives manufacture
Oleum is used in the manufacture of many explosives, with the notable exception of nitrocellulose.[5] The chemical requirements for explosives manufacture often call for anhydrous mixtures containing nitric acid and sulfuric acid. Ordinary commercial grade nitric acid consists of the constant boiling azeotrope of nitric acid and water, and contains 68% nitric acid. Mixtures of ordinary nitric acid in sulfuric acid therefore contain substantial amounts of water and are unsuitable for processes such as occur in the manufacture of trinitrotoluene.
Anhydrous nitric acid, referred to as white fuming nitric acid, can be used to prepare water-free nitration mixtures, and this method is used in laboratory scale operations where the cost of material is not of primary importance. Fuming nitric acid is very hazardous to handle and transport, because it is extremely corrosive and volatile. For industrial use, such strong nitration mixtures are prepared by mixing oleum with ordinary commercial nitric acid so that the free sulfur trioxide in the oleum consumes the water in the nitric acid.[6]
Reactions
Like concentrated sulfuric acid, oleum is such a strong dehydrating agent that if poured onto powdered glucose, or virtually any other sugar, it will draw the elements of water out of the sugar in an exothermic reaction, leaving nearly pure carbon as a solid. This carbon expands outward, hardening as a solid black substance with gas bubbles in it.
References
- ↑ Considine, Douglas M. Chemical and Process Technology Encyclopedia; McGraw-Hill: New York, 1974; pp 1070–71.
- ↑ Major Accidents at Chemical/Refinery Plants in Contra Costa County, <http://www.cchealth.org/groups/hazmat/accident_history.php>.
- ↑ Baskett, R. L.; Vogt, P. J.; Schalk III; Pobanz, B. M. ARAC Dispersion Modeling of the July 26, 1993 Oleum Tank Car Spill in Richmond, California, February 3, 1994. UCRL-ID-116012.
- ↑ CASE STUDY - Richmond, California Oleum Release, <http://www.epicode.com/epiwebcase.html>.
- ↑ Urbanski, Tadeusz Chemistry and Technology of Explosives; Pergamon: Oxford, 1965; Vol. 2, p 329.
- ↑ Urbanski, Tadeusz Chemistry and Technology of Explosives; Pergamon: Oxford, 1965; Vol. 1, p 347–49.
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