Oleum
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Oleum refers to a solution of sulfur trioxide in sulfuric acid or sometimes more specifically to pyrosulfuric acid, disulfuric acid.
Oleums can be described by the formula xSO3.H2O where x is the total molar sulfur trioxide content. The value of x can be varied, to include different oleums. They can also be described by the forumula 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 2 gives us the empirical formula H2S2O7 of pyrosulfuric acid also called disulfuric acid. Pure pyrosulfuric acid itself is a solid at room temperature, melting at 36 °C and rarely used either in the laboratory or industrial processes.
Oleum is an important intermediate in the manufacture of sulfuric acid. If mainly due to its high enthalpy of hydration when SO3 is added directly to water, rather than simply dissolving, it tends to form a fine mist of sulfuric acid which is difficult to manage. If SO3 is added to concentrated sulfuric acid instead, it dissolves readily forming oleum which can then be diluted with water to produce additional concentrated sulfuric acid.
An advantage of oleum is that it can be shipped in bulk liquid railcars, but is at normal temperature not a liquid, enhancing the safety of shipment. It is converted to a liquid by the destination processor by steam heating, which requires some care to avoid overheating and so overpressurizing the container, which will then release suphuric acid fumes through the container's pressure relief valve, likely creating a general health and safety hazard over a wide area.
Like concentrated sulfuric acid itself, the acid 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 glucose in an exothermic reaction, leaving nearly pure carbon as a solid. This expands out of the container, hardening as a solid black substance with gas bubbles in it. Oleum is highly corrosive.
The lead chamber process is notable here because it cannot produce sulfur trioxide or even concentrated sulfuric acid directly due to corrosion of the lead, and absorption of NO2 gas. So during the reign of this otherwise very successful process and up until the development of the contact process much later, oleum had to be obtained by separate means. Industrially the biggest source of this acid was by the distillation of iron sulfates at Nordhausen, from which the historical name Nordhausen sulfuric acid is derived.
(Note: sulfur/sulfuric can also be spelt sulphur/sulphuric.)
External links
- For a full list of external links to MSDSs, spectroscopic data, commercial chemicals suppliers etc. for this compound, see [Chemical sources].
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