Everything about Sulfur Trioxide totally explained
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Sulfur trioxide (also spelled
sulphur trioxide) is the chemical compound with the formula SO
3. In the gaseous form, this species is an important pollutant, being the primary agent in
acid rain. It is prepared on massive scale as a precursor to
sulfuric acid.
Structure and bonding
Gaseous SO
3 is a
trigonal planar molecule of D
3h symmetry, as predicted by
VSEPR theory.
In terms of electron-counting formalisms, the sulfur atom has an oxidation state of +6, a formal charge of 0, and is surrounded by 6 electron pairs. From the perspective of
molecular orbital theory, most of these electron pairs are non-bonding in character, as is typical for
hypervalent molecules.
Sulfur trioxide also exhibits
resonance.
Chemical reactions
SO
3 is the
anhydride of H
2SO
4. Thus, the following reaction occurs:
» SO
3(l) + H
2O(l) → H
2SO
4(l) (-88
kJ mol−1)
The reaction occurs both rapidly and exothermically. At or above ~340 °C, sulfuric acid, sulfur trioxide, and water coexist in significant equilibrium concentrations.
Sulfur trioxide also reacts with
sulfur dichloride to yield the useful
reagent,
thionyl chloride.
» SO
3 + SCl
2 → SOCl
2 + SO
2
Sulfur Trioxide reacts with
water to create
sulfuric acid, though the reaction is too violent to be used in large-scale manufacturing.
SO
3 is a strong Lewis acid readily forming crystalline complexes with
pyridine,
dioxane and
trimethylamine which can be used as sulfonating agents.
Preparation
Sulfur trioxide can be prepared in the laboratory by the two-stage
pyrolysis of
sodium bisulfate:
1) dehydration: » 2NaHSO4 → Na2S2O7 + H2O @ 315°C
;2) cracking: » Na2S2O7 → Na2SO4 + SO3 @ 460°C
This method will work for other metal bisulfates, the controlling factor being the stability of the intermediate pyrosulfate salt.
Industrially SO3 is made by the contact process. Sulfur dioxide, generally made by the burning of sulfur or iron pyrite (a sulfide ore of iron), is first purified by electrostatic precipitation. The purified SO2 is then oxidised by atmospheric oxygen at between 400 and 600 °C over a catalyst consisting of vanadium pentoxide V2O5 activated with potassium oxide K2O on kieselguhr or silica support. Platinum also works very well but is too expensive and is poisoned (rendered ineffective) much more easily by impurities.
The majority of sulphur 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.
Structure of solid SO3
The nature of solid SO
3 is a surprisingly complex area because of structural changes caused by traces of water. Upon condensation of the gas, absolutely pure SO
3 condenses into a trimer, which is often called
γ-SO
3. This molecular form is a colorless solid with a melting point of 16.8 °C. It adopts a cyclic structure described as [S(=O)
2(
μ-O)]
3.
If SO
3 is condensed above 27 °C, then
α-"SO
3" forms, which has a melting point of 62.3°C.
α-SO
3 is fibrous in appearance, like asbestos (with which it has no chemical relationship). Structurally, it's the
polymer [S(=O)
2(
μ-O)]
n. Each end of the polymer is terminated with OH groups (hence
α-"SO
3" isn't really a form of SO
3).
β-SO
3, like the alpha form, is fibrous but of different molecular weight, consisting of an hydroxyl-capped polymer, but melts at 32.5 °C. Both the gamma and the beta forms are metastable, eventually converting to the stable alpha form if left standing for sufficient time. This conversion is caused by traces of water.
Relative vapor pressures of solid SO
3 are alpha< beta< gamma at identical temperatures, indicative of their relative
molecular weights. Liquid sulfur trioxide has vapor pressure consistent with the gamma form. Thus heating a crystal of
α-SO
3 to its melting point results in a sudden increase in vapor pressure, which can be forceful enough to shatter a glass vessel in which it's heated. This effect is known as the "alpha explosion."
SO
3 is aggressively
hygroscopic. In fact, the heat of hydration is sufficient that mixtures of SO
3 and wood or cotton can ignite. In such cases, SO
3 dehydrates these
carbohydrates.
Sources
Further Information
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