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Sulfuryl chloride is used as a source of Cl 2. Because it is a pourable liquid, it is considered more convenient than Cl 2 to dispense. Sulfuryl chloride is used in the conversion of C−H to C−Cl adjacent to activating substituents such as carbonyls and sulfoxides: [5] [6] RC(O)CH 2 R' + SO 2 Cl 2 → RC(O)CHClR' + HCl + SO 2
The reaction occurs via a free radical mechanism. UV-light initiates homolysis of chlorine, producing a pair of chlorine atoms: . Chain initiation: Thereafter a chlorine atom attacks the hydrocarbon chain, freeing hydrogen to form hydrogen chloride and an alkyl free radical.
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SO 2 + Cl 2 → SO 2 Cl 2. Sulfur dioxide is the oxidising agent in the Claus process, which is conducted on a large scale in oil refineries. Here, sulfur dioxide is reduced by hydrogen sulfide to give elemental sulfur: SO 2 + 2 H 2 S → 3 S + 2 H 2 O. The sequential oxidation of sulfur dioxide followed by its hydration is used in the ...
S 8 + 4 Cl 2 → 4 S 2 Cl 2, ΔH = −58.2 kJ/mol. Excess chlorine produces sulfur dichloride, which causes the liquid to become less yellow and more orange-red: S 2 Cl 2 + Cl 2 ⇌ 2 SCl 2, ΔH = −40.6 kJ/mol. The reaction is reversible, and upon standing, SCl 2 releases chlorine to revert to the disulfur dichloride.
The addition of Cl 2 to S 2 Cl 2 has been proposed to proceed via a mixed valence intermediate Cl 3 S−SCl. SCl 2 undergoes even further chlorination to give SCl 4, but this species is unstable at near room temperature. It is likely that several S n Cl 2 exist where n > 2. Disulfur dichloride, S 2 Cl 2, is the most common impurity in SCl 2.
The sulfolene is about 40 kJ/mol more stable than the isometric sulfine in CH 2 Cl 2 /SO 2 solution. [ 6 ] Reaction of 1,2-dimethylidenecyclohexane with SO 2 gives a sultine through a hetero-Diels-Alder reaction under kinetic control or a sulfolene through a cheletropic reaction under thermodynamic control
For many substances, the formation reaction may be considered as the sum of a number of simpler reactions, either real or fictitious. The enthalpy of reaction can then be analyzed by applying Hess' law, which states that the sum of the enthalpy changes for a number of individual reaction steps equals the enthalpy change of the overall reaction.