Passing chlorine gas over molten sulphur can easily make S2CL2. The disulphur dichloride vapour is condensed and redistill to give a pale yellow liquid (bp 138 C).
SO3 is made by heating ferric sulphate (Fe2(SO4)2 -> Fe2O3 + 3SO3 ) or by heating sodium hydrogen sulphate ( 2NaHSO4 -> Na2S2O7 + H2O, Na2S2O7 -> Na2SO4 + SO3 ). The water vapour will have to be removed in the second reaction with something like calcium oxide.
You can also make phosphoryl chloride by passing SO3 thru PCl3 ( PCl3 + SO3 -> POCl3 + SO2 )
The most versatile reaction would be to make PCL5 and pass SO2 through it. This produces both thionyl chloride and phosphoryl chloride ( PCl5 + SO2 -> POCL3 + SOCl2 ) which can be separated by fractional distillation ( Bp SOCl2 78 C, Bp POCl3 107 C ). The SO2 is conveniently made by adding concentrated sulphuric acid to copper metal and drying the gas produced before passing into the PCl5.
PCl5 can be synthesised using a 2 stage procedure, first from CL and P to make PCl3, then Cl and PCl3 to make PCL5. The most difficult component of this whole scheme is making the phosphorus"
Here is another version...........
The oxidation of SCl2 by atmospheric oxygen has been investigated using activated charcoal as the catalyst. The reaction has been discussed in terms of two reactions. Firstly, the irreversible oxidation of SCl2 to SO2Cl2 :
SCl2 + O2 __> SO2Cl2
and secondly, the reversible reaction between the SCl2 and the SO2Cl2 to form SOCl2 :
SCl2 + SO2Cl2 <__> SOCl2
This oxidation has been investigated at the temperatures 193°C, 138°C and 320°C, and the equilibrium constant of the reversible equilibrium reaction has been determined for each temperature. From the temperature dependence of this equilibrium constant it is found that the reaction is exothermic to the extent of 18 kcal.
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