6dthjd1
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sulfur dichloride/sulfur monochloride sulfure precipitate
I had made disulfur dichloride mixed with sulfur dichloride in 2018. it was distilled.
Recently I discovered that it it has yellow precipitate which reminds me of sulfur.
But if it is sulfur it is weird as a 2004 sciencemadness link suggest one of the sulfur chlorides can dissolve up to 67% of S8 by weight.
I am thinking of bubbling Cl2 into the sulfur chloride in the hopes that I can dissolve this yellow precipitate.
Is this a good plan?
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j_sum1
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In my limited understanding, sulfur chlorides have a limited shelf life. I would not be surprised to see S precipitate in dusulfur dichloride. What
else could it possibly be? (You should not see anything in SCl2)
You have the choice of using the liquid present (if it is sufficient for your needs) or of reacting the sulfur precipitate with Cl2 as you have
suggested – which is essentially the same as repeating the synthesis.
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6dthjd1
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Quote: Originally posted by j_sum1  | In my limited understanding, sulfur chlorides have a limited shelf life. I would not be surprised to see S precipitate in dusulfur dichloride. What
else could it possibly be? (You should not see anything in SCl2)
You have the choice of using the liquid present (if it is sufficient for your needs) or of reacting the sulfur precipitate with Cl2 as you have
suggested – which is essentially the same as repeating the synthesis. |
Do you think I must re-distill or use heat? I'd desire to avoid to do so as time has been a bit short for me recently
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j_sum1
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I guess it would depend on your procedure. If you have S precipitated then it would be logical to assume that what you have left is S2Cl2 and that
some Cl2 has escaped since 2018. If there is no possibility of impurities getting in then I don't think distillation would be needed. If your
procedure needs SCl2 then you will want to convert it by reaction with Cl2.
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Bedlasky
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| Quote: Originally posted by 6dthjd1 |
But if it is sulfur it is weird as a 2004 sciencemadness link suggest one of the sulfur chlorides can dissolve up to 67% of S8 by weight.
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I agree that this is quite strange. S2Cl2 reacts with sulfur to form dichloropolysulfanes SxCl2.
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