IIARTLEY ON CRLORSULPITIDB OF &IRl3ON. 1V.-On a Chlorsulphide of Carbon By WALTER NOELHARTLEE-. INthe preparation of a large quantity of dichloride of carbon tlr tetrachlorethjlene a solution of hydropotassic sulphide was used VOL xx. D HARTLEP ON CHLORBULPMDE OF CARBON. for reducing the terchloride of carbon according to the following equation :-The mode of operation was as follows :-To a mixture of the di- and terchlorides which contained as an impurity the protochlo- ride of carbon was gradually added the reducing agent prepared by dissolving potash in absolute alcohol and passing sulphuretted hydrogen through to saturation ; after warming slightly the re- action ceased and the reduced chloride of carbon was precipitated by water from its solution in the alcohol separated and distilled.There was a residue in the retort after distillation which had a brown colour and a remarkable smell suggestive of a sulphur compound. For examinatioii a portion was heated in a test-tube and the result was a sublimate of sulphur and fine needle-shaped cl*ystals. On digestion in alcohol the substance proved to be soluble and left on evaporation a deposit of brownish crystals. TOpurify this substance it was boiled in a flask with much alcohol and animal charcoal an inverted condenser being attached to prevent the waste of alcohol; the liquid after about four hours was filtered hot and allowed to cool in a porcelain basin; the crys- tals sere separated; and the alcohol was used again to extract what yet remained in the flask; a fresh crop of crystals formed and the alcohol with a little added to it was used again and again until the solid residue was exhausted.The substance not yet quite pure was again treated with alcohol and charcoal and the filtrate was allowed to evaporate spontaneously. The resulting crystals slightly yellow in dour were dried under the air-pump and submitted to analysis. The specimen beiug only small a8 little as possible was used. 0.109 grms. burnt with chromate of lead gave 0.0519 grrns. of carbonic acid corresponding to 00141 grms. of carbon or 12-93per cent. 0.115 grms. were burnt in a small combustion-tube with pure quicklime and oxygen was passed through the tube ; it was then while hot dipped cautiously into water as in an ordinary chlorine determination and treated with nitric acid.The solution yielded with nitrate of baryta 0.424 grms. of sulphate corresponding to 0.058 grms. of sulphur or 50*43per cent. On treating with nitrate of silver thc filtrate yielded 0.17 SLARTLEY ON CHLORSULPHIDE OF CARBON. grms. of chloride of silver corresponding to 0.042 grms. of chlorine or 36.52 per cent. Calculated for the Found by snalysis. formula Q2CI,S.;. C= 12.93 per cent. 12.56 C1 36.52 , 37.1'7 s 50.43 )) 50.26 99.88 ) 99-99 The formula deducible from these data is then €2C12S3 the name applicable under these circumstances being chlors u lp h o-form a body of the composition G2H2S,,being already known and called sixlphoform it being chloroform in which sulphur re-places chlorine.Chlorsulphoform crystallises from solii tions and by sublimatiou in fine needles possessing a disagreeable and peculiar smell soluble in alcohol and ether with difficulty; easily soluble in chloroform the bisulphide and the liquid chlorides of carllon and in oil of turpentine. Its melting-point is not below 250° C. andit begins to sublime before it melts. 'When it is treated with moderately strong uitric acid in sealed tubes for three or four hours at 120° to 130" C. white crystalline scales are formed of which 1 had not enough for analysis but from their contRiriing sulphur which fact I provcd and the nitric acid containing snL phuric acid they may be regarded as a substance with perhaps this formula G,Cl,SB,.The formation of the chlorsulphoform can be in no way explained except by supposing that the sulihr pro-duced in the reducing process just as it gains its state of freedom combines with the protochloride of carbon (G2Cl2). Facts sup-port this idea for if there be no G2Cl2 in the mixture to be reduced none of the new compound is formed and unless much sulphur be separated in the reaction we find the G2C12unacted upon; a solution of the hydropotassic sulphide alone has no action on it. I do not know that any other substance has been obtained by the actioq of nascent sulphur; if not this may be the first in- stance of the formation of a compound being attributed to such an agent. The subject of this paper is part of an unfinished research upon which I mas working last year in the laboratory of Professor K ol be.