of Chlorine and Carbon, &c. 347 
used. . Other experiments gave very nearly the same results ; and 
I have deduced from them, that one volume of olefiant gas re- 
quires five volumes of chlorine for its conversion into muriatic 
acid and chloride of carbon; that four volumes of muriatic acid 
gas are formed; that three volumes of chlorine combine with 
the two volumes of carbon in the olefiant gas to form the solid 
crystalline chloride; and that, when chlorine acts on the fluid 
compound of chlorine and olefiant gas, for every volume of chlo- 
rine that combines, an equal volume of hydrogen is separated. 
I have endeavoured to verify these proportions by analytical 
experiments. The mode I adopted was, to send the substance 
in vapour over metals and metallic oxides at high temperatures. 
Considerable care is requisite in such experiments; for if the 
process be carried on quickly, a portion of fluid chloride of car- 
bon is formed, and escapes decomposition. The following are 
two results from a number of experiments agreeing well with 
each other. 
Five grains were passed over peroxide of copper in an iron 
tube, and the gas collected over mercury; it amounted to 3:9 
cubic inches, barometer 29°85; thermometer 54° Fahr. Of 
these nearly 3:8 cubic inches were carbonic acid, and rather 
more than 1 of a cubic inch was carbonic oxide. These are 
nearly equal to +5004 of a grain of carbon. Hence, 100 of the 
chloride would give 10 of carbon nearly, but by calculation 100 
should give 10:19. The difference is so small as to come within 
the limits of errors in experiment. 
Five grains were passed over peroxide of copper in a tube 
made of green phial glass, and the chlorine estimated in the same 
manner as before. 17°7 grains of chloride of silver were obtained 
equal to 4°36 grs. of chlorine. This result approaches much 
nearer to the calculated result than the former ; but there had 
still been action on the tube, and a minute portion of the sub- 
stance had passed undecomposed, and condensed at the opposite 
end of the tube in crystals. 
Experiments made by passing the perchloride over hot lime 
or barytes, promise to be more accurate and easy of performance. 
In the mean time, the above analytical results will, perhaps, be 
considered as strong corroboration of the opinion of the nature 
of the compound, deduced from the synthetical experiments 5 
and the composition of the perchloride of carbon will be 
Three proportions of chlorine «+ «2 = 100°5 
Two dittocarbon .«. «+ ee oe =II'4 
' 111-9 
Protochloride of Carbon. 
Having said so much on the nature of the perchloride of car- 
Xx 2 bon, 
