742 
ME. C. GEEVILLE WILLIA3IS OS S0:ME OE THE PEODUCTS 
The formula requires — 
12 volumes of carbon vapour . . =:0-8290 x 12 = 9-9480 
24 volumes of hydrogen .... =0-0692x24=1-6608 
11-6088 
= 2-9022 
4 
The excess is partly due to the extra pressure*, but chiefly to the presence of a little 
The fluid procured in this manner is therefore caproylene or hexylene. Its forma- 
tion by the process detailed is interesting, because it is an instance of the regeneration 
of a hydrocarbon by means of a complex decomposition similar to that found by 
MM. Beethelot and De Luca to occur with propylene. The hexylene is not there- 
fore a mere product of decomposition in the ordinary sense of the term, but is identical 
in kind with the fluid in the naphtha which yielded the bromine compound. This is 
proved by the identity of boiling-point. The naphtha distilled between 71° and 77°, 
and the hexylene produced from it boiled at 71°. 
Hexylene was discovered by FEEMvf among the products of the distillation of hydro- 
leic and metoleic acids. 
Bouis found that chloride of capryle treated with sodium in the cold yielded capryle. 
but that if the reaction took place with heat, caprylene resulted. It appearing probable 
from this that the products of the action of sodium on the bromine compounds would 
vary with the temperature, I repeated my experiments with the necessai-)' precautions. 
With the view of obtaining the next homologue of hexylene, the fi-action boiling 
between 82° and 88° was selected. About twelve ounces of bromine were satui-ated 
with naphtha in the same manner as before, but, during the treatment of the bromi- 
nated oil mth sodium (after the action of alcoholic potash), all rise of temperatui-e was 
carefully avoided, the apparatus being constantly covered with cold water. The decom- 
position is of course more gradual than when heat is applied, but it is quite as perfect. 
* I have been occupied at intervals during the last two years in ascertaining the amount of influence exer- 
cised by pressure on vapour volume, and also in endeavouring to improve the processes generally used for 
determining the densities of vapours. I hope before long to coimnunicate these results to the Societv'. In 
the meantime some values obtained with propyle are annexed, to give an idea of the extent to which the 
density is increased by pressure. 
Vapour -density of Propyle at various pressures. 
Theory 2-976=4 vohmies. 
Temperature. 
Pressure. 
Density. 
100-0 
772-1 
2-963 
97-0 
870-6 
3-005 
97-0 
943-8 
3-022 
98-7 
1013-0 
3-032 
+ Ann. de Chim, et de Phys, Ixv. 139. 
