IOWA ACADEMY OF SCIENCES. 
185 
We have now made alcohol from acetylene in two ways: 
1. By converting it to ethylene; this to ethyl sulphuric 
acid; and this to ethyl alcohol, and, 
2. By converting the acetylene to ethane; then to ethyl 
chloride; and then to alcohol. 
Before taking up a third synthesis, it may be of interest 
to consider briefly the red precipitate HC^C Cu. Cl Cu. 
obtrdned from the action of acetylene on the ammoniacal 
solution of cuprous chloride. It is an exceedingly unstable 
compound. If it is heated to 100° , it will explode violently; 
or, if it is dry, as slight a disturbance as touching it with a 
feather will sometimes cause it to decompose with an ex- 
plosion. If it is treated with hydrochloric acid, the 
acetylene will be released in a chemically pure state. This 
is one of the best methods of obtaining chemically pure 
acetylene. The reaction is given in the following equation; 
HC^C Cu. Cl Cu. +HC1=C2H2 + 2 CuCl. . . .(11). 
We shall now proceed to the consideration of a third 
synthesis, which is perhaps more nearly practical than any 
other yet devised. It is unique in that no reagents are 
consumed, which is a very extraordinary occurrence in a 
set of complicated reactions. 
It is known that acetylene is practically insoluble in 
water. If it were soluble, and if as it dissolved, it united 
chemically with the water, the reaction would be accord- 
ing to this equation. 
C2H2+H20=C2H40....(12). 
The C 2 H 4 0 being acetaldehyde, which, it will be noticed, 
is a very near approach to ethyl alcohol, being different 
from it only by containing two atoms less of hydrogen, 
which, if they could be added to acetaldehyde would give 
a reaction as represented in this equation: 
C2H40 + 2H =C2H50H ....(13). 
The equations, though so apparently simple, are 
extremely difficult to effect properly, there being a tend- 
ency toward the formation of by-products. The follow- 
