570 
DR. H. DEBUS ON THE CHEMICAL THEORY OF GUNPOWDER. 
K 2 S0 4 +4CO=K 2 S+4C0 2 
the volume of the gas would not be changed. But since potassic disulphide is formed, 
we have to base our calculations on equation 
2K 3 S0 4 +7 C 0=K 3 C0 3 +KoS 3 + 6 C0 3 
from which it follows that, if no carbonic oxide but only carbonic acid is produced, the 
volume of the entire gas will be diminished by yth of the volume of the carbonic oxide 
which in reality is formed. 
The greatest amount of carbon in gunpowders generally, as far as I know, is con¬ 
tained in the mixtures of Waltham Abbey, and these also produce the largest quantity 
of carbonic oxide, 3 mols. or 6 vols. for every 16 mols. of decomposed saltpetre. In 
addition to 3 mols. of carbonic oxide, 13 mols. of carbonic acid and 8 mols. of nitrogen 
are generated, which together amount to 24 mols. or 48 vols. of gas. 
Now, if in place of carbonic oxide, carbonic acid had been formed, the volume of 
the entire gas would have been 47*14 instead of 48 vols. In other words, if we frame 
our calculation on the assumption that only carbonic acid and no oxide has resulted 
from the combustion, we shall find for the English service powders 1*8 per cent, less 
gas than was actually obtained by experiment. And as other descriptions of powder 
contain less carbon than those of Waltham Abbey, in their case the error will be 
smaller than 1*8 per cent. If then we calculate the volumes of gas which mixtures 
of saltpetre, carbon, and sulphur in various proportions will produce, on the assumption 
that no carbonic oxide, but only carbonic acid is formed, we shall obtain numbers that 
will not differ much from the sum of the volumes of carbonic acid, carbonic oxide, 
and nitrogen produced by gunpowders containing corresponding quantities of saltpetre, 
carbon, and sulphur. 
By adding the coefficients of carbonic acid and nitrogen of equation (VIII.), and 
putting x—\ 6, and a= 0, we obtain for the sum, G, of the molecules of carbonic acid 
and nitrogen, which a mixture of 16 mols. of saltpetre, y atoms ot carbon, and z atoms 
of sulphur, by its complete combustion, can produce, the equation 
ri _ 160 + 20y+16a 
~28 
and for the volume, V 
r 160 + 202 / +16a 
V — 14 
In Bunsen and Schischkoff’s experiment 16 mols. of saltpetre, 13 3 atoms of carbon, 
and 6*3 atoms of sulphur were consumed in the formation of the chief products of 
combustion (page 562). The values y= 13*3, z= 6*3, placed in equation (IX.), give 
V= 37*62. Now 16 mols. of saltpetre, 13*3 atoms of carbon, and 6*3 atoms of sulphur 
correspond to 1977*2 parts by weight, and if these parts are expressed in grammes, then 
(IX.) 
