186 
IOWA ACADEMY OF SCIENCE 
CHs 
CHs 
NO, 
+ 4NH3 
Cl 
NO3 
— > 
\/c=o 
S02C1 
+ 2NH4C1 
so 
0=0 
^ N • NH4 
A suitable amount of the acid chloride was placed in an open 
beaker and treated with concentrated ammonia. Apparently 
there was no action in the cold, but on raising the temperature 
slowly to boiling, so as to keep the concentration of the am- 
monia as high as possible, the acid chloride dissolved. When 
the excess of ammonia was evaporated off and the residue was 
cooled somewhat, the ammonium salt of the imide crystallized 
out as small glistening cubes. These were recrystallized from 
water several times. They then gave a melting point, with de- 
composition, of 3 10° -320°. 
Total nitrogen was determined by the modified Gunning meth- 
od, and sulphur by the Liebig method. Ammoniacal nitrogen 
was determined by dissolving a weighed portion of the salt in 
water in a Kjeldahl fiask, adding 30 cc. of strong sodium hydrox- 
ide, and distilling into .IN hydrochloric acid. 
.2193 g. ammonium salt required 23.41 cc .1084N hydro- 
chloric acid. 
.1950 g. ammonium salt required 20.80 cc .1084N hydro- 
chloric acid. 
For ammoniacal nitrogen — 
.3002 g. ammonium salt required 11.00 cc .1088N hydro- 
chloric acid. 
.1674 g. ammonium salt gave .1509 g. barium sulphate. 
Theory for CgHgOgNgS Found 
Total nitrogen, 16.21 per cent. 16.20 - 16.18 per cent. 
Ammon, nitrogen, 5.40 per cent. 5.58 per cent. 
Sulphur, 12.35 per cent. 12.38 per cent. 
The Imide. 
1-2 
CO 
NOa • CH3 • CeH,/ ^NH 
SO, 
When the cold mother liquor from the crystallization of the 
ammonium salt of the imide is made acid with hydrochloric 
