CHEMISTRY — AGREE. iS/ 



tions of a quinone group with a salt of a phenol, or with an aniline-like group, 

 and the mechanical change from one to the other, or a corresponding move- 

 ment of electrons, is very probably connected with the color changes. A 

 small amount of color is, of course, due to the quinone group. 



Studies in Catalysis: (i) On the Hydrolysis of Amides by Acids. 

 (American Chemical Journal, j8, 489-507.) (2) On the Reactions of 

 Carbonyl Compounds with Hydroxylamine and Hydroxylamine Hydro- 

 chloride. (American Chemical Journal, jp, 300-309.) 



(i) In the first of these articles is the report of a quantitative study of 

 the hydrolysis of acetamide by hydrochloric acid. The experimental and 

 mathematical evidence shows clearly that neither the amide nor the undis- 



sociated amide hydrochloride is readily decomposed, but that the amide 



-1- 

 cation, CH3CONH3, is the chief substance hydrolyzed. Similar reactions 

 take place in the saponification of esters and amides by alkalies. 



RCONH3 + H,0(or H + OH) m-->^ RC(0H),NH3 m^ RCOOH + NH, 



RCONH, + K + OH ^-> RCO(OH)NH, + K ^-*- RCOO + K + NH3 



This theory enables us to predict that other substances, such as alcohols, 

 mercaptans, hydroxylamine, etc., should also react with the amide cation. 

 Dr. E. E. Reid has been able to show that excellent yields of esters may 

 be formed from alcohols and amides, anilides, and hydrazides in the presence 

 of acids. It was found that certain salts accelerate these catalytic reactions 

 while other salts retard them : the cause of this salt catalysis is being investi- 

 gated. We are making a study of the reverse reactions, the formation of 

 amides, anilides and hydrazides from the esters, or acids, and ammonia, 

 amines, hydrazines, etc. 



CH3COOR+NH3 (or H -f NH, or NH, + NH,) ^->- CH,CONH,+ ROH. 



(2) In the study of the reactions of carbonyl compounds with hydroxyla- 

 mine and its salts it has been established that the reaction between free 

 hydroxylamine and acetone proceeds nearly to completion with a velocity 

 which, though somewhat slow, is readily measured. When acids are added 

 this reaction velocity is very greatly increased and the process, instead of 

 going to completion, shows itself to be reversible, the equilibrium point de- 

 pending upon the amount of acid added. This is the first experimental 

 disproof of the so-called law of catalysis postulating that the equilibrium 

 point of a catalyzed reaction does not vary with a change in the concentration 

 of the catalyzer. 



