VELOCITY OF REACTION. HETEROGENEOUS SYSTEMS 1 09 



giving the observed concentrations compared with cal- 

 culated values; z gives the time of reaction, t the temper- 

 ature, q the quantity added, i.e. the inverse value of the 

 velocity v. 



As will be seen from these figures the formula may be 

 well used in this case. We observe also that the magnitude 

 /i increases with decreasing time of reaction. With a pro- 

 longed reaction-time, the quantities of ammonia used do 

 not exceed very much the quantity necessary for 

 total haemolysis and then our premises are not fulfilled. 

 Hence the real value of /<&, corresponding to the theo- 

 retical premises, is that to which the values of ^ converge 

 with decreasing time of reaction. It does not seem to 

 differ very much from that valid for z = 10 min. The appli- 

 cability of the known equation from physical chemistry for 

 even longer times renders it highly probable that it would 

 hold for the limit-value, which would be reached in an ex- 

 ceedingly short time of observation, if it were possible to 

 observe it directly. In heterogeneous systems the direct 

 observation of the velocity of reaction meets in most cases 

 with great difficulties, as has been indicated above, so 

 that the indirect observations such as those executed by 

 Madsen, Noguchi, and Walbum are necessary to obtain 

 a knowledge of these phenomena. I therefore reproduce 

 the values of p found by them for different bases and 

 acids. The interval of temperature was always between 

 about 17 and 39 C. The experiments were arranged in 

 the same manner as those dealing with ammonia. 



These figures give occasion to remarks similar to those 

 made regarding the behaviour of ammonia. If we could 

 carry out experiments extended through a very long time, 



