MECHANISM OF PROCESS OF DEATH 63 



pose the calculated values given in the third column of 

 Table I, we obtain the values of the velocity constant 

 K 3 given in the fifth column of the table. 



It is evident from an inspection of these values that 

 the velocity constant K 3 falls below the average value at 

 the start. 



The amount by which it falls below the average value 

 will depend on the relation K l -r- K 2 . When K and K 2 

 are nearly equal, the velocity constant falls a good deal 

 below the average value at the start, but as the difference 

 between them is increased the velocity constant K 3 will be 

 found to fall less and less below the average level at the 

 start. 35 This is easily shown by assuming various values 36 

 of K l and K 2 . 



From this it follows that we can tell something about 

 K 1 -f- K 2 from the experimental values of K 3 . It is 

 evident that in the present case the experimental values 

 of K point to the relation K 2 -=- K l = 30 (or K l --K 2 = 

 30). This relation was actually assumed by the writer, in 

 order to fit, not the NaCl curve, but antagonism curves 37 

 in various mixtures of NaCl + CaCl 2 . It is therefore a 

 striking confirmation of the general correctness of the 

 underlying assumption that we are also able by means of 

 this assumption to fit the NaCl curve so closely. 



In general, where a chemical reaction is slower at 

 the start than is expected, we may suspect that we have 



" It should be noted that we get the same result (as .regards K, falling 

 below the average at the start) when .K^ -^ ITj = 30 as when JBT, ~ K t 



= 30. With certain relations of K^ -+- K 2 the constant K 3 may be above 

 the average value at the start. 



M When the values of K^ and K 3 are changed, the concentrations of A 

 and M must also be changed in such a way that Cone. A +- Cone. M = 

 K! -f- Kt if we wish the concentrations of A and M to remain constant 

 in the normal environment. 



87 See Chapter IV. 



