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^ given in the fifth column of the table. 



It is evident from an inspection of these values that 

 the velocity constant K^ falls below the average value at 

 the start. 



The amount by which it falls below the average value 

 will depend on the relation K^ -^ K^. When K^ and K^ 

 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^ will be 

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

 start.^^ This is easily shown by assuming various values^" 

 of Ki and K^. 



From this it follows that we can tell something about 

 K^ ~- K2 from the experimental values of K^. It is 

 evident that in the present case the experimental values 

 of K point to the relation £"2 -^ £"1 = 30 {ov K^-i- K2 = 

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

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

 in various mixtures of NaCl + CaCla- 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 £'i-4-£i = 30 as when Kt-~-Kt 

 = 30. With certain relations of Ki -h -ffz the constant K^ may be above 

 the average value at the start. 



"When the values of Ki and K, are changed, the concentrations of A 

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

 Ki -r- .Sl] if we wish the concentrations of A and M to remain constant 

 in the normal environment. 



" See Chapter IV. 



