144 
in a short time, and then it is, indeed, clear that we must exclusively 
look for the cause of this setting in of the equilibrium in the metal 
surface. 
In this it is supposed that the metal remains in contact with the 
liquid in which it-is polarized, or is transferred to a liquid in 
which the concentration of the M“-ions and electrons is smaller than 
in the liquid which is in electromotive equilibrium with the unary 
metal. In this case the reaction 
Mr Mi + v,Ór 
would have to cause a sufficient increase of the concentration of the 
MY-ions and electrons in a short time, so that these by deposition 
on the metal could reduce the latter to the state of internal equilibrium. 
In some cases, however, it will be possible to bring the metal in 
an electrolyte in which the concentration of the M“-ions and electrons 
is greater than in the liquid in electromotive equilibrium with the 
unary metal, and then, of course, the case is different, for then the 
M™ -ions and electrons will deposit on the metal without there being any 
necessity of the above-mentioned reaction taking place, and in this 
case the electrolyte will certainly be able to reduce the metal to 
the state of internal equilibrium in a comparatively short time. If 
in this way a sufficient quantity of baser ions is deposited, also the 
occurrence of local currents will greatly accelerate the establishment 
of the internal equilibrium. 
If, however, we do not make use of such a liquid, the electrolyte, 
as has been said, will have to be left out of account for a rapidly 
proceeding activation, and the setting in of the internal equilibrium 
takes place exclusively by transformations in the metal surface, in 
which the reaction: 
Mss gee en (Sal 
will take place, till the equilibrium corresponding to the unary metal: 
(M3 + 1,0) = (Ms! + 1,09) | i 
; , \" vd ee) ia festa lS 
or Ms A (0, = Ps 
has again set in. 
After anodic polarisation it is, therefore, the reaction (38«) that 
governs the setting in of the internal equilibrium, and speaking 
generally we may say that a metal can be thrown out of its state 
of internal equilibrium through the comparatively slow progress of 
the reversible reactions 
