If we assume that the complex is decomposed so fast as to supply new silver ions rapidly enough, to allow us to consider the precipitation of silver and silver sulphide as direct actions of the silver ions, then we may, conservatively, consider T_{Decomposition} to be about 1 / 100 second. Then T_{Formation} would be only 1 / 10^{24} second. Considering the limiting results for the dimensions of atoms (and ions) and taking account of the fact that the formation of the complex ‹involves electrical changes›, that is, in modern terms, changes in position of electrons,[470] Haber finds, that to satisfy the above value for the time constant, such changes must involve a motion of electrical charges at a speed about a million times as great as the velocity of light. Such a velocity is, unquestionably, incompatible with our knowledge of the velocities of light and of electrical charges. We must draw the conclusion that ‹the complex argenticyanide-ion probably cannot decompose fast enough into its ions›, to enable the latter to be the ‹only› components which make it possible to precipitate silver sulphide or metallic silver from its solutions[471] (see above, p. 232). That would make it necessary to assume ‹direct action› [p235] (as given in equation II, p. 232) ‹between the complex› and the ‹precipitating agent›, to some extent, at least, the extent being dependent on the concentrations involved in a given case. If further investigations should confirm such a view, we would probably find that ‹both› the actions under consideration (equations I and II, p. 232) must proceed ‹simultaneously›. The second one would have the advantage of enormously greater concentrations of the reacting components, ‹e.g.› of the complex ion; the first one would, probably, be found to have the advantage of an enormously greater velocity constant. The actual velocities of the two reactions have never been measured[472] and no final explanation of the relations can be offered. The problem is a very important one, involving the whole question of the mode of ionic action (‹cf.› Chap. V, especially p. 83). Aside from the theoretical value of the problem that has been raised, the question of immediate moment to us, from the point of view of analytical chemistry, is the question whether such conclusions would invalidate, in any way, the use we have made of the theory of complex ions, in elucidating the question of the precipitation and nonprecipitation of salts of simple ions from solutions of their complex ions.