2(AgCl,3NH3)
There are, therefore, three phases, viz. AgCl,3NH3; 2AgCl,3NH3, and NH3, in the one case; and 2AgCl,3NH3; AgCl, and NH3 in the other. These two systems are therefore univariant, and to each temperature there must correspond a definite pressure of dissociation, quite irrespective of the amounts of the phases present. Similarly, if, at constant temperature, the volume is increased (or if the ammonia which is evolved is pumped off), the pressure will remain constant so long as two solid phases, AgCl,3NH3 and 2AgCl,3NH3, are present, i.e. until the compound richer in ammonia is completely decomposed, when there will be a sudden fall in the pressure to the value corresponding to the system 2AgCl,3NH3—AgCl—NH3. The pressure will again remain constant at constant temperature, until all the ammonia has been pumped off, when there will again be a sudden fall in the pressure to that of the system formed by solid silver chloride in contact with its vapour.
The reverse changes take place when the pressure of the ammonia is gradually increased. If the volume is continuously diminished, the pressure will first increase until it has reached a certain value; the compound 2AgCl,3NH3 can then be formed, and the pressure will now remain constant until all the silver chloride has disappeared. The pressure will again rise, until it has reached the value at which the compound AgCl,3NH3 can be formed, when it will again remain constant until the complete disappearance of the lower compound. There is no gradual change of pressure on passing from one system to another; but the changes are abrupt, as is demanded by the Phase Rule, and as experiment has conclusively proved.[[152]]
The dissociation pressures of the two compounds of silver
chloride and ammonia, as determined by Isambert,[[153]] are given in the following table:—
| AgCl,3NH3. | 2AgCl,3NH3. | ||
| Temperature. | Pressure. | Temperature. | Pressure. |
| 0° | 29.3 cm. | 20.0° | 9.3 cm. |
| 10.6° | 50.5 ,, | 31.0° | 12.5 ,, |
| 17.5° | 65.5 ,, | 47.0° | 26.8 ,, |
| 24.0° | 93.7 ,, | 58.5° | 52.8 ,, |
| 28.0° | 135.5 ,, | 69.0° | 78.6 ,, |
| 34.2° | 171.3 ,, | 71.5° | 94.6 ,, |
| 48.5° | 241.4 ,, | 77.5° | 119.8 ,, |
| 51.5° | 413.2 ,, | 83.5° | 159.3 ,, |
| 54.0° | 464.1 ,, | 86.1° | 181.3 ,, |
| 88.5° | 201.3 ,, | ||
The conditions for the formation of these two compounds, by passing ammonia over silver chloride, to which reference has already been made, will be readily understood from the above tables. In the case of the triammonia mono-chloride, the dissociation pressure becomes equal to atmospheric pressure at a temperature of about 20°; above this temperature, therefore, it cannot be formed by the action of ammonia at atmospheric pressure on silver chloride. The triammonia dichloride can, however, be formed, for its dissociation pressure at this temperature amounts to only 9 cm., and becomes equal to the atmospheric pressure only at a temperature of about 68°; and this temperature, therefore, constitutes the limit above which no combination can take place between silver chloride and ammonia under atmospheric pressure.
Attention may be here drawn to the fact, to which reference will also be made later, that two solid phases are necessary in order that the dissociation pressure at a given temperature shall be definite; and for the exact definition of this pressure it is necessary to know, not merely what is the substance undergoing dissociation, but also what is the solid product of dissociation formed. For the definition of the equilibrium, the latter is as important as the former. We shall presently find proof of this in the case