. An introductory course of lessons and exercises in chemistry (rewritten 1919). als increases withits concentration until the two are equal: then we have equili-brium. Crystals are then neither dissolved nor formed (or lookedat in another way, just as much of the crystals is dissolved persecond as is separated from the solution in the same time). The experiment also shows the effect of temperature upon thisequilibrium:—it shows that, at higher temperatures, equilibriumrequire? more of the potassium nitrate to be present in the solu-tion. We say, technically:—the equilibrium has been shiftedto
. An introductory course of lessons and exercises in chemistry (rewritten 1919). als increases withits concentration until the two are equal: then we have equili-brium. Crystals are then neither dissolved nor formed (or lookedat in another way, just as much of the crystals is dissolved persecond as is separated from the solution in the same time). The experiment also shows the effect of temperature upon thisequilibrium:—it shows that, at higher temperatures, equilibriumrequire? more of the potassium nitrate to be present in the solu-tion. We say, technically:—the equilibrium has been shiftedtoward the solution side, meaning thereby that relatively less ofthe potassium nitrate will remain as crystals. This shift is iden-tical in sense with the temperature shift of the first example ofequilibrium. Why ? 12. Relation Between Solubility and Temperature. The foregoing experiment showed an example in which the sol-ubility of the solid increases with temperatures. From our generalexperience in this world, we are likely to jump at the conclusion Chapter IV 49 iSOr 140. O 1CP 30° 50° 40 5CT bO° 70° 80° 90° 1009 JLl :?_: :: 72-_ Chapter V 51 CHAPTER V. A REVERSIBLE CHEMICAL REACTION—THIRD ILLUSTRA-TION OF EQUILIBRIUM. 1. Introduction. For the first two illustrations of equilibrium, we presentedchanges which are as simple as any that could be secured—thevaporization of a liquid, and the dissolution of a solid. Thesechanges are usually spoken of as physical changes; but since theforces of nature are not limited, in their application, by theboundaries set by man between the domains of physics and chem-istry, these illustrations show the same relations and forces thatare shown by strictly chemical changes. However, for the next, more complicated example, we shallpresent a purely chemical phenomenon. But before the equili-brium conditions can be considered, some of the experimental datamust be presented separately. These data also are important ontheir own account. 2
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