File:The phase rule and its applications (1911) (14596131657).jpg

Identifier: phaseruleitsappl00find (find matches)
Title: The phase rule and its applications
Year: 1911 (1910s)
Authors: Findlay, Alexander, 1874-
Subjects: Phase rule and equilibrium Solution (Chemistry) Chemistry, Physical and theoretical
Publisher: London, New York, Longmans, Green
Contributing Library: Mugar Memorial Library, Boston University
Digitizing Sponsor: Boston University

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rightangles to one another along which could be measured thevalues of pressure, temperature, and concentration of the com-ponents in the solution. Instead of this, however, there maybe employed the accompanying projection figure 2 (Fig. 43),the lower portion of which shows the projection of the equili-brium curve on the surface containing the concentration andtemperature axes, while the upper portion is the projection onthe plane containing the pressure and temperature axes. Thelower portion is therefore a concentration-temperature diagram; 1 Ramsay and Young, Journ. Chem. Soc, 1886, 49. 458. 2 Vant Hoff, Lectures on Physical Chemistry, T. p. 77 (. (Arnold). TWO VOLATILE COMPONENTS 169 the upper portion, a pressure-temperature diagram. The corre-sponding points of the two diagrams are joined by dottedlines. Corresponding to the point C, the melting point of pureiodine, there is the point C, which represents the vapourpressure of iodine at its melting point. At this point three liquid
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Fig. 43. curves cut: I, the sublimation curve of iodine; 2, the vapori-zation curve of fused iodine; 3, CiB^ the vapour-pressurecurve of the saturated solutions in equilibrium with solidiodine. Starting, therefore, with the system solid iodine—liquidiodine, addition of chlorine will cause the temperature of equili-brium to fall continuously, while the vapour pressure will firstincrease, pass through a maximum and then fall continuously 170 THE PHASE RULE until the eutectic point, B (B^, is reached.1 At this point thesystem is invariant, and the pressure will therefore remainconstant until all the iodine has disappeared. As the concen-tration of the chlorine increases in the manner represented bythe curve B/H, the pressure of the vapour also increases asrepresented by the curve B^H^ At Hj, the eutectic point foriodine monochloride and iodine trichloride, the pressure againremains constant until all the monochloride has disappeared.As the concentration of the solution passes along the

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