| | PAGE |
| CHAPTER I |
| Introduction | [1] |
| General, I. Homogeneous and heterogeneous equilibrium,[5]. Real and apparent equilibrium, [5]. |
| CHAPTER II |
| The Phase Rule | [7] |
| Phases, [8]. Components, [10]. Degree of freedom. Variabilityof a system, [14]. The Phase Rule, [16]. Classification of systemsaccording to the Phase Rule, [17]. Deduction of the PhaseRule, [18]. |
| CHAPTER III |
| Typical Systems of One Component | [21] |
| A. Water. Equilibrium between liquid and vapour. Vaporizationcurve, [21]. Upper limit of vaporization curve, [23].Sublimation curve of ice, [24]. Equilibrium between ice andwater. Curve of fusion, [25]. Equilibrium between ice, water,and vapour. The triple point, [27]. Bivariant systems of water,[29]. Supercooled water. Metastable state, [30]. Other systemsof the substance water, [32]. B. Sulphur, [33]. Polymorphism, [33].Sulphur, [34]. Triple point—Rhombic and monoclinic sulphurand vapour. Transition point, [34]. Condensed systems, [36].Suspended transformation, [37]. Transition curve—Rhombicand monoclinic sulphur, [37]. Triple point—Monoclinic sulphur,liquid, and vapour. Melting point of monoclinic sulphur, [38].Triple point—Rhombic and monoclinic sulphur and liquid, [38].Triple point—Rhombic sulphur, liquid, and vapour. Metastabletriple point, [38]. Fusion curve of rhombic sulphur, [39].Bivariant systems, [39]. C. Tin, [41]. Transition point, [41].Enantiotropy and monotropy, [44]. D. Phosphorus, [46]. Enantiotropycombined with monotropy, [51]. E. Liquid Crystals, [51].Phenomena observed, [51]. Nature of liquid crystals, [52]. Equilibriumrelations in the case of liquid crystals, [53]. |
| CHAPTER IV |
| General Summary | [55] |
| Triple point, [55]. Theorems of van't Hoff and of Le Chatelier,[57]. Changes at the triple point, [58]. Triple point solid—solid—vapour,[62]. Sublimation and vaporization curves,[63]. Fusion curve—Transition curve, [66]. Suspended transformation.Metastable equilibria, [69]. Velocity of transformation,[70]. Law of successive reactions, [73]. |
| CHAPTER V |
| Systems of Two Components—Phenomena of Dissociation | [76] |
| Different systems of two components, [77]. Phenomena of Dissociation. Bivariant systems, [79]. Univariant systems,[80]. Ammonia compounds of metal chlorides, [82]. Salts withwater of crystallization, [85]. Efflorescence, [86]. Indefinitenessof the vapour pressure of a hydrate, [87]. Suspended transformation,[89]. Range of existence of hydrates, [90]. Constancyof vapour pressure and the formation of compounds, [90].Measurement of the vapour pressure of hydrates, [91]. |
| CHAPTER VI |
| Solutions | [92] |
| Definition, [92]. Solutions of Gases in Liquids, [93].Solutions of Liquids in Liquids, [95]. Partial or limitedmiscibility, [96]. Phenol and water, [97]. Methylethylketoneand water, [100]. Triethylamine and water, [101]. General formof concentration-temperature curve, [101]. Pressure-concentrationdiagram, [102]. Complete miscibility, [104]. Pressure-concentrationdiagram, [104]. |
| CHAPTER VII |
| Solutions of Solids in Liquids, only One of the Components being Volatile | [106] |
| General, [106]. The saturated solution, [108]. Form of thesolubility curve, [108]. A. Anhydrous Salt and Water.The solubility curve, [111]. Suspended transformation andsupersaturation, [113]. Solubility curve at higher temperatures,[114]. (1) Complete miscibility of the fused components. Ice assolid phase, [116]. Cryohydrates, [117]. Changes at the quadruplepoint, [119]. Freezing mixtures, [120]. (2) Partial miscibility ofthe fused components. Supersaturation, [124]. Pressure-temperaturediagram, [126]. Vapour pressure of solid—solution—vapour,[126]. Other univariant systems, [127]. Bivariant systems, [129].Deliquescence, [130]. Separation of salt on evaporation, [130].General summary, [131]. |
| CHAPTER VIII |
| Solutions of Solids in Liquids, only One of the Components being Volatile | [133] |
| B. Hydrated Salt and Water, (1) The compoundsformed do not have a definite melting point. Concentration-temperaturediagram, [133]. Sodium sulphate and water, [134].Suspended transformation, [137]. Dehydration by means ofanhydrous sodium sulphate, [138]. Pressure-temperature diagram,[138]. (2) The compounds formed have a definite melting point.Solubility curve of calcium chloride hexahydrate, [145]. Pressure-temperaturediagram, [149]. The indifferent point, [150]. Thehydrates of ferric chloride, [151]. Suspended transformation,[155]. Evaporation of solutions at constant temperature, [155].Inevaporable solutions, [157]. Illustration, [158]. |
| CHAPTER IX |
| Equilibria between Two Volatile Components | [161] |
| General, [161]. Iodine and chlorine, [161]. Concentration-temperaturediagram, [162]. Pressure-temperature diagram, [165].Bivariant systems, [167]. Sulphur dioxide and water, [169].Pressure-temperature diagram, [170]. Bivariant systems, [173]. |
| CHAPTER X |
| Solid Solutions. Mixed Crystals | [175] |
| General, [175]. Solution of gases in solids, [176]. Palladiumand hydrogen, [178]. Solutions of solids in solids. Mixedcrystals, [180]. Formation of mixed crystals of isomorphoussubstances, [182]. I. The two components can form an unbrokenseries of mixed crystals. (a) The freezing points of all mixtureslie between the freezing points of the pure components. Examples,[183]. Melting-point curve, [183]. (b) The freezing-point curve passesthrough a maximum. Example, [186]. (c) The freezing-pointcurve passes through a minimum. Example, [188]. Fractionalcrystallization of mixed crystals, [188]. II. The two componentsdo not form a continuous series of mixed crystals. (a) Thefreezing-point curve exhibits a transition point, [190]. Example,[190]. (b) The freezing-point curve exhibits a eutectic point, [191].Examples, [192]. Changes in mixed crystals with the temperature,[192]. |
| CHAPTER XI |
| Equilibrium between Dynamic Isomerides | [195] |
| Temperature-concentration diagram, [196]. Transformationof the unstable into the stable form, [201]. Examples, [203].Benzaldoximes, [203]. Acetaldehyde and paraldehyde, [204]. |
| CHAPTER XII |
| Summary.—Application of the Phase Rule to the Study of Systems of Two Components | [207] |
| Summary of the different systems of two components, [208].(1) Organic compounds, [212]. (2) Optically active substances,[213]. Examples, [216]. Transformations, [217]. (3) Alloys, [220].Iron—carbon alloys, [223]. Determination of the composition ofcompounds without analysis, [228]. Formation of minerals, [232]. |
| CHAPTER XIII |
| Systems of Three Components | [234] |
| General, [234]. Graphic representation, [235]. |
| CHAPTER XIV |
| Solutions of Liquids in Liquids | [240] |
| 1. The three components form only one pair of partiallymiscible liquids, [240]. Retrograde solubility, [245]. The influenceof temperature, [247]. 2. The three components can form twopairs of partially miscible liquids, [249]. 3. The three componentsform three pairs of partially miscible liquids, [251]. |
| CHAPTER XV |
| Presence of Solid Phases | [253] |
| A. The ternary eutectic point, [253]. Formation of compounds,[255]. B. Equilibria at higher temperatures. Formationof double salts, [258]. Transition point, [258]. Vapour pressure.Quintuple point, [261]. Solubility curves at the transition point,[264]. Decomposition of the double salt by water, [267]. Transitioninterval, [270]. Summary, [271]. |
| CHAPTER XVI |
| Isothermal Curves and the Space Model | [272] |
| Non-formation of double salts, [272]. Formation of doublesalt, [273]. Transition interval, [277]. Isothermal evaporation,[278]. Crystallization of double salt from solutions containingexcess of one component, [280]. Formation of mixed crystals,[281]. Application to the characterization of racemates, [282].Representation in space. Space model for carnallite, [284].Summary and numerical data, [287]. Ferric chloride—hydrogenchloride—water, [290]. Ternary systems, [291]. The isothermalcurves, [294]. Basic Salts, [296]. Bi[2]O[3]—N[2]O[5]—H[2]O, [298].Basic mercury salts, [301]. Indirect determination of the compositionof the solid phase, [302]. |
| CHAPTER XVII |
| Absence of Liquid Phase | [305] |
| Iron, carbon monoxide, carbon dioxide, [305]. |
| CHAPTER XVIII |
| Systems of Four Components | [312] |
| Reciprocal salt-pairs. Choice of components, [313]. Transitionpoint, [314]. Formation of double salts, [315]. Transitioninterval, [315]. Graphic representation, [316]. Example, [317].Ammonia-soda process, [320]. Preparation of barium nitrite, [327].Barium carbonate and potassium sulphate, [328]. |
| APPENDIX |
| Experimental Determination of the Transition Point | [331] |
| I. The dilatometric method, [331]. II. Measurement ofthe vapour pressure, [334]. III. Solubility measurements, [335].IV. Thermometric method, [337]. V. Optical method, [338].VI. Electrical methods, [338]. |
| |
| Name Index | [341] |
| |
| Subject Index | [345] |