versible transformation are above oo ; starting from 2 7 . 1 2 percent of nickel, the transformation point for cooling lies below oo,the value for 29.94 percent nickel lying below, - 7 8 O . At 25.84 percent nickel, there occur poiiits both of reversible a11d of irreversible transformation, tlie teniperatnre at which the reversible change takes place rising with increasing percentage of nickel. 1V. D. B.
Solubility of benzophenone. E. De17 z'eii. c o m j f e s i-endzs, 130,;zr (1900). W. D. B - Isolated solubility determinations in ahout twenty solvents.
On the liquefaction of mixtures of carbon dioxide and sulphur dioxide. 1". C a i ~ b r t . C O I I E / Arendrts, ~S 130, S A ' (1900). - The author has determilied the boiling-point and dew-point curtes for a number of mixtures of carbon dioxide and sulpliur dioxide. A11 mixtures show retrograde condensation. 117. D. B.
Po&- Coi~ijonenfS ~ ~ s f e i n s Action of hydrogen on antimony sulphide. 27.PJlabon. Coi~~flfesi.endus, 130, 911 (1900).-The author has studied the reaction Sb,S, 3H, 2Sb 7 311,s. At 440" both the antiniony and the sulphide are solid and the ratio of the two gases is found to be independent of the absolnte amouyt of the two solid pliases. At 610" the snlphide of atltitnotiy is liquid a n d dissolves tlie metallic antimony. The ratio of the gases varies with the amount of antimony until so mucli is IV. D. B. added that antimony separates as solid phase.
+
Solubility of a mixture of salts having a common ion. C. tower^. Coiitpfes reidus, 130, 90S,zzzz (1900).-The autlior lias determined isotherms for potassiuni nitrate and chloride, for potassium nitrate a n d bromide, and for potassiam chloride and bromide in aqueous solutions. Equivalent quantities of potassium cliloride a n d of potassiuni bromide have exactly the same effect on the solubility of the potassium nitrate. Potassiuni bromide and chloride give one continuous curve instead of tv,o intersectiiig curves. T h e autlior is perfectly clear as to the theoretical significance of this. llf. D. B, ' Note on partially miscible aqueous inorganic solutions. J . S. N e z d h . J o u ~Chein. . SOL.77,; ;7 (1900 ) - Saturated potassium carbonate and strong aqueous atnnioiiia form two liquid la) ers, aiid the temperatures at which these phases heconie identical vary with the aniount of water present. bv. D. B.
Chemical reactions produced in a solution ; vapor-pressure of the solvent. 130, ;Sz i~goo). --h cyclical proof to show that, at constant pressure and teniperatnre, a reversible reaction alwaj s increases tlie vapor-prewire of the solvent. provided the solvent takes 110 part in the reaction, Tliis is interesting, of course, but one cannot help wondering wlietlier it woulcl hold true for the clialige of paraldeliyde into acetaldehyde, for instance, or for the reaction between alcohol and acetic acid in benzene solution. I t is very easy to overlook things even i n the simplest thermodynamic proof. W . D.B.
A.POZFO~. Coirz.bPfes mndus,
Limited chemical reactions in homogeqeous systems. A.Ponsol. Comjtes ~ . e n d ~130, ~ s , $29 (1900).- The author shows that the equilibrium in a hornogeiieoiis gaseous mixture is independent of tlie nature arid concentration of snbstances not entering into the reaction. H e also claims that, at equilibrium, the
150
Reviews
volume is a minimuin for constant pressure and temperature, wliicli is certainly not true. The author further deduces Valson’s law of the nioduli, ostensibly without use of the electrolytic dissociatioii hypothesis, though, as a matter of fact, he postulates the acid and basic radicals as independent constituents.’
1v.D. L’. The combination of sulphur dioxide and oxygen. E. J . R m s c l l and A? Smith. Jour. Chem. SOC.77, 340 (rgno).-The following coiiclusioiis were drawn : I. \Vlien a mixture of sulphur dioxide and oxygen is allowed to stand over certain metallic oxides at the ordiiiary temperature, conil~inationtakes place to a certain extent between the two gases, owing to the “ surface action ” exerted by the metallic oxide. 2. I f i t h the same oxide, the amount of the sulphur trioxide formed depends on the extent of the surface of the oxide. 3. With the same oxide, this amount clepends also on the state of the surface. I t appears to be least with freshly precipitated oxides which are not yet dried, and to increase if the oxide has been nioderately heated or kept for a long time so as to become dry. 4. The aniount appears to be absolutely depeiideiit on a simultaneous combination of the oxide with the sulphur dioxide, and in fact seems to proceed concurrently with this. . 5 . The most striking instance of this surface action is afforded by manganese peroxide, some twenty percent of the sulphur dioxide being converted into sulphur trioxide If the materials are carefully dried by mentis of phosphorus pentoxide, no combination takes place as, even after standing several days, no change in rolunie can be detected. By drying the mixture, combination of manganese dioxide and stilfur dioxide is thus prevented, as is also the surface action of the oxide wliicli brings about the unionof sulphur dioxide and oxygen. 6. \\’hen sulpliur dioxide and oxygen are p a d over heated platinized pumice, combination diminishes as the materials are more cotiipletely dried, and can be made very small. 1v. D. 6.
..
Influence of the nascenf state on the combination of dry carbon monoxide and 77,36r (rpoo).-Pure carbonyl suloxygen. E . J . Russell. Jour-. Chern. SOC. phide will not explode if sparked with oxygen. With a small amount of mipurity, some carbonyl sulphide is decomposed into carbon monoxide and sulphur, witliout these substances reacting with the excess of oxygen. The same thing is true of mixtures of carbonyl sulphide and nitrous oxide. The state of affairs following 011 a violent reaction - such as explosion of carbon disulphide or chlorine monoxide- has a considerable influence in bringing about a combination of carbon monoxide and oxygen, but there is no satisfactory proof that nascent carbon monoxide differs appreciably from the ordinary gas.
UT.D. B. The decomposition of chlorates. U’. H. Sodenu. Jour. Ckem. SOC. 77, r.37, 77 ‘ (r9ao). -The author’s experiments are explained by him on the assumption of two independent reactions, the evolution of oxygen, and the evolution chlorine and oxygen. With potassium chlorate there are only traces of
