Carbon disulphide density

Phosphorus(III) oxide dissolves in several organic solvents, for example benzene, carbon disulphide the molecular weight in these solvents corresponds to the formula P40(, as does the density of the vapour, and the structure is ... 

The increase in the solubility of bromine in soln. of ammonium salts is very marked, as is also the case with the alkali chlorides. The case with the alkali bromides is specially interesting. The solubilities by F. P. Worley are indicated in Table IX. The marked increase in the solubility of bromine in soln. of potassium bromide was attributed by M. Roloff to the formation of molecules of KBr3. He shook up a soln. of bromine in carbon disulphide with water and with an aq. soln. of potassium biomide, and measured the concentration of the bromine in the two layers. M. Wildermann has shown that the density of bromine vapour over a soln. of potassium bromide sat. with bromine is the same as over water sat. with bromine, indicating that the cone, of the free bromine in all the aq. soln. is the same, and any excess in the presence of potassium bromide must be united with the potassium bromide. All the bromine dissolved by a soln. of potassium bromide can be removed... 

Carbon disulphide vapour appears to be associated to a small extent. When the vapour and ether vapour are mixed at constant volume at 80° C. under atmospheric pressure, the increase of pressure observed indicates previous association of the carbon disulphide to the extent of 0-14 per cent., whilst vapour density determinations by Dumas method give results corresponding with 2 per cent, association.3... 

Thiocarbonyl Tetrachloride, Carbon Tetrachlorosulphide, or Trichloromethyl Sulphur Chloride, CSC14 or C13C.SC1.—Thiocarbonyl tetrachloride may be prepared by the action of dry chlorine on dried carbon disulphide in the presence of iodine.2 It is a golden-yellow liquid, with an intensely disagreeable odour it attacks the eyes and respiratory organs. Its density is 1-722.3 It boils at 149° C.4... 

Monoclinic selenium has a density of 4-44 3 at 0° C. It is only sparingly soluble in carbon disulphide, giving a red solution. When heated rapidly it melts at 170° to 180° C., but transformation into metallic selenium commences to occur slowly near 120° C.4 The liquid obtained by rapid heating passes into the vitreous condition when cooled. 

It is a very deep red liquid having a density of 3-60 at 15° C. its odour is unpleasant. It is soluble in carbon disulphide and in chloroform and is, in its turn, a solvent for selenium. When heated, partial decomposition occurs, with formation of bromine and the tetrabromide, distillation taking place at 225° C. 

Arsenic Pentiodide ( ), Asls.—When a mixture of arsenic and iodine in the requisite proportions is heated in an atmosphere of carbon dioxide in a sealed tube at 150° C., a brown crystalline product is obtained.3 The crystals, which melt at 70° C. and have density 3-93, are soluble in water, carbon disulphide, alcohol, ether and chloroform. The solution in carbon disulphide yields, when allowed to crystallise, a mixture of arsenic triiodide and iodine. The latter is readily lost from the pentiodide, and heating at 100° C. in nitrogen in a sealed tube brings about the decomposition. Like the triiodide, the pentiodide dissolves boron tribromide.4... 

Many of these solvents, e.g., carbon disulphide, amyl alcohol, amyl acetate, ether, benzene, etc., may be easily identified—especially if unmixed with other solvents—by their odour, density, b.pt. and various reactions (see chapter on Chemical Products, Vol. I, and Tables XXXV and XXXVI, opposite.)... 

Analyses of the purified compound by G. Lemoine, G. Ramme, H. Schulze, J. Mai and F. Schaffer, L. Wolter, and A. Stock and co-workers are in agreement with the formula P4S3. G. Lemoine found that the fractional crystallization and fractional sublimation of the tetritatrisulphide gave no evidence of a heterogeneity. The vap. density determinations of G. Ramme, G. Lemoine, F. Isambert, A. Helff, and A. Stock and H. von Bezold are in agreement with this formula, so also is the mol. wt. calculated from the effect of this sulphide on the b.p. of carbon disulphide by A. Helff, and A. Stock and H. von Bezold. The fused product appears as a... 

The melting-point of the commercial sulphide was 255° C.2 and that of the recrystallised product 275° to 276° C.3 The melting-point was raised to 284° to 291° C. by repeated recrystallisation from carbon disulphide.4 Boiling occurs with partial decomposition at 513° to 515° C.4 Other values which have been found are 520° C.,5 523-6° C.e The sulphide distils in a water-pump vacuum at 332° to 340° C., probably with considerable dissociation (see Vapour Density ).7... 

The triamide, SP(NH2)s, was prepared by saturating PSC13 with ammonia. It was a white solid of density 1-7. When heated it dissociated into ammonium sulphide and sulphur, leaving phosphorus in the residue, probably as phospham, and was decomposed by warm water giving H2S and ammonium thiophosphate. It was only slightly soluble in alcohol or carbon disulphide. 

The density of the hydride is 0-92,8 and the vapour-tension for each interval of 10° between 300° C. and 410° C. is 15, 17, 21, 27, 38, 55, 87, 186, 201, 285, 396, and 540 mm. respectively.7 Sodium hydride is the most stable of the alkali-metal hydrides, and caesium hydride the least. The sodium derivative is unaffected by dry air, but decomposes in presence of traces of moisture. Although insoluble in organic solvents such as carbon disulphide, carbon tetrachloride, benzene, and turpentine, it dissolves in the alkali-metals and their amalgams. 

Subsulphides.—Several supposedly subsulphides of iron have been described from time to time, namely FeJS,6 Fe2S,6 and Fe4S3. The last-named is produced when iron is heated m an atmosphere of carbon disulphide vapour, at 1300° to 1400° C., and allowed to cool in the disulphide vapour.7 It is a crystalline body of density 6 96, and soluble in dilute mineral acids. evolving hydrogen sulphide and hydrogen. It does not alter when exposed to air, and is oxidised only with difficulty. 

The volume changes on mixing non-aqueous liquids, the densities of mixed liquids, of solutions of non-polar solutes in non-polar solvents, and the changes of total volume on the solution of solid salts in water, noticed at an early period and much investigated, can only be mentioned here some aspects of these will be dealt with later. Hyde found the densities of solutions of jp-nitrotoluene in carbon disulphide smaller than the density of either component, but the anomaly disappears if the p-nitrotoluene is supposed to be in the liquid state. Biron found that the volume change on mixing two liquids was Av=kx( —x where x , (1— ) are the mol fractions, and he investigated the effect of pressure on the value of Av. The apparent specific volume of alcohol in aqueous mixtures was determined by Brown, lo... 

In this contribution the concept of instantaneous normal modes is applied to three molecular liquid systems, carbon monoxide at 80 K and carbon disulphide at ambient temperature and two different densities. The systems were chosen in this way because pairs of them show similarities either in structural or in dynamical properties. The systems and their simulation are described in the following section. Subsequently two different types of molecular coordinates are used cis input to normal mode calculations, external, i.e. translational and rotational coordinates, and internal, i.e. vibrational coordinates of strongly infrared active modes, respectively. The normal mode spectra are related quantitatively to molecular properties and to those of liquid structure and dynamics. Finally a synthesis of both calculations is attempted on qualitative grounds aiming at the treatment of vibrational dephcising effects. 

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