Carbon disulfide boiling point

Carbon disulfide is completely miscible with many hydrocarbons, alcohols, and chlorinated hydrocarbons (9,13). Phosphoms (14) and sulfur are very soluble in carbon disulfide. Sulfur reaches a maximum solubiUty of 63% S at the 60°C atmospheric boiling point of the solution (15). SolubiUty data for carbon disulfide in Hquid sulfur at a CS2 partial pressure of 101 kPa (1 atm) and a phase diagram for the sulfur—carbon disulfide system have been published (16). Vapor—Hquid equiHbrium and freezing point data ate available for several binary mixtures containing carbon disulfide (9). 

Solubility-. Very slightly soluble in water (0.05% by volume) miscible with benzene, chloroform, diethyl ether, carbon disulfide and ethanol (Budavari, 1996) Vapour pressure 12 kPa at 20°C relative vapour density (air = 1), 5.3 at the boiling-point (American Conference of Governmental Industrial Hygienists, 1991)... 

The use of aromatic solvents was unsuitable for this spectroscopy even at the highest temperature, 110° C, because of the lack of fine detail in the spectra. Carbon disulfide gave suitable separation of the various methyl proton resonances. Nonetheless, it was unacceptable because of its low boiling point. In addition, a comparison of the spectra obtained in carbon disulfide and carbon tetrachloride indicates that some secondary resonances in the methyl proton region are not resolved in carbon disulfide. With carbon tetrachloride at higher temperature the resonances were less distinct. Separation of the methyl proton resonances was poor with hexachlorobutadiene at room temperature but increased as the temperature increased. The secondary resonances noted using carbon tetrachloride were also visible. Experience with a number of samples indicated that... 

A precipitate is formed immediately upon addition of the carbon disulfide the mixture becomes warm, and the temperature soon approaches the boiling point. The temperature is maintained just below the boiling point cooling with ice water may be necessary to keep it there. As the carbon disulfide is added, the mixture soon becomes pasty, then more fluid, and finally pasty again. 

O Brien and Alford have measured the heat of vaporization of carbon disulfide from (VC to the critical point.314 Buublik and co-workers have also studied (he heat of vaporization of carbon disulfide.211- The value at (he boiling point Is reponed for the other three compounds.2 1 Kharbtinda s nomograph wus used to estimate the heat of vaporization at other temperatures.11 Comparison with five experimental value showed an average error of 2.9%. 

Use the data from Appendix B to determine the normal boiling point of carbon disulfide (CS2). 

Arsenic triiodide commonly crystallizes in orange-red leaflets which show some tendency to sublime below 100°C. and melt to a red liquid at 149°C. The boiling point is about 400°C. Arsenic triiodide is readily soluble in carbon disulfide, chloroform, benzene, toluene, and xylene and less so in alcohol, ether, and water. It does not... 

Antimony triiodide forms beautiful ruby-red crystals which are soluble in carbon disulfide, benzene, alcohol, and acetone. The tendency to sublime becomes noticeable at temperatures as low as 100°C., but the melting point and boiling point are 166°C. and about 400°C., respectively. 

Carbon disulfide. Carbon disulfide (CS2) is produced commercially by the direct union of sulfur vapor and hot carbon at considerably elevated temperatures in an enclosed electric furnace. The reaction must be carried out in the absence of air. Solid sulfur and carbon (usually in the form of coke) are fed continuously into the furnace, which is heated electrically to a temperature sufficient to vaporize the sulfur and to maintain the carbon at a temperature such that combination occurs when the sulfur vapor comes into contact with the solid carbon. Since carbon disulfide is a low-boiling-point liquid (46°C), it passes out of the furnace as a vapor, which is conducted into a condenser. Although the resulting pale-yellow liquid may be purified by distillation, the crude product is used directly for many purposes. 

Phosphorus trichloride is a colourless transparent motile liquid (the boiling point is 76 °C) it fumes in air. It mixes with diethyl ether, petrol, chloroform, carbon disulfide and dichloroethane in all ratios It can be easily destroyed with water, acids and alcohols. Phosphorus trichloride vapours hydrolyse even in humid air. 

Phosphorus(V) sulfochloride is a colorless, fuming liquid with boiling point 125° and specific gravity 1.635. The alpha form solidifies at —40.8°, while the beta form solidifies at —36.2°.7 The compound hydrolyzes slowly in water and rapidly in alkaline solution. In water, the hydrolysis products are orthophosphoric acid, hydrochloric acid, and hydrogen sulfide. Phosphorus (Y) sulfochloride is soluble in benzene, carbon tetrachloride, carbon disulfide, and chloroform. It reacts with ethanol, yielding O-ethyl dichlorothiophosphate8 (synthesis 25). 

Covalent compounds have a wider variety of properties than ionic compounds. Some dissolve in water, and some do not. Some conduct electricity when molten or dissolved in water, and some do not. If you consider only covalent compounds that contain bonds with an electronegativity difference that is less than 0.5, you will notice greater consistency. For example, consider the compounds carbon disulfide, CS2, dichlorine monoxide, C120, and carbon tetrachloride, CC14. What are some of the properties of these compounds They all have low boiling points. None of them conducts electricity in the solid, liquid, or gaseous state. 

Carbon tetrachloride is colorless, heavy, non-flammable liquid with a characteristic odor. It has a boiling point of 78 Celsius, and a melting point of -23 Celsius. Carbon tetrachloride is insoluble in water, but miscible with alcohol, benzene, chloroform, ether, and carbon disulfide. Carbon tetrachloride is a potential poison, and inhalation, ingestion, and skin absorption should be avoided at all cost. Carbon tetrachloride may be a carcinogen. It is prepared on an industrial scale by the chlorination of methane, but can be conveniently prepared by reacting chlorine with carbon disulfide in the presence of iron fillings the carbon tetrachloride is recovered by distillation. 

Sulfur chloride forms a non-flammable, light amber to yellowish red, fuming oily liquid, which has a penetrating odor. It has a melting point of-77 Celsius, and a boiling point of 138 Celsius. It is soluble in alcohol, ether, carbon disulfide, toluene, carbon tetrachloride, and many oils. It reacts with water yielding sulfur dioxide, hydrogen chloride, and other products. Over exposure... 

Asphaltenes are dark brown to black friable solids that have no definite melting point, and when heated, usually intumesce, then decompose leaving a carbonaceous residue. They are obtained from petroleums and bitumens by addition of a nonpolar solvent (such as a hydrocarbon) with a surface tension lower than 25 dynes cm-1 at 25°C (such as liquefied petroleum gases, the low-boiling petroleum naphthas, petroleum ether, pentane, isopentane, and hexane) but are soluble in liquids having a surface tension above 25 dynes cm-1 (such as pyridine, carbon disulfide, carbon tetrachloride, and benzene) (6, 7). 

The aluminum derivative of ethyl acetoacetate is a white crystalHne material, reported to melt at 76°, or 78 to 79°. It supercools readily from the melt to a straw-colored, very viscous liquid. Molecular weight determinations in carbon disulfide indicate that the compound is not associated in that solvent. The aluminmn derivative of ethyl acetoacetate is very soluble in benzene, ether, and carbon disulfide. It is less soluble in petroleum ether or cyclohexane and is insoluble in water. The compound boils at 190 to 200° at 11 mm. The reported dipole moment, in benzene, is 3.96 Debye. Surface tension and density values for the liquid above the melting point have been reported by Robinson and Peak. ... 

For most substances a rough value of the heat of vaporization can be predicted from Trouton s rule, which states that the quotient of the molal heat of vaporization by the absolute boiling point has a constant value, about 21. For example, this rule predicts that the molal heat of vaporization of carbon disulfide, b.p. 319.3 A, be 21 X 319.8 6700 cal the experimental value is 6391 cal. The heats ol vaporization of water and alcohol are larger than expected from Trouton s rule, apparently because of the strong intermolecular forces in the liquids, due to the action of hydrogen bonds. 

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