Carbon disulfide, ignition

The most important hazard ia the manufacturiag of xanthates is the use of carbon disulfide (qv) because of its low flash poiat, ignition temperature, and its toxicity. A report on the manufacture of sodium ethyl xanthate at Keimecott Nevada Mines Division discusses the various safety problems and the design of a faciUty (81). A plant layout and a description of the reagent preparations are also given. 

Trinidad asphalt has a relatively uniform composition of 29% water and gas, 39% bitumen soluble in carbon disulfide, 27% mineral matter on ignition, and 5% bitumen that remains adsorbed on the mineral matter. Refining is essentially a process of dehydration by heating the cmde asphalt to ca 165°C. The refined product averages 36% mineral ash with a penetration at 25°C of about 2 (0.2 mm), a softening point (ring and ball method) of 99°C, a flash point (Cleveland open cup) of 254°C, a sulfur content of 3.3%, and a saponification value of 45 mg KOH/g. The mineral matter typically contains... 

Hot surfaces and electric sparks are potential ignition sources for carbon disulfide. The ignition temperature depends on specific conditions, and values from 90 to 120°C in air have been reported (2,22). Data on carbon disulfide oxidation and combustion have been summarized (18). Oxidation products ate generally sulfur dioxide [7446-09-5] and carbon dioxide [124-58-9J ... 

FPN No. 3) Certain chemical atmospheres may have characteristics that require safeguards beyond those required for any of the above groups. Carbon disulfide is one of these chemicals because of its low ignition temperature [100°C (212°F)] and the small joint clearance permitted to arrest its flame. 

Niepce s Incendiary Composition. Contained benz, petroleum or carbon disulfide with a small piece of metallic potassium or Ca phosphate as igniter. Potassium was later replaced with metallic sodium Ref Daniel (1902), 153... 

Njkles, Proposed an incendiary compn, called "feu lorrain", consisting of hydrochloric and sulfuric acids, and a soln of phosphorus in carbon disulfide. The mixt ignites, evolving heavy reddish fumes, when brought in contact with an ammonia-cal soln... 

Matignon, C., Compt. rend., 1900, 130, 1391 Aluminium powder ignites in carbon disulfide vapour. 

Dining the preparation of chloronitromethane by adding portions of dry sodium acz-nitromethanide to chlorine (40 mol of each) dissolved in carbon disulfide, a violent explosion occurred when the addition was half-complete. Similar reactions using bromine had been executed uneventfully many times previously [1], No certain explanation has emerged, but the sodium salt is known to be explosively unstable, and mixtures of carbon disulfide vapour and air are of course extremely flammable and explosive. Contact of the dry salt with traces of chlorine above its carbon disulfide solution may have led to an exotherm and ignition of the vapour-air mixture in the flask [2],... 

Disposal of 2 1 of the solvent into a rusted iron sewer caused an explosion. Initiation of the solvent-air mixture by rust was suspected [1], A hot gauze falling from a tripod into a laboratory sink containing some carbon disulfide initiated two explosions [2], It is a very hazardous solvent because of its extreme volatility and flammability. The vapour or liquid has been known to ignite on contact with steam pipes, particularly if rusted [3], When a winchester of the solvent fell off a high shelf and broke behind a rusted steel cupboard, ignition occurred [4],... 

Antimony trisulfide, carbon disulfide vapour, chromium(II) sulfide and hydrogen sulfide all ignite in contact with fluorine at ambient temperature, the solids becoming incandescent [1]. Iron(II) sulfide reacts violently on mild warming, and barium sulfide, potassium sulfide or zinc sulfide all incandesce in the gas, as does molybdenum(III) sulfide at 200°C [2],... 

Passage of moist hydrogen sulfide over unheated sodium causes melting and then usually ignition of the metal. Mixtures of sodium (or its alloy with potassium) and carbon disulfide are shock-sensitive explosives. 

Both yellow and red phosphorus ignite on contact with fluorine and chlorine red ignites in liquid bromine or in a heptane solution of chlorine at 0°C. Yellow phosphorus explodes in liquid bromine or chlorine, and ignites in contact with bromine vapour or solid iodine [1]. Interaction of bromine and white phosphorus in carbon disulfide gives a slimy by-product which explodes violently on heating [2], Interaction of phosphorus and iodine in carbon disulfide is rather rapid [3], A less hazardous preparation of diphosphorus tetraiodide from phosphorus trichloride and potassium iodide in ether is recommended [4],... 

Fenian Fire (liquid Fire)—consisted of a solution of yellow phosphorous in carbon disulfide. On evaporation of the CS2, the phosphorous self-ignited in the air and ignited nearby flammable objects... 

As soon as part of carbon disulfide evaporated, P on coming in contact with air ignited and its flame ignited die flammable liquid of grenade... 

Sulfur is determined as the further loss of weight on extraction with carbon disulfide in a Wilcv extractor or other suitable apparatus. After the extraction, the crucible ought to be allowed to dry in the air away from flames until all the inflammable carbon disulfide has escaped. It is then dried in the oven to constancy of weight, and the residue is taken as charcoal. Ash is determined by igniting the residue in the crucible until all carbon has burned away. A high result for ash may indicate that the water extraction during the determination of potassium nitrate was not complete. The analytical results may be calculated on a moisture-free basis for a closer approximation to the formula by which the manufacturer prepared the powder. 

As expected for a molecular solid that contains small, nonpolar molecules, white phosphorus has a low melting point (44°C) and is soluble in nonpolar solvents such as carbon disulfide, CS2. It is highly reactive, bursting into flames when exposed to air, and is thus stored underwater. When white phosphorus is heated in the absence of air at about 300°C, it is converted to the more stable red form. Consistent with its polymeric structure, red phosphorus is higher melting (mp 600°C), less soluble, and less reactive than white phosphorus, and it does not ignite on contact with air (Figure 19.9). 

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