Production of CS₂

Abstract

Production of Carbon DisulfideA process based on the system carbon monoxide plus sulfur at 500°C. ' X he traditional method of manufacturing carbon disulfide involves reaction between charcoal and sulfur at about 850°C .; charcoal is used because the reaction of sulfur with coke is prohibitively slow at all reasonable temperatures. In England both raw materials have to be imported. Efforts to produce carbon disulfide by other means may be conveniently divided into two groups: Chemical reactions other than the straightforward C + S2 = CS2, involving sulfur dioxide or hydrogen sulfide instead of -elemental sulfur and carbon monoxide or methane instead of elemental carbon. Replacing natural beech chars by artificially prepared carbonized briquets prepared from cheap low grade indigenous coals, and using the chemical reaction C + S2 = CS2.' By far the most widely used method is the reaction between charcoal and

Ionic liquids for metal extraction from chalcopyrite: solid, liquid and gas phase studies

“…The presence of carbon and oxygen in the chalcopyrite, and formation of CS 2 and CO 2 in the gas phase during leaching, is reminiscent of a Stock-like reaction mechanism (4). 44,45 …”

Carbon-Negative production of Hydrogen through Sulfur Intermediates

“…The rate of reaction to form CS 2 in step 1 is negligible below 450 °C and is highly dependent on the form of carbon species reacting. [16][17][18]. While cellulose, more so than methane, accurately reflects MSW feedstock, at the temperature required, cellulose decomposes into multiple simpler molecules such as CH 4 , H 2 O, and CO. [19] Among alkanes, methane is the most thermodynamically difficult to dehydrogenate and requires more severe conditions to react with sulfur.…”

“…Alternatively, reaction at higher temperatures with gaseous S will convert the char into CS 2 which may be utilized via reaction 2b to generate more elemental S. Charcoal and other reduced forms of carbon (e.g., methane, methanol, ethane, and CO) has been previously used to generate CS 2 on both laboratory and industrial scale. [16,18,29,31,[33][34][35] The extra S produced through reaction 2b may then be used in reaction 3a to generate more SO 2 feedstock, thereby improving the final yield of H 2 per unit of biomass (reaction 1 verses reaction 2). However, this method will also produce significant quantities of CO 2 from carbon that would otherwise remain sequestered in sulfur-enriched char.…”

A novel approach to sulfate geoengineering with surface emissions of carbonyl sulfide

“…Approximately 1 million tons of CS 2 is produced per year (Madon and Strickland-Constable, 1958), with China consuming approximately half of the global production of CS 2 for rayon manufacturing. CS 2 is highly unstable and is flammable in air.…”