Carbon disulphide
 |
|
 |
|
| Names | |
|---|---|
|
IUPAC name
Methanedithione
|
|
| Other names
Carbon bisulfide
|
|
| Identifiers | |
|
3D model (Jmol)
|
|
| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.000.767 |
| EC Number | 200-843-6 |
| KEGG | |
|
PubChem CID
|
|
| RTECS number | FF6650000 |
| UNII | |
| UN number | 1131 |
|
|
|
|
| Properties | |
| CS2 | |
| Molar mass | 76.13 g·mol−1 |
| Appearance | Colorless liquid Impure: light-yellow |
| Odor |
Chloroform (pure) Foul (commercial) |
| Density | 1.539 g/cm3 (-186°C) 1.2927 g/cm3 (0 °C) 1.266 g/cm3 (25 °C) |
| Melting point | −111.61 °C (−168.90 °F; 161.54 K) |
| Boiling point | 46.24 °C (115.23 °F; 319.39 K) |
| 0.258 g/100 mL (0 °C) 0.239 g/100 mL (10 °C) 0.217 g/100 mL (20 °C) 0.014 g/100 mL (50 °C) |
|
| Solubility | Soluble in alcohol, ether, benzene, oil, CHCl3, CCl4 |
| Solubility in formic acid | 4.66 g/100 g |
| Solubility in dimethyl sulfoxide | 45 g/100 g (20.3 °C) |
| Vapor pressure | 48.1 kPa (25 °C) 82.4 kPa (40 °C) |
| -42.2·10−6 cm3/mol | |
|
Refractive index (nD)
|
1.627 |
| Viscosity | 0.436 cP (0 °C) 0.363 cP (20 °C) |
| Structure | |
| Linear | |
| 0 D (20 °C) | |
| Thermochemistry | |
| 75.73 J/mol·K | |
|
Std molar
entropy (S |
151 J/mol·K |
|
Std enthalpy of
formation (ΔfH |
88.7 kJ/mol |
|
Gibbs free energy (ΔfG˚)
|
64.4 kJ/mol |
|
Std enthalpy of
combustion (ΔcH |
1687.2 kJ/mol |
| Hazards | |
| Safety data sheet | See: data page |
| GHS pictograms |
  
|
| GHS signal word | Danger |
| H225, H315, H319, H361, H372 | |
|
P210, P281, P305+351+338, P314 ICSC 0022 |
|
| Inhalation hazard | Irritant |
| Eye hazard | Irritant |
| Skin hazard | Irritant |
| NFPA 704 | |
| Flash point | −43 °C (−45 °F; 230 K) |
| 102 °C (216 °F; 375 K) | |
| Explosive limits | 1.3%-50% |
| Lethal dose or concentration (LD, LC): | |
|
LD50 (median dose)
|
3188 mg/kg (rat, oral) |
|
LC50 (median concentration)
|
>1670 ppm (rat, 1 hr) 15500 ppm (rat, 1 hr) 3000 ppm (rat, 4 hr) 3500 ppm (rat, 4 hr) 7911 ppm (rat, 2 hr) 3165 ppm (mouse, 2 hr) |
|
LCLo (lowest published)
|
4000 ppm (human, 30 min) |
| US health exposure limits (NIOSH): | |
|
PEL (Permissible)
|
TWA 20 ppm C 30 ppm 100 ppm (30-minute maximum peak) |
|
REL (Recommended)
|
TWA 1 ppm (3 mg/m3) ST 10 ppm (30 mg/m3) [skin] |
|
IDLH (Immediate danger)
|
500 ppm |
| Related compounds | |
|
Related compounds
|
Carbon dioxide Carbonyl sulfide Carbon diselenide |
| Supplementary data page | |
|
Refractive index (n), Dielectric constant (εr), etc. |
|
|
Thermodynamic
data |
Phase behaviour solid–liquid–gas |
| UV, IR, NMR, MS | |
|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|
|
 (what is   ?) |
|
| Infobox references | |
Carbon disulfide is a colorless volatile liquid with the formula CS2. The compound is used frequently as a building block in organic chemistry as well as an industrial and chemical non-polar solvent. It has an "ether-like" odor, but commercial samples are typically contaminated with foul-smelling impurities.
Small amounts of carbon disulfide are released by volcanic eruptions and marshes. CS2 once was manufactured by combining carbon (or coke) and sulfur at high temperatures.
A lower-temperature reaction, requiring only 600 °C, utilizes natural gas as the carbon source in the presence of silica gel or alumina catalysts:
The reaction is analogous to the combustion of methane. It is isoelectronic with carbon dioxide. CS2 is highly flammable:
Global production/consumption of carbon disulfide is approximately one million tonnes, with China consuming 49%, followed by India at 13%, mostly for the production of rayon fiber. United States production in 2007 was 56,000 tonnes.
Carbon disulfide is a solvent for phosphorus, sulfur, selenium, bromine, iodine, fats, resins, rubber, and asphalt. It has been used in the purification of single-walled carbon nanotubes.
Compared to CO2, CS2 is more reactive toward nucleophiles and more easily reduced. These differences in reactivity can be attributed to the weaker π donor-ability of the sulfido centers, which renders the carbon more electrophilic. Amines afford dithiocarbamates:
...
Wikipedia