Potassium sulfide
| |
| |
| Names | |
|---|---|
| IUPAC name
Potassium sulfide
| |
| Other names
Dipotassium monosulfide,
Dipotassium sulfide, Potassium monosulfide, Potassium sulfide | |
| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
| ECHA InfoCard | 100.013.816 |
| EC Number |
|
PubChem CID
|
|
| RTECS number |
|
| UNII | |
| UN number | 1847 1382 |
CompTox Dashboard (EPA)
|
|
| |
| |
| Properties | |
| K2S | |
| Molar mass | 110.262 g/mol |
| Appearance | pure: colourless impure: yellow-brown |
| Odor | H2S |
| Density | 1.74 g/cm3 |
| Melting point | 840 °C (1,540 °F; 1,110 K) |
| Boiling point | 912 °C (1,674 °F; 1,185 K) (decomposes) |
| converts to KSH, KOH | |
| Solubility in other solvents | soluble in ethanol, glycerol insoluble in ether |
| −60.0·10−6 cm3/mol | |
| Structure | |
| antiFluorite | |
| Thermochemistry | |
Std molar
entropy (S⦵298) |
105.00 J·mol−1·K−1[1] |
Std enthalpy of
formation (ΔfH⦵298) |
-406.2 kJ·mol−1[2] |
Gibbs free energy (ΔfG⦵)
|
-392.4 kJ·mol[2] |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
|
Causes skin burns. Dangerous for the environment |
| GHS labelling: | |
 
| |
| Danger | |
| H314, H400 | |
| P260, P264, P273, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P391, P405, P501 | |
| Related compounds | |
Other anions
|
Potassium oxide Potassium selenide Potassium telluride Potassium polonide |
Other cations
|
Lithium sulfide Sodium sulfide Rubidium sulfide Caesium sulfide |
Related compounds
|
Potassium hydrosulfide Potassium sulfite Potassium sulfate Iron(II) sulfide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Potassium sulfide is an inorganic compound with the formula K2S. The colourless solid is rarely encountered, because it reacts readily with water, a reaction that affords potassium hydrosulfide (KSH) and potassium hydroxide (KOH). Most commonly, the term potassium sulfide refers loosely to this mixture, not the anhydrous solid.
Structure
It adopts "antifluorite structure," which means that the small K+ ions occupy the tetrahedral (F−) sites in fluorite, and the larger S2− centers occupy the eight-coordinate sites. Li2S, Na2S, and Rb2S crystallize similarly.[3]
Synthesis and reactions
It can be produced by heating K2SO4 with carbon (coke):
- K2SO4 + 4 C → K2S + 4 CO
In the laboratory, pure K2S may be prepared by the reaction of potassium and sulfur in anhydrous ammonia. [4]
Sulfide is highly basic, consequently K2S completely and irreversibly hydrolyzes in water according to the following equation:
- K2S + H2O → KOH + KSH
For many purposes, this reaction is inconsequential since the mixture of SH− and OH− behaves as a source of S2−. Other alkali metal sulfides behave similarly.[3]
Use in fireworks
Potassium sulfides are formed when black powder is burned and are important intermediates in many pyrotechnic effects, such as senko hanabi and some glitter formulations.[5]
See also
References
- ^ CRC Handbook of Chemistry and Physics (95th ed.). CRC Press. 2014. pp. 5–15. ISBN 1482208679.
- ^ a b Johnson, G.K.; Steele, W.V. (1981). "The standard enthalpy of formation of potassium sulfide (K2S) by fluorine bomb calorimetry". The Journal of Chemical Thermodynamics. 13 (10): 985–990. doi:10.1016/0021-9614(81)90075-6.
- ^ a b Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ^ Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 360.
- ^ Shimizu, Takeo. "Fireworks: the Art, Science, and Technique." Pyrotechnica Publications: Austin, 1981. ISBN 0-929388-05-4.