12030-88-5

Basic information

• Product Name: Potassium superoxide
• Synonyms: PotassiuM Superoxide, Uncatalyzed Granules;PotassiuM Superoxide, Uncatalyzed Granules, 3/8 to 1/4 in.;PotassiuM dioxide powder;Potassium dioxide chunks, 5-10 mm;potassiumsuperoxide(k(o2));potassiumsuperoxide,ko2,industrial;potassiumsuperoxide,ko2,industrial-(fluff);potassiumsuperoxide,ko2,industrial-(granules)
• CAS NO: 12030-88-5
• Molecular Formula: KO2 *
• Molecular Weight: 71.1
• EINECS: 234-746-5
• Product Categories: metal oxide
• Mol File: 12030-88-5.mol
• Article Data: 12

Chemical Properties

• Melting Point: 400 °C
• Boiling Point: °Cat760mmHg
• Flash Point: °C
• Appearance: Yellow-green/powder
• Density: 2,14 g/cm3
• Vapor Pressure: 322000mmHg at 25°C
• Storage Temp.: Store at +15°C to +25°C.
• Solubility: Soluble in ethanol and ether.
• Water Solubility: reacts
• Sensitive: Air & Moisture Sensitive
• Stability: Stable, but reacts violently with water. Incompatible with moisture, alcohols, strong reducing agents, strong acids, finely powd
• CAS DataBase Reference: Potassium superoxide(CAS DataBase Reference)
• NIST Chemistry Reference: Potassium superoxide(12030-88-5)
• EPA Substance Registry System: Potassium superoxide(12030-88-5)

Safety Data

• Hazard Codes: O,C
• Statements: 8-14-34-35
• Safety Statements: 17-27-36/37/39-8-45-26
• RIDADR: UN 2466 5.1/PG 1
• WGK Germany: 3
• RTECS: TT6053000
• TSCA: Yes
• HazardClass: 5.1
• PackingGroup: I
• Hazardous Substances Data: 12030-88-5(Hazardous Substances Data)

Usage

Chemical Properties

light yellow powder or chunks

Uses

Different sources of media describe the Uses of 12030-88-5 differently. You can refer to the following data:
1. Reagent and intermediate.One use of potassium superoxide,KO2, is for generating oxygen. It has the ability to absorb carbon dioxide, while giving out oxygen at the same time:4KO2(s)+ 2CO2(g)--->2K2CO3(s)+ 3O2(g)This property has been made use of in breathing equipment,e.g.for mountaineers, in submarines and in spacecraft.
2. Potassium oxide is used as a carbon dioxide scrubber, water dehumidifier and oxygen generator. It finds application in rebreathers for fighting with fire and mine rescue work. It is also used in spacecraft, submarines and spacesuit life support systems.

General Description

A yellowish to white solid. Melting point 948°F. Mixtures with combustible material readily ignite by friction, heat, or contact with moisture. Prolonged exposure to fire or heat may cause vigorous decomposition of the material and rupturing of the container.

Air & Water Reactions

Reacts explosively with water [Mellor 2, Supp. 3: 1631. 1963].

Reactivity Profile

Potassium superoxide is a powerful oxidizer. Forms on the surface of potassium metal, solid or molten, that is exposed to the air. Attempts to extinguish burning potassium with powdered graphite has resulted in violent explosions [Chem. Abstr. 63:424. 1965]. Highly oxidized potassium metal was dropped into a dish of ethyl alcohol, an immediate explosion shattered the dish. Potassium superoxide was considered the cause of the reaction [Health and Safety Inf. 251. 1967]. Potassium superoxide should not be added to pure organic materials (hydrocarbons), as ignition and violent explosion may occur. Oxidation of arsenic, antimony, copper, potassium, tin, or zinc proceeds with incandescence, [Mellor, 1941, Vol. 2, 493]. Interaction between the superoxide and diselenium dichloride is violent, [Mellor, 1947, Vol. 10, 897].

Hazard

Corrosive to tissue.

Health Hazard

TOXIC; inhalation, ingestion or contact (skin, eyes) with vapors, dusts or substance may cause severe injury, burns or death. Fire may produce irritating and/or toxic gases. Toxic fumes or dust may accumulate in confined areas (basement, tanks, hopper/tank cars, etc.). Runoff from fire control or dilution water may cause pollution.

Fire Hazard

May explode from friction, heat or contamination. These substances will accelerate burning when involved in a fire. May ignite combustibles (wood, paper, oil, clothing, etc.). Some will react explosively with hydrocarbons (fuels). Containers may explode when heated. Runoff may create fire or explosion hazard.

Safety Profile

Explosive reaction when heated with carbon, 2-aminophenol + tetrahydrofuran (at 65°C). Forms a friction- sensitive explosive mixture with hydrocarbons. Violent reaction with lselenium dichloride, ethanol, potassium- sodium alloy. May ignite on contact with organic compounds. Incandescent reaction with metals (e.g., arsenic, antimony, copper, potassium, tin, and zinc). When heated to decomposition it emits toxic fumes of K2O. See also PEROXIDES.

InChI:InChI=1/K.O2/c;1-2/q+1;

Upstream product

• 7440-09-7 potassium 
• 10028-15-6 ozone 
• 7732-18-5 water 
• 80937-33-3 oxygen 
• 1204-49-5 benzhydrol potassium salt 
• 32767-18-3 oxygen-18 
• 7722-84-1 dihydrogen peroxide 
• 865-47-4 potassium tert-butylate 

Downstream Products

• 78762-95-5 [K*dibenzo-18-crown-6][Al₂Me₆O₂]*(n)C₆H₅Me 
• 1207072-63-6 [(O₂)Fe(C₂₀H₈N₄(C₆H₂(CH₃)3)3)(C₃N₂H₃CH₂C₆H₄CONHC₆H₄)]^(1-) 
• 1207072-64-7 [(tmpIm)Fe(III)OOH] 
• 1352062-25-9 K[Fe(III)(tBuTPP)(O₂^(2-))] 
• 20427-59-2 copper hydroxide 
• 1255941-62-8 [K(18-crown-6)][Cu(C₅H₃N(CONC₆H₃(CH(CH₃)2)2)2)(superoxide)] 
• 7722-84-1 dihydrogen peroxide 
• 80937-33-3 oxygen 

Related news

Ultrasound promoted N-alkylation of pyrrole using Potassium superoxide (cas 12030-88-5) as base in crown ether07/28/2019

Ultrasound accelerates the N-alkylation of pyrrole by alkylating reagents using potassium superoxide as base in the presence of 18-crown-6. A much lower yield of N-alkylated pyrrole was realized in the absence of ultrasound. N-alkylating reagents employed for pyrrole are methyl iodide, ethyl bro...detailed

Relevant articles and documents

Thermo-analytical Investigations on the Superoxides AO2 (A = K, Rb, Cs), Revealing Facile Access to Sesquioxides A4O6

Rb4O6 and Cs4O6 represent open shell p electron systems, featuring charge, spin, orbital and structural degrees of freedom, which makes them unique candidates for studying the ordering processes related, otherwise exclusively encountered in transition metal based materials. Probing the physical responses has been restrained by the intricacy of synthesizing appropriate amounts of phase pure samples. Tracing the thermal decomposition of respective superoxides has revealed that at least the rubidium and cesium sesquioxides exist in thermodynamic equilibrium, appropriate p-T conditions given. These insights have paved the way to highly efficient and convenient access to Rb4O6 and Cs4O6.

A study of the kinetics of synthesis of potassium superoxide from an alkaline solution of hydrogen peroxide

Kinetic aspects and the mechanism of shaping of particles of potassium superoxide in its synthesis from drops of an alkaline solution of hydrogen peroxide in a flow of a drying agent were studied.

Electrochemistry in liquid ammonia. 5. Electroreduction of oxygen

The reduction of O2 in liquid NH3 at a Pt electrode has been investigated. Chemical and electrochemical measurements show that the first reduction of O2 is a one-electron process producing O2-·, which is a stable species in liquid NH3 and precipitates as KO2 in the presence of K+. The solubility of O2 in liquid NH3 at temperatures between -60 and -40°C was determined, and from these results, the diffusion coefficient of O2 in liquid NH3 was evaluated as 4.4 × 10-5 cm2/s at -55°C.

Kinetic Study of the Reaction K + O2 + M (M = N2, He) from 250 to 1103 K

The recombination reaction K + O2 + M was studied by the technique of pulsed photolysis of a K atom precursor followed by time-resolved laser induced fluorescene spectroscopy of K atoms at λ = 404 or 760 nm.Termolecular behavior was demonstrated and absolute third-order rate constants obtained over the temperature range 250-1103 K.A fit of this data to the form AT-n yields k(T,M = N2) = -30>(T/300)-(1.32+/-0.04) cm6 molecule-2 s-1 and k(T,M = He) = -30>(T/300)-(1.22+/-0.07) cm6 molecule-2 s-1.These results are compared to two previous studies of these reactions by different experimental methods, which were in marked disagreement below 600 K.A lower limit of D0(K-O2) > 203 kJ mol-1 is derived.The rate coefficients are then extrapolated from the experimental temperature range to ambient mesopheric temperatures (140 K T 240 K) and to flame temperatures (1500 K T 2200 K), by means of the Troe formalism.Finally, the rates of formation and bond energies of LiO2, NaO2, and KO2 are compared.

Choice of a stabilizer for the reaction of KOH with hydrogen peroxide to produce potassium superoxide

A stabilizer for the reaction of KOH and H2O2 yielding potassium superoxide was proposed. The stabilizer does not affect the main consumer properties of the regenerative product based on KO2.

Synthetic models for the cysteinate-ligated non-heme iron enzyme superoxide reductase: Observation and structural characterization by XAS of an FeIII-OOH intermediate

Superoxide reductases (SORs) belong to a new class of metalloenzymes that degrade superoxide by reducing it to hydrogen peroxide. These enzymes contain a catalytic iron site that cycles between the FeII and FeIII states during catalysis. A key step in the reduction of superoxide has been suggested to involve HO2 binding to FeII, followed by innersphere electron transfer to afford an FeIII-OO(H) intermediate. In this paper, the mechanism of the superoxide-induced oxidation of a synthetic ferrous SOR model ([FeII- (SMe2N4(tren))]+ (1)) to afford [FeIII(SMe2N4(tren)(solv))]2+ (2-solv) is reported. The XANES spectrum shows that 1 remains five-coordinate in methanolic solution. Upon reaction of 1 with KO2 in MeOH at -90 °C, an intermediate (3) is formed, which is characterized by a LMCT band centered at 452(2780) nm, and a lowspin state (S=1/2), based on its axial EPR spectrum (g⊥ = 2.14; g∥ = 1.97). Hydrogen peroxide is detected in this reaction, using both 1H NMR spectroscopy and a catalase assay. Intermediate 3 is photolabile, so, in lieu of a Raman spectrum, IR was used to obtain vibrational data for 3. At low temperatures, a vo-o Fermi doublet is observed in the IR at 788(2) and 781(2) cm-1, which collapses into a single peak at 784 cm-1 upon the addition of D2O. This vibrational peak diminishes in intensity over time and essentially disappears after 140 s. When 3 is generated using an 18O-labeled isotopic mixture of K18O2/K16O2 (23.28%), the vibration centered at 784 cm-1 shifts to 753 cm-1. This new vibrational peak is close to that predicted (740 cm-1) for a diatomic 18O-18O stretch. In addition, a vo-o vibrational peak assigned to free hydrogen peroxide is also observed (vo-o = 854 cm-1) throughout the course of the reaction between FeII-1 and superoxide and is strongest after 100 s. XAS studies indicate that 3 possesses one sulfur scatterer at 2.33(2) A and four nitrogen scatterers at 2.01(1) A. Addition of two Fe-O shells, each containing one oxygen, one at 1.86(3) A and one at 2.78(3) A, improved the EXAFS fits, suggesting that 3 is an end-on peroxo or hydroperoxo complex, [FeIII(SMe2N4(tren))(OO(H))]+. Upon warming above -50 °C, 3 is converted to 2-MeOH. In methanol and methanol:THF (THF = tetrahydrofuran) solvent mixtures, 2-MeOH is characterized by a LMCT band at λmax = 511(1765) nm, an intermediate spin-state (S = 3/2), and, on the basis of EXAFS, a relatively short Fe-O bond (assigned to a coordinated methanol or methoxide) at 1.94-(10) A. Kinetic measurements in 9:1 THF:MeOH at 25 °C indicate that 3 is formed near the diffusion limit upon addition of HO2 to 1 and converts to 2-MeOH at a rate of 65(1) s-1, which is consistent with kinetic studies involving superoxide oxidation of the SOR iron site.