12031-80-0 Usage
Chemical Properties
Different sources of media describe the Chemical Properties of 12031-80-0 differently. You can refer to the following data:
1. Lithium peroxide is a white crystalline solid or pale yellow powder which is thermodynamically stable at room temperature. The substance decomposes on heating to 195°C (the exact decomposition temperature is subject to dispute) with the formation of lithium oxide and oxygen. The decomposition forms the basis for one preparation of lithium oxide. High-purity lithium peroxide may be stored for long periods of time with no significant decomposition.
The reaction of carbon dioxide and lithium peroxide is noted above. When lithium peroxide is exposed to the air, lithium carbonate is the final product. Dissolving pure lithium peroxide in water produces an alkaline solution containing lithium ions and hydroperoxide ions. The decomposition of the solution is typical in that oxygen is released on heating or in the presence of a catalyst. The water solubility of lithium peroxide decreases with increasing temperature.
2. Lithium peroxide, Li2O2, Mr 45.9, 2.36 g/cm3, has an active oxygen content of 34.8%, which is the highest of all metal peroxides. Lithium peroxide is pale yellow solid, stable at ambient temperature, and not hygroscopic. On heating to about 300 °C, it loses oxygen and forms lithium monoxide.
Uses
Different sources of media describe the Uses of 12031-80-0 differently. You can refer to the following data:
1. Lithium peroxide is used in air purifiers. It is also used to produce high-purity oxygen. It acts as a catalyst for polymerization of styrene to polystyrene. Further, it serves as a curing agent for special polymers and a source of oxygen in sealed spaces such as submarines and in breathing apparatus.
2. At this time no important industrial uses of lithium peroxide are known. One interesting potential application is in the field of atmosphere regeneration for undersea and space applications, since the compound reacts with carbon dioxide to release oxygen: Li2O2+C02 -> Li2CO3 + 0.5O2.
Preparation
Lithium peroxide is prepared industrially by the reaction of lithium hydroxide monohydrate with hydrogen peroxide which yields lithium hydroperoxide monohydrate.
LiOH·H20 + H202 → LiOOH·H20+H20
The hydroperoxide may be dehydrated by heating in a vacuum to yield the peroxide.
2LiOOH·H20 → Li202+H202 + 2H20
General Description
A white powder or sandy yellow granular solid. Irritates skin, eyes and mucous membranes. Used to produce a supply of high-purity oxygen.
Air & Water Reactions
Contact with water or moist air generates a large amount of heat and corrosive, alkaline lithium hydroxide [AAR 1991].
Reactivity Profile
Lithium peroxide is strongly basic and an extremely powerful oxidizing agent. Accelerates the combustion of other materials, especially organic materials, involved in a fire. Can ignite wood, paper, oil, clothing, etc. on contact. May react explosively with hydrocarbons (fuels). Exposure to heat in a closed container may result in a vigorous reaction that violently ruptures the container.
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.
Flammability and Explosibility
Notclassified
Safety Profile
A powerful oxidizer
and irritant to skin, eyes, and mucous
membranes. A very dangerous fire hazard
because it is an extremely powerful oxidizing
agent. Will react with water or steam to
produce heat; on contact with reducing
materials, can react vigorously. See also
LITHIUM COMPOUNDS, PEROXIDES,
and PEROXIDES, INORGANIC.
Check Digit Verification of cas no
The CAS Registry Mumber 12031-80-0 includes 8 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 5 digits, 1,2,0,3 and 1 respectively; the second part has 2 digits, 8 and 0 respectively.
Calculate Digit Verification of CAS Registry Number 12031-80:
(7*1)+(6*2)+(5*0)+(4*3)+(3*1)+(2*8)+(1*0)=50
50 % 10 = 0
So 12031-80-0 is a valid CAS Registry Number.
InChI:InChI=1/2Li.2O/rLi2O2/c1-3-2-4-1
12031-80-0Relevant articles and documents
Thermal decomposition study on Li2O2 for Li2NiO2 synthesis as a sacrificing positive additive of lithium-ion batteries
Kim, Jaekwang,Kang, Hyunchul,Hwang, Keebum,Yoon, Songhun
, (2019)
Herein, thermal decomposition experiments of lithium peroxide (Li2O2) were performed to prepare a precursor (Li2O) for sacrificing cathode material, Li2NiO2. The Li2O2 was prepared by a hydrometallurgical reaction between LiOH·H2O and H2O2. The overall reaction during annealing was found to involve the following three steps: (1) dehydration of LiOH·H2O, (2) decomposition of Li2O2, and (3) pyrolysis of the remaining anhydrous LiOH. This stepwise reaction was elucidated by thermal gravimetric and quantitative X-ray diffraction analyses. Furthermore, over-lithiated lithium nickel oxide (Li2NiO2) using our lithium precursor was synthesized, which exhibited a larger yield of 90.9% and higher irreversible capacity of 261 to 265 mAh g?1 than the sample prepared by commercially purchased Li2O (45.6% and 177 to 185 mAh g?1, respectively) due to optimal powder preparation conditions.
Amorphous Li2O2: Chemical Synthesis and Electrochemical Properties
Zhang, Yelong,Cui, Qinghua,Zhang, Xinmin,McKee, William C.,Xu, Ye,Ling, Shigang,Li, Hong,Zhong, Guiming,Yang, Yong,Peng, Zhangquan
, p. 10717 - 10721 (2016)
When aprotic Li–O2batteries discharge, the product phase formed in the cathode often contains two different morphologies, that is, crystalline and amorphous Li2O2. The morphology of Li2O2impacts strongly on the electrochemical performance of Li–O2cells in terms of energy efficiency and rate capability. Crystalline Li2O2is readily available and its properties have been studied in depth for Li–O2batteries. However, little is known about the amorphous Li2O2because of its rarity in high purity. Herein, amorphous Li2O2has been synthesized by a rapid reaction of tetramethylammonium superoxide and LiClO4in solution, and its amorphous nature has been confirmed by a range of techniques. Compared with its crystalline siblings, amorphous Li2O2demonstrates enhanced charge-transport properties and increased electro-oxidation kinetics, manifesting itself a desirable discharge phase for high-performance Li–O2batteries.
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