Lithium peroxide

Lithium Peroxide. Lithium peroxide [12031 -80-0] Li202, is obtained by reaction of hydrogen peroxide and lithium hydroxide in ethanol (72) or water (73). Lithium peroxide, which is very stable as long as it is not exposed to heat or air, reacts rapidly with atmospheric carbon dioxide releasing oxygen. The peroxide decomposes to the oxide at temperatures above 300°C at atmospheric pressure, and below 300°C under vacuum. 

Peroxides. In the presence of lithium peroxide, both water and carbon dioxide react, resulting in evolution of oxygen. The following steps have been postulated (17) ... 

Because of the delay in decomposition of the peroxide, oxygen evolution follows carbon dioxide sorption. A catalyst is required to obtain total decomposition of the peroxides 2 wt % nickel sulfate often is used. The temperature of the bed is the controlling variable 204°C is required to produce the best decomposition rates (18). The reaction mechanism for sodium peroxide is the same as for lithium peroxide, ie, both carbon dioxide and moisture are required to generate oxygen. Sodium peroxide has been used extensively in breathing apparatus. 

K. J. Dressier and R. N. Prince, "Lithium Peroxide for Portable Life Support System Atmospheric Regeneration," Conference on Portable Eife Support Systems, NASA-Ames Research Center, Moffett Field, Calif., Apr. 1969. 

Alkali metal peroxides are stable under ambient conditions in the absence of water. They dissolve vigorously in water, forming hydrogen peroxide and the metal hydroxide. They are strong oxidizing agents and can react violendy with organic substances. Only lithium peroxide and sodium peroxide have been commercialized. 

Lithium peroxide is a strong oxidizer and can promote combustion when in contact with combustible materials. It is a powerful irritant to skin, eyes, and mucous membranes (2) protective clothing should be worn when handling lithium peroxide. The LD q has not been deterrnined, and there is no designated threshold limit value (TLV). However, 5 g of many lithium compounds can be fatal. 

Commercial lithium peroxide has been assigned UN No. 1472 and should be transported in accordance with international transport regulations pertaining to Class 5.1, oxidizing substances. It is manufactured by ChemetaH AG (Germany) and Lithium Corp. of America (United States). The U.K. price in 1994 was J48—198/kg ( 70—285/kg), depending on quantity. 

Lithium peroxide/hypochlorite Magnesium nitrate/perchlorate Nickel nitrate... 

Lithium oxide(s), 15 134, 141 Lithium perchlorate, 3 417 15 141-142 dessicant, 3 360 in lithium cells, 3 459 Lithium peroxide, 15 142 18 393 Lithium phosphate, 15 142 Lithium-polymer cells, 3 551 in development, 3 43 It Lithium primary cells, 3 459-466 Lithium production, 9 640 Lithium products, sales of, 15 121 Lithium salts, 15 135-136, 142 Lithium secondary cells, 3 549-551 ambient temperature, 3 541-549 economic aspects, 3 551-552 high temperature, 3 549-551 Lithium silicate glass-ceramics, 12 631-632... 

Lead dioxide Lead perchlorate Lithium chlorate Lithium hypochlorite Lithium perchlorate Lithium peroxide Magnesium bromate Magnesium chlorate Magnesium perchlorate Magnesium peroxide Manganese dioxide Mercurous chlorate Mono-(trichloro)-tetra-(mono-potassium dichloro)-penta-s-triazinetrione... 

Run a similar experiment with metallic lithium. What forms in this case How can lithium peroxide be prepared What products form when rubidium and cesium react with the oxygen of the air ... 

Preparation of Lithium Peroxide, a. Preparation o/ Lithium Hydroxide Monohydrate. Put 5 g of lithium sulphate into a 400-ml... 

Separate the formed precipitate of lithium peroxide monohydrate from the mother liquor by filtration and wash it twice on the filter with 5-ml portions of absolute ethanol. Dry the substance in the air. 

Add distilled water to a small amount of the lithium peroxide. See how the mixture reacts with solutions of potassium permanganate and potassium iodide acidified with sulphuric acid (add two nr three drops of a starch size to,the potassium iodide solution). What do you observe Write the equations of the reactions. 

Lithium Peroxide. Lithium peroxide, U2O2, is used in space technology because it absorbs carbon dioxide and liberates oxygen. This peroxide, also used for hardening certain plashes, is a white or pale yellow solid, stable at ambient temperature, and not hygroscopic... 

Lithium peroxide, Li202, has a hexagonal unit cell with two molecules per cell, C h, P6, a0 = 3.142, and co = 7.650A. Two projections are shown in Figure 8.15. The heights along c0 are ... 

Figure 8.15. Two views of the hexagonal cell of lithium peroxide, Li2C>2-(Source R.W.G. Wyckoff, Crystal Structures, Vol. 1, 2nd ed., Wiley, New York, 1964, p. 168.)...

For parts (b), (c), and (d), note that pure oxygen gas is not necessarily the most compact source of oxygen for a confined fuel system because of the weight of the cylinder necessary to confine the gas. Other compact sources are hydrogen peroxide and lithium peroxide. The oxygen-yielding reactions are... 

Lithium hydroxide 1-hydrate, formation of, from lithium hydroperoxide 1-hydrate, 6 3 Lithium nitride, 4 1 Lithium oxide, 6 1, 5 Lithium peroxide, 5 1... 

The conjugate addition of lithium peroxides on enones is a non-classical route to epoxidation. The original lithium enolate rearranges immediately in situU3. Note that a catalytic asymmetric version of this reaction was also developed (Scheme 41)184. 

SCHEME 41. Enantioselective catalytic conjugate addition of a lithium peroxide on chalcone184... 

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