Lithium fire

COLORANTSFORFOOD,DRUGS,COSTffiTICSANDTffiDICALDEVICES] (Void) -for lithium fires THIUM AND LITHIUM COMPOUNDS] (Vol 15)... 

Carbon dioxide reacts slowly with fragmented lithium at 20 C. With the powdered metal, its ignition is instantaneous. It also happens when it is hot. This is the reason why carbon dioxide extinguishers are forbidden for putting out lithium fires (and metals in general see later). 

Lithium burns violently in contact with sodium carbonate. This behaviour explains why use of extinguishing powders containing carbonates (and especially hydrogencarbonates) are forbidden for putting out lithium fires (and all fires of highly reducing metals). 

This reaction shows that it is impossible to put out lithium fires with sodium chloride although it is an extinguishing agent for metal fires. 

Although carbon dioxide reacts slowly with lithium at ambient temperature, the molten metal will bum vigorously in the gas, which cannot be used as an extinguisher on lithium fires. Carbon monoxide reacts in liquid ammonia to give the carbonyl which reacts explosively with water or air. Lithium rapidly attacks silica or glass at 250°C. 

Sodium carbonate and sodium chloride are unsuitable to use as extinguishers for lithium fires, since burning lithium will liberate the more reactive sodium in contact with them. 

As an element (metal), it must be stored in oil or in some type of air and moisture-free container, given that many of its compounds will also burn when exposed to air or water. Lithium fires are difficult to extinguish. If water is poured on the fire, hthium will just burn faster or explode. A supply of special chemicals or even dry sand is required to extinguish such fires. 

Fire control. Lithium fires can be controlled by smothering with anhydrous lithium chloride or with Ansul Plus 50 fire-extinguishing compound. 

Hazard Ignites in air near its melting point dangerous fire and explosion risk when exposed to water, acids, or oxidizing agents. Extinguish lithium fires only with chemicals designed for this purpose. Lithium in solution is toxic to the central nervous system. 

Uses. Lithium fluoride is used primarily in the ceramic industry to reduce firing temperatures and improve resistance to thermal shock, abrasion, and acid attack (see Ceramics). Another use of LiF is in flux compositions with other fluorides, chlorides, and borates for metal joining (17) (see Solders). 

Normally, lithium hydride ignites in air only at high temperatures. When heated it reacts vigorously with CO2 and nitrogen. With the former, lithium formate is obtained. Reaction at high temperature with nitrogen produces lithium nitride. Therefore, dry limestone or NaCl powders are used to extinguish LiH fires. Lithium hydride reacts exothermically with moist air and violently with water. 

Selenium and selenium compounds are also used in electroless nickel-plating baths, delayed-action blasting caps, lithium batteries, xeroradiography, cyanine- and noncyanine-type dyes, thin-film field effect transistors (FET), thin-film lasers, and fire-resistant functional fluids in aeronautics (see... 

Single-effec t indirect-fired lithium bromide cycle is shown in Fig. 11-99. The machine consists of five major components ... 

Health Hazards Information - Recommended Personal Protective Equipment Rubber or plastic gloves face shield respirator fire-retardant clothing Symptoms Following Exposure Contact with eyes causes caustic irritation or burn. In contact with skin lithium react with body moisture to cause chemical burns foil, ribbon, and wire react relatively slowly General Treatment for Exposure EYES or SKIN flush with water and treat with boric acid Toxicity by Inhalation (ThresholdUmit Value) Data not available Short-Term Inhalation Limits Data not available Toxicity by Ingestion Data not available Late Toxicity Data not available Vapor (Gas) Irritant Characteristics Data not available Liquid or Solid Irritant Characteristics Data not available Odor Threshold Data not available. 

The poor efficiencies of coal-fired power plants in 1896 (2.6 percent on average compared with over forty percent one hundred years later) prompted W. W. Jacques to invent the high temperature (500°C to 600°C [900°F to 1100°F]) fuel cell, and then build a lOO-cell battery to produce electricity from coal combustion. The battery operated intermittently for six months, but with diminishing performance, the carbon dioxide generated and present in the air reacted with and consumed its molten potassium hydroxide electrolyte. In 1910, E. Bauer substituted molten salts (e.g., carbonates, silicates, and borates) and used molten silver as the oxygen electrode. Numerous molten salt batteiy systems have since evolved to handle peak loads in electric power plants, and for electric vehicle propulsion. Of particular note is the sodium and nickel chloride couple in a molten chloroalumi-nate salt electrolyte for electric vehicle propulsion. One special feature is the use of a semi-permeable aluminum oxide ceramic separator to prevent lithium ions from diffusing to the sodium electrode, but still allow the opposing flow of sodium ions. 

Perfluorosuccinamide-Lithium Aluminum Hydride (Danger of Explosion). In an attempt to reduce perfluorosuccinamide to the corresponding diamine, it was added to an ether soln of lithium aluminum hydride in a nitrogen atm. Hydrolysis was then attempted, but as a second drop of w was added, a violent expln and ether fire resulted. It was shown that the diamide and the lithium aluminum hydride reacted to give an unstable complex which detonated at room temp Ref T.S. Reid G.H. Smith, C EN 29,3042 (1951) CA 46, 3279 (1952)... 

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