LITHIUM OXIDE Li2OWhite, hygroscopic, refractory, when heated, does not decompose. Behaves as a typical oxide, reacts vigorously with water (formed alkaline solution), acids, metals, acid oxides, absorbs CO2 from air. Obtaining Lithium oxide Li2O: 4Li + O2 = 2Li2O (t > 200°C, impurity Li2O2) 2LiOH = Li2O + H2O (800-1000°C, in the atm. of H2). Li2CO3 = Li2O + CO2 (730-1270°C). Li2CO3 + C(coke) = Li2O + 2CO (800°C). 4LiNO3 = 2Li2O + 4NO2 + O2 (475-650°C). Reactions with Lithium oxide Li2O: Li2O + H2O = 2LiOH. Li2O + 2HCl (deluted) = 2LiCl + H2O. Li2O + H2S = Li2S + H2O (900-1000°C). 2Li2O + Si = 4Li + SiO2 (1000°C). Li2O + Mg = 2Li + MgO (t >800°C). 3Li2O + 2Al = 6Li + Al2O3 (t >1000°C). Li2O + CO2 = Li2CO3 (500-600°C). 2Li2O + SiO2 = Li4Si04 (1000°C), Li2O + SiO2 = Li2SiO3 (1200-1300°C). |
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Approximately 20% of the oxygen in the atmosphere was produced by the Amazon rainforest.