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The Distillation of Lithium Metal
Leo F. Epstein & W.H. Howland
Science
Vol.114(2965) 1951, pp.443-444.
DOI: 10.1126/science.114.2965.443
Abstract
If a piece of lithium is heated in air in a glass test tube, the metal first darkens becasue the the temperature-accelerated reaction with nitrogen, oxygen and other constituents of the air. At, or a little above, the melting point (1) 186C, a spectacular reaction with the glass occurs. The test tube grows red, then white hot. In a short time, the bottom falls out of it and the metal burns with a brilliant white flame, like that of magnesium. It has been reported (2) that the lithium in this reaction reduces the SiO2 and silicates of the glass to form lithium silicide. Attempts to purify lithium on a laboratory scale by distillation in glass have usually ended in failure, accompanied by a fireworks display similar to that described above. It is the purpose of this paper to show how a glass system can be used to carry out this process.
Effect of Pressure on the Refining of Lithium by Distillation
R. R. Rogers and G. E. Viens
J. Electrochem. Soc.
Vol.98(12) 1951, pp.483-487
DOI:10.1149/1.2778029
Abstract
The experiments described show that lithium containing 0.5 per cent sodium can be refined by distillation in the presence of argon in a straight retort, the refined material containing as low as 0.002 per cent sodium. At gauge pressures up to 1 micron the sodium content differs very little from this value. In increasing the pressure from 1 to 740 microns the sodium content is quadrupled. In the presence of argon, nitrogen, oxygen, and hydrogen at different pressures in a slightly V-shaped retort, a sodium content of less than 0.01 per cent was not obtained. There was little or no evidence of oxide, nitride, or hydride formation at pressures of oxygen, nitrogen, or hydrogen below 35 microns.
The Distillation of Lithium Metal
Leo F. Epstein & W.H. Howland
Science
Vol.114(2965) 1951, pp.443-444.
DOI: 10.1126/science.114.2965.443
Abstract
If a piece of lithium is heated in air in a glass test tube, the metal first darkens becasue the the temperature-accelerated reaction with nitrogen, oxygen and other constituents of the air. At, or a little above, the melting point (1) 186C, a spectacular reaction with the glass occurs. The test tube grows red, then white hot. In a short time, the bottom falls out of it and the metal burns with a brilliant white flame, like that of magnesium. It has been reported (2) that the lithium in this reaction reduces the SiO2 and silicates of the glass to form lithium silicide. Attempts to purify lithium on a laboratory scale by distillation in glass have usually ended in failure, accompanied by a fireworks display similar to that described above. It is the purpose of this paper to show how a glass system can be used to carry out this process.
Effect of Pressure on the Refining of Lithium by Distillation
R. R. Rogers and G. E. Viens
J. Electrochem. Soc.
Vol.98(12) 1951, pp.483-487
DOI:10.1149/1.2778029
Abstract
The experiments described show that lithium containing 0.5 per cent sodium can be refined by distillation in the presence of argon in a straight retort, the refined material containing as low as 0.002 per cent sodium. At gauge pressures up to 1 micron the sodium content differs very little from this value. In increasing the pressure from 1 to 740 microns the sodium content is quadrupled. In the presence of argon, nitrogen, oxygen, and hydrogen at different pressures in a slightly V-shaped retort, a sodium content of less than 0.01 per cent was not obtained. There was little or no evidence of oxide, nitride, or hydride formation at pressures of oxygen, nitrogen, or hydrogen below 35 microns.
The Distillation of Lithium Metal.pdf