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Calcium Oxide의 Hydration Resistance에 關한 硏究
洪允命 연세대학교 대학원 1974 延世論叢 Vol.11 No.1
This study was performed to investigate the hydration resistance of calcia which was sintered below 1,400℃. In this study, the effects by the additives, maturing conditions, hinder addition, compacting pressure, relative humidity, etc., have been studied with a measurement of hydration ratio. Hydration ratio was measured by TGA, X-ray diffraction analysis and weight gain information. Fe2O3, Cr2O3, TiO2 were used as additives and organic compounds such as methanol, toluene, petroleum ether, oleic acid, as binders. As a result, maturing temperature and additive variations are presented as the evidence for the reducing the hydration ratio. Especially, hydration resistance of calcic can be increased by the formation of protective layer of calcium carbonate on the surface. The experiments were operated in a carbon dioxide atmosphere in 700˚∼750℃ On the basis of this study, the optimum conditions were presented when the addition of TiO2 is 0.6∼0.8%, maturing conditions are 1,300℃, 2hr and the addition of petroleum ether+oleic acid as binder.
洪允命,鄭國三 연세대학교 대학원 1980 延世論叢 Vol.16 No.2
This study was performed to investigate the conversion yield from sulfuric acid into sulfur dioxide by thermal catalytic decomposition which was conducted in 950~1200˚K. Experiments were conducted with 98 wt.% sulfuric arid and some metal oxides such as ZnO, CaO, MgO, Fe2O3, MnO2, TiO2 were effective as the catalysts. And the effects by the catalyst content, decomposition temperature, space velocity, initial sulfur trioxide concentration, etc have been studied with a measurement of sulfur dioxide conversion yield which was measured by iodometric analysis method for sulfur dioxide. As a result, TiO2 and Fe2O3 showed the good catalytic activity which may be brought by oxidation reduction reaction and the formation of sulfate or oxide sulfate. Especially, with the increasing of space velocity, sulfur dioxide conversion yield was decreased, but Arrhenius plot was approximately tendenced linear equation.
洪允命 연세대학교 대학원 1969 延世論叢 Vol.6 No.1
This investigation is mainly concerned with producing manganese dioxide in high purity from the domestic Rhodochrosite by the manufacturing process is carried out by reacting the Rhodochrosite sample with sulfuric acid to extract out the manganese sulfate into the acidic solution and electrolyzing the solution thereafter to electrolytically crystallize out the desired manganese dioxide. From the experimental results, the most optimum process is recommended as follows; addition of 30% sulfuric acid to the Rhodochrosite sample pulverized in 80 mesh, and extraction of manganese sulfate for 2 hours yield 93% of efficiency. The folllowed iron removal from the manganese sulfate solution is accomplished by adding a small amount of oxidant and make-up manganese dioxide with heating to oxidize the iron impurities and regulating pH of the solution with calcium hydroxide. According to this procedure, 95% of the original iron content is esaily removed from the solution. When the previously obtained 13% manganese sulfate solution is added with sulfuric acid in such a mole ratio that H2SO4/MnSO4=0.2, the solution shows the highest current efficiency (79%) at 80℃ of the electrolyte and 1.0 A/dm2 of current density. It is also verb advantageous that influence of the residual impurities on the current efficiency in the manganese sulfate electrolyte solution, which is produced by this research investigation, is negligible.
Silica Gel-MoO₃觸媒에 의한 Methanol의 酸化反應
김재구,정국삼,홍윤명 연세대학교 산업기술연구소 1983 논문집 Vol.15 No.2
The vapor phase oxidation of methanol to formaldehyde over silica gel supported-MoO₃catalyst was studied at atmospheric pressure as a function of reaction temperature, feed rate and concentration. The silica gel supported-MoO₃catalyst was found very selective in formaldehyde formation but conversion was rather poor. The following rate equation was deduced assuming a steady state with two stage irreversible oxidation-reduction process. γ= ? The rate equation matched experimental data reasonably well and activation energies of the steps were calculated to be 8.345Kcal/g-mole and 7.074Kcal/g-mole respectively.