[보고서]고온 용융염 전해환원시스템 개발

허진목

보고서 정보

주관연구기관

한국원자력연구원

연구책임자

허진목

참여연구자

조수행 , 최인규 , 권선길 , 서중석 , 강대승 , 정명수 , 김익수 , 오승철 , 홍순석 , 정상문 , 박병흥 , 최은영 , 박우신 , 임현숙 , 이한수 , 김종국 , 김계훈 , 도재범 , 신호섭 , 유민아 , 이원경 , 이수철 , 이일우 , 이승훈

보고서유형

2단계보고서

발행국가

대한민국

언어

한국어

발행년월

2012-04

과제시작연도

2011

주관부처

교육과학기술부

사업 관리 기관

한국연구재단

등록번호

TRKO201300018157

과제고유번호

1345144864

DB 구축일자

2013-08-26

키워드

전해환원,부피감용,사용후핵연료,용융염,금속전환,실험실규모,공학규모,파이로프로세싱,스케일-업Electrolytic Reduction,Volume Reduction,Spent Fuel,Molten Salt,Metallization,Laboratory-scale,Engineering-scale,Pyroprocessing,Scale-up

표 Fig. 2.1.1 Flowsheet of PYROX Process for LWR Spent Fuel.
표 Fig. 2.1.2 Hot Fuel Dissolution Apparatus(HFDA).
표 Fig. 2.1.3. Bench scale reactor and cathode basket used at INL.
표 Fig. 2.1.4 Secondary circuit concept for an electrolytic reduction of INL.
표 Fig. 2.1.5 Electrolytic reduction equipment concept.
표 Fig. 2.1.7 Electrochemical reduction concept of CRIEPI.
표 Fig. 2.1.6 Material flow of pyroprocessing of MOX spent fuel by electrochemical reduction technology
표 Fig. 2.1.8 Experimental setup for an electrolytic reduction of CRIEPI.
표 Fig. 2.2.1 Vacuum distillation apparatus of LANL.
표 Fig. 2.2.2 Cathode processor of INL.
표 Fig. 2.2.3 (a) Zirconia-based crucible and (b) after cathode processor test.
표 Fig. 2.2.4 (a) Hafnium nitride coated and (b) after cathode processor test.
표 Fig. 2.2.6 Distillation device of CEA.
표 Fig. 2.2.5. Schematic diagram of cathode processor developed in CRIEPI.
표 Fig. 3.1.1.1 Drawing of the modified reactor 20 kgHM/batch.
표 Fig. 3.1.1.2 Position of the modified top flange (a) during a reduction and (b) after a reduction.
표 Fig. 3.1.1.3 Comparison of the top flange (a) before and (b) after a modification.
표 Fig. 3.1.1.4 Comparison of a cathode (a) before and (b) after a modification.
표 Fig. 3.1.1.5 Comparison of an anode module (a) before and (b) after a modification
표 Fig. 3.1.1.6 Temperature profile with a distance from the bottom.
표 Fig. 3.1.1.7 Potential and current profiles with time for the 1st run
표 Fig. 3.1.1.8 Li2O concentration behavior with the time for 1st run
표 Fig. 3.1.1.9 Polarization curves of the cathode and anode for the 1st run.
표 Fig. 3.1.1.10 Potential and current profiles with time for the 2nd run
표 Fig. 3.1.1.11 Li2O concentration behavior with time for the 2nd run
표 Fig. 3.1.1.12 Recovered reduced product
표 Fig. 3.1.1.13. Potential and current profiles with time for the 3rd run.
표 Fig. 3.1.1.14 Li2O concentration behavior with time for the 3rd run.
표 Fig. 3.1.1.15 Polarization curves of the cathode and anode for the 3rd run.
표 Fig. 3.1.2.1 Photographs of the developed stainless steel cathode basket.
표 Fig. 3.1.2.2 Photographs of the vaporized salt on the inside wall of the reactor.
표 Fig. 3.1.2.3 Photographs of heat shields and the reactor after electrolysis.
표 Fig. 3.1.2.4 Li+ potential measurement by using a Pt reference electrode.
표 Fig. 3.1.2.5 Li-Pb alloy and reference electrode prepared in this work.
표 Fig. 3.1.2.6 Photographs of the platinum anodes for old and new electrolytic systems
표 Fig. 3.1.2.7 Photographs of a bench scale electrolytic cell.
표 Fig. 3.1.2.8 Photographs of a lab-scale (20 kgHM/batch) electrolytic cell.
표 Fig. 3.1.2.9 Cyclic voltammogram by using a Li-Pb reference electrode.
표 Fig. 3.1.2.10 Polarization curves in 1wt% Li2O-LiCl molten salt.
표 Fig. 3.1.2.11 Cathode potential, current and applied cell voltage as a function of the electrolysis time
표 Fig. 3.1.2.13 SEM images of U3O8 power and the reduced metal powder.
표 Fig. 3.1.2.12 Photographs of the cross section of the metal basket contained U3O8 powder
표 Fig. 3.1.2.14 TGA and XRD results of the reduced metal powder.
표 Fig. 3.1.2.15 Photographs of the reduced powder in a 1wt% Li2O/LiCl molten salt.
표 Fig. 3.1.2.16 Photographs of the reduced oxide mixtures in a 1wt% Li2O/LiCl molten salt.
표 Fig. 3.1.2.17 Temperature gradient calculated by computational fluid dynamics.
표 Fig. 3.1.2.18 Temperature gradient with a variation of the heating time calculated by computational fluid dynamics
표 Fig. 3.1.2.19 Design drawing of 20 kgHM/batch electrolytic reactor.
표 Fig. 3.1.2.21 Photographs of unit parts of a lab scale reactor and 3D image.
표 Fig. 3.1.2.20 Photographs of cathode basket and anode assembly.
표 Fig. 3.1.2.22 Furnace for high-temperature voloxidation of U3O8 powder.
표 Fig. 3.1.2.23 Design drawing and photograph of an Ar-glove box system.
표 Fig. 3.1.2.24 Photographs of cathode operation and power supply system.
표 Fig. 3.1.3.1 Analysis of the potential gradient and the electric field in the molten salt in the absence of MgO shroud around a platinum anode.
표 Fig. 3.1.3.2 Analysis of the potential gradient and the electric field in the molten salt when MgO shroud is located up to the center of platinum anode
표 Fig. 3.1.3.3 Analysis of the potential gradient and the electric field in the molten salt in case of a fully covered MgO shroud around platinum anode
표 Fig.3.1.3.4 Material balance around the electrochemical reduction process.
표 Fig. 3.1.4.1 Macroscopic and microscopic images of the prepared U3O8 SIMFUEL granule
표 Fig. 3.1.4.2 Cathode potential, current and applied voltage during the electrolytic reduction of SIMFUEL granule and a cross-sectional view of the reduced granule
표 Fig. 3.1.4.3 Macroscopic and microscopic images of the UO2 SIMFUEL.
표 Fig. 3.1.4.4 Cathode potential, current and applied voltage during the electrolytic reduction of SIMFUEL granule and a cross-sectional view of the reduced granule.
표 Fig. 3.1.4.5 Macroscopic and microscopic images of a dense pellet after electrolysis.
표 Fig. 3.1.5.1 Stability of oxides.
표 Fig. 3.1.5.2 Diffusion evaporation of salts.
표 Fig. 3.1.5.3 Melting system and vessel.
표 Fig. 3.1.5.4 The used crucibles.
표 Fig. 3.1.5.5 Products from melting experiments.
표 Fig. 3.1.5.7 Reactions between U and Li2O.
표 Fig. 3.1.5.6 Stability of oxides (U-O-Li).
표 Fig. 3.1.5.8 Thermodynamic equilibrium compositions.
표 Fig. 3.1.5.9 Reactions between U3O8 and Li measured by DSC.
표 Fig. 3.1.5.11 Reduction by reaction with metals.
표 Fig. 3.1.5.10 Sintered U3O8 formed by the reaction with Li.
표 Fig. 3.1.5.12 U melting with Li and Fe.
표 Fig. 3.1.5.13 Filling and solidification of molten salts.
표 Fig.3.1.6.1. Procedure of lab-scale electrolytic reduction experiments.
표 Fig. 3.1.6.2. CAD drawing of lab-scale electrolytic reduction system.
표 Fig. 3.1.6.3. CAD drawing of electrodes for lab-scale electrolytic reduction system
표 Fig. 3.1.6.4. Oil seal and cold trap.
표 Fig.3.1.6.8. Li-Pb reference electrode.
표 Fig. 3.1.6.5. Photograph of furnace.
표 Fig.3.1.6.6. Cathode basket.
표 Fig.3.1.6.7. Pt anode and shroud
표 Fig.3.1.6.10. Chemical structure of acrowax
표 Fig.3.1.6.9. Photographs of (a) a glove box, which is thoroughly controlled with high purity argon gas. (b) top view of lab-scale electrolysis cell
표 Fig. 3.1.6.11. Pelletizer used for preparation of UOx pellets.
표 Fig. 3.1.6.12. Procedure of UOx pellets preapration.
표 Fig. 3.1.6.13. Schematic diagram of apparatus for moisture removal in LiCl (left); its top-view photograph
표 Fig.3.1.6.14. Detailed procedure of lab-scale electrolytic reduction experiments.
표 Fig.3.1.6.15. Applied voltage-time plot during electrolysis of 1.88 kg-uranium oxide pellet in a Li2O/LiCl molten salt at 650 °C.
표 Fig.3.1.6.16. Cathode potential-time plot during electrolysis of 1.88 kg-uranium oxide pellet in a Li2O/LiCl molten salt at 650 °C.
표 Fig.3.1.6.17. Current-time plot during electrolysis of 1.88 kg-uranium oxide pellet in a Li2O/LiCl molten salt at 650 °C.
표 Fig.3.1.6.20. Photograph of cathode basket (left) before and (right) after electrolytic reduction of 1.88 kg-oxide pellet.
표 Fig.3.1.6.18. Photograph of the cross-section of a partially reduced uranium oxide pellet.
표 Fig.3.1.6.19. Photograph of anode after electrolytic reduction of 1.88 kg-oxide pellet
표 Fig.3.1.6.21. Applied voltage-time plot during electrolysis of 17 kg-uranium oxide pellet in a Li2O/LiCl molten salt at 650 °C.
표 Fig.3.1.6.22. Cathode potential-time plot during electrolysis of 17 kg-uranium oxide pellet in a Li2O/LiCl molten salt at 650 °C.
표 Fig. 3.1.6.23. Current-time plot during electrolysis of 17 kg-uranium oxide pellet in a Li2O/LiCl molten salt at 650 °C.
표 Fig. 3.1.6.24. Photograph of anode after electrolytic reduction of 17 kg-oxide pellet.
표 Fig. 3.1.6.26. Photograph of the cross-secton of a reduced uranium oxide pellet.
표 Fig. 3.1.6.25. Photograph of cathode basket after electrolytic reduction of 17 kg-oxide pellet
$Fig. 3.1.6.27. X-ray diffraction patterns of the reduced sample.$ 표 Fig. 3.1.6.27. X-ray diffraction patterns of the reduced sample.
표 Fig. 3.1.6.28. Thermal gravimetric analysis of the reduced sample.
표 Fig. 3.2.1.1 Compounds of MgO-MgAl2O4 and MgO-Mg2TiO4.
표 Fig. 3.2.1.3 Compounds of Li2MgSiO4 and Mg2SiO4-Mg2TiO4.
표 Fig. 3.2.1.2 Compounds of CaMgSiO4 and CaTiO3.
표 Fig. 3.2.1.4 Compound-CaMgSiO4 and potential curve.
표 Fig. 3.2.1.6 DTA-TG curve of MgO-SiO2.
표 Fig. 3.2.1.5 DTA-TG curves of CaO and SiO2.
표 Fig. 3.2.1.8 Cross-sectional SEM image and EDS result of surface defect.
표 Fig. 3.2.1.7 Mg-Si-Ca-O oxide in grain boundaries.
표 Fig. 3.2.1.9 Surface defect of pressing MgO filter and potential curve (0.8A).
표 Fig. 3.2.1.10 Surface defect of pressing MgO filter and potential curve (1.0A).
표 Fig. 3.2.1.11 Surface defect of casting MgO filter and potential curve (0.5A).
표 Fig. 3.2.1.12 Surface defect of casting MgO filter and potential curve (0.8A).
표 Fig. 3.2.1.13 Rupture strength of MgO specimen as a function of porosity and time.
표 Fig. 3.2.1.14 Rupture strength of MgO specimen as a function of porosity and Li2O concentration.
표 Fig. 3.2.1.15 Rupture strength of MgO-additives specimen as a function of additives amount
표 Fig. 3.2.1.16 DTA-TG curves of MgO and SiO2.
표 Fig. 3.2.1.18 DTA-TG curves of MgO-Al2O3 and MgO-ZrO2.
표 Fig. 3.2.1.17 DTA-TG curves of CaO and MgO-Y2O3.
표 Fig. 3.2.1.19 XRD patterns of the MgO-Y2O3 (a), MgO-Al2O3 (b) and MgO-ZrO2 (c).
표 Fig. 3.2.1.20 Cross-sectional SEM image and the elemental distribution of MgO-Al2O3-SiO2-CaO-TiO2.
표 Fig. 3.2.1.21 Cross-sectional SEM image and the elemental distribution of MgO-Al2O3 (a) and MgO-Y2O3.
표 Fig. 3.2.1.22 Cross-sectional SEM image and the elemental distribution of MgO-ZrO2
표 Fig. 3.2.2.1 Cross-sectional SEM image, elemental distribution and XRD pattern of Type 304 S.S.
표 Fig. 3.2.2.2 Cross-sectional SEM image, elemental distribution and XRD pattern of Type 316 S.S.
표 Fig. 3.2.2.3 XRD patterns of Inconel 600.
표 Fig. 3.2.2.4 Cross-sectional SEM image and elemental distribution of Inconel 600.
표 Fig. 3.2.2.5 Potential curves of Inconel 600.
표 Fig. 3.2.2.6 XRD patterns of Inconel 713LC.
표 Fig. 3.2.2.8 Potential curves of Inconel 713LC.
표 Fig. 3.2.2.7 Cross-sectional SEM image and elemental distribution of Inconel 713LC
표 Fig. 3.2.2.9 XRD patterns of Superalloy N-1.
표 Fig. 3.2.2.10 Cross-sectional SEM image and elemental distribution of Superalloy N-1
표 Fig. 3.2.2.11 Cross-sectional SEM image and elemental distribution of Superalloy N-1.
표 Fig. 3.2.2.13 Tafel plot of Type 316 S.S in molten salt of LiCl-1%Li2O.
표 Fig. 3.2.2.12 Potential curves of Superalloy N-1.
표 Fig. 3.2.2.14 Cross-sectional SEM image and elemental distribution of Type 316 S.S.
표 Fig. 3.2.2.15 Tafel plot of Incoloy 800H in molten salt of LiCl-1%Li2O.
표 Fig. 3.2.2.16 Cross-sectional SEM image and elemental distribution of Incoloy 800H
표 Fig. 3.2.2.17 Tafel plot of Inconel 625 in molten salt of LiCl-1%Li2O.
표 Fig. 3.2.2.18 Cross-sectional SEM image and elemental distribution of Inconel 625.
표 Fig. 3.2.2.19 Tafel plot of Superalloy N-9 in molten salt of LiCl-1%Li2O.
표 Fig. 3.2.2.20 Cross-sectional SEM image and elemental distribution of Superalloy N-9.
표 Fig. 3.2.3.1 Pt electrode photo and potential curve(Li2O concentration > 1 wt.%).
표 Fig. 3.2.3.3 Uniform corrosion of Pt electrode and potential curve(Li2O concentration < 0.3 wt.%).
표 Fig. 3.2.3.2 Local corrosion of Pt electrode and potential curve(Li2O concentration < 0.6 wt.%).
표 Fig. 3.2.3.4 XRD pattern of corrosion product and potential curve of localized Pt electrode.
표 Fig. 3.2.3.5 XRD pattern of corrosion product and potential curve of uniformed Pt electrode
표 Fig. 3.2.3.7 Photo and cross-sectional SEM image and elemental distribution of uniformed Pt electrode.
표 Fig. 3.2.3.6 Photo and cross-sectional SEM image and elemental distribution of localized Pt electrode
표 Fig. 3.2.3.8 XRD patterns of Pt electrode corroded at 650℃ in molten salt of LiCl-1%Li2O as a function of reaction time.
표 Fig. 3.2.3.9 XRD patterns of Pt electrode corroded at 650℃ in molten salt of LiCl-3%Li2O as a function of reaction time
표 Fig. 3.2.3.10 Cross-sectional SEM image and elemental distribution of Pt electrode corroded at 650℃ for 72 h in molten salt of LiCl-1%Li2O.
표 Fig. 3.2.3.11 Cross-sectional SEM image and elemental distribution of Pt electrode corroded at 650℃ for 72 h in molten salt of LiCl-3%Li2O.
표 Fig. 3.2.3.12 Cross-sectional SEM image and elemental distribution of Pt electrode corroded at 650℃ for 216 h in molten salt of LiCl-1%Li2O.
표 Fig. 3.2.3.13 Cross-sectional SEM image and elemental distribution of Pt electrode corroded at 650℃ for 216 h in molten salt of LiCl-3%Li2O.
표 Fig. 3.2.4.2 XRD pattern of the sintered SrZrO3 body(1,400oC, 5hrs).
표 Fig. 3.2.4.1 Formed and sintered bodies of reaction production from SrCO3 and ZrO2.
표 Fig. 3.2.4.3 XRD pattern of the reaction production from BaCO3 and ZrO2.
표 Fig. 3.2.4.4 XRD pattern of the reaction production from SrCO3 and SnO2.
표 Fig. 3.2.4.5 Formed bodies of reaction production from CaCO3 and SnO2.
표 Fig. 3.2.4.6 Formed and sintered bodies of reaction production from BaCO3 and SnO2.
표 Fig. 3.2.4.8. SEM photograph and data analysis of the sintered body for SrRuO3 with 3mol% CaSiO3(1,400℃, 5hrs).
표 Fig. 3.2.4.7. Formed and sintered bodies for SrRuO3 with 3mol% CaSiO3.
표 Fig. 3.2.4.9 Variation of the electrical conductivity according to temperature for the sintered SrRuO3 with 3mol% CaSiO3
표 Fig. 3.2.4.10 Formed and sintered bodies for BaRuO3 with 3mol% CaSiO3.
표 Fig. 3.2.4.11 Photograph of resistance measurement for the sintered BaRuO3 with 3mol% CaSiO3.
표 Fig. 3.2.4.12 XRD pattern of the reaction production from RuO2(1/3), SnO2(2/3) and SrCO3(1).
표 Fig. 3.2.4.13 XRD pattern of the reaction production from RuO2(1/2), SnO2(1/2) and SrCO3(1).
표 Fig. 3.2.4.14 XRD pattern of the reaction production from RuO2(2/3), SnO2(1/3) and SrCO3(1).
표 Fig. 3.2.4.15 Photographs of SEM and resistance measurement for the sintered SrRuO3-SrSnO3 mixture.
표 Fig. 3.2.4.16 XRD patterns and SEM photographs of the sintered SrRuO3-3mol% CaTiO3 according to sintering time at 1,200℃.
표 Fig. 3.2.4.17 XRD patterns and SEM photographs of the sintered SrRuO3-3mol% CaTiO3 according to sintering time at 1,300℃.
표 Fig. 3.2.4.18 XRD patterns and SEM photographs of the sintered SrRuO3-3mol% CaTiO3 according to sintering time at 1,400℃.
표 Fig. 3.2.4.19 XRD patterns and SEM photographs of the sintered SrRuO3-3mol% CaTiO3 according to sintering time at 1,500℃.
표 Fig. 3.2.4.20 XRD patterns and SEM photographs of the sintered SrRuO3-3mol% CaSiO3 according to sintering time at 1,200℃.
표 Fig. 3.2.4.21 XRD patterns and SEM photographs of the sintered SrRuO3-3mol% CaSiO3 according to sintering time at 1,300℃.
표 Fig. 3.2.4.22 XRD patterns and SEM photographs of the sintered SrRuO3-3mol% CaSiO3 according to sintering time at 1,400℃.
표 Fig. 3.2.4.23 XRD patterns and SEM photographs of the sintered SrRuO3-3mol% CaSiO3 according to sintering time at 1,500℃.
표 Fig. 3.2.4.24 XRD patterns and SEM photographs of the sintered SrRuO3-5mol% CaSiO3 according to sintering time at 1,200℃.
표 Fig. 3.2.4.25 XRD patterns and SEM photographs of the sintered SrRuO3-5mol% CaSiO3 according to sintering time at 1,400℃.
표 Fig. 3.2.4.26 XRD patterns and SEM photographs of the sintered SrRuO3-5mol% CaSiO3 according to sintering time at 1,500℃.
표 Fig. 3.2.4.27 XRD patterns and SEM photographs of the sintered SrRuO3-7mol% CaSiO3 according to sintering time at 1,400℃.
표 Fig. 3.2.4.28 XRD patterns and SEM photographs of the sintered SrRuO3-7mol% CaSiO3 according to sintering time at 1,500℃.
표 Fig.3.2.5.1. Schematic drawing of (a) SWV and (b) electrolytic reduction
표 Fig.3.2.5.2. Square wave voltammogrames at various concentrations (0.00 ~ 0.77 wt% of Li2O) SWV parameters
표 Fig.3.2.5.3. Relationship of Li2O concentration vs applied charges during electrolytic reduction of 3.0 V [inset] square wave voltammogramesof different applied charges.
표 Fig.3.2.5.4. Relationship of Li2O concentration vs applied charges during electrolytic reduction of 3.0 V [inset] square wave voltammogramesof different applied charges
표 Fig. 3.3.1.1 Electrochemical measurement system
표 Fig.3.3.1.2 Cathodic cyclic voltammogram of 3wt% LiBr in LiCl molten salt at 650℃ (scan rate = 50mV/sec).
표 Fig. 3.3.1.3 Anodic cyclic voltammogram of 3wt% LiBr in LiCl molten salt at 650℃.
표 Fig. 3.3.1.4 Electrode potentials during the electrolysis of LiBr in LiCl molten salt at 650℃.
표 Fig. 3.3.1.5 Electrolysed LiCl salt of 3wt% LiBr with 100mA reduction current
표 Fig. 3.3.1.6 Electrolysed LiCl salt of LiBr after washing with water
표 Fig. 3.3.1.7 Cathodic cyclic voltammogram of 3wt% LiI in LiCl molten salt at 650℃ (scan rate = 50mV/sec).
표 Fig. 3.3.1.8 Anodic cyclic voltammogram of 3wt% LiI in LiCl molten salt at 650℃.
표 Fig. 3.3.1.9 Electrode potentials during the electrolysis of LiI in LiCl molten salt at 650℃.
표 Fig. 3.3.1.10 After electrolysis of LiI in LiCl salt with 200 and 250mA reduction current
표 Fig. 3.3.1.11 Iodine deposition on the anode after LiI electrolysis
표 Fig. 3.3.1.12 Cathodic cyclic voltammogram of 3wt% Li2Se in LiCl molten salt at 650℃ (scan rate = 50mV/sec).
표 Fig. 3.3.1.13 Anodic cyclic voltammogram of 3wt% Li2Se in LiCl molten salt at 650℃.
표 Fig. 3.3.1.14 Electrode potentials during the electrolysis of Li2Se in LiCl molten salt at 650℃.
표 Fig. 3.3.1.15 Precipitates after the electrolysis of Li2Se in LiCl with 400mA current for 1 hour.
$Fig. 3.3.1.16 X-ray diffraction pattern of precipitates in LiCl molten salt after the electrolysis of 3wt% Li2Se at 650℃.$ 표 Fig. 3.3.1.16 X-ray diffraction pattern of precipitates in LiCl molten salt after the electrolysis of 3wt% Li2Se at 650℃.
표 Fig.3.3.2.1 Schematic description of a reduction container
표 Fig. 3.3.2.2 Li2O concentration change for a blank test.
표 Fig. 3.3.2.3. Li2O concentration change during RE2O3 reduction by Li metal in a molten LiCl salt.
표 Fig. 3.3.2.4 Li2O concentration change during LiYO2 and Y2O3 reduction by Li metal in a molten LiCl salt.
표 Fig. 3.3.2.5 Li2O concentration change during Lu2O3 and Sc2O3 reduction by Li metal in a molten LiCl salt.
표 Fig. 3.3.2.6 XRD patterns of Li-Li2O-Sc2O3 reaction product and Sc2O3
표 Fig. 3.3.2.7 XRD patterns of Li-Li2O-Lu2O3 reaction product and Lu2O3
표 Fig. 3.3.3.1 Cyclic voltammogram of platinum wire as a function of scan rates.
표 Fig. 3.3.3.2 Relationship between peak maximum current and scan rate.
표 Fig. 3.3.4.1 Concept of a semi-empirical model.
표 Fig. 3.3.4.2 Comparison of calculated reduction yield with experimental data.
$Fig. 3.3.4.3 Unreduced oxide fraction of an integrated cathode.$ 표 Fig. 3.3.4.3 Unreduced oxide fraction of an integrated cathode.
표 Fig. 3.3.4.4 Time for complete reduction with applied current.
표 Fig. 3.4.1.1 P-T diagram of LiCl.
표 Fig. 3.4.1.2 Porous MgO chips for solid-liquid separation of LiCl.
표 Fig. 3.4.1.4 Recovered MgO chips after a run.
표 Fig. 3.4.1.3 MgO chips before LiCl wetting.
표 Fig. 3.4.1.5 Porous MgO wetted by LiCl.
표 Fig. 3.4.1.6 MgO sticks and basket (top), before LiCl wetting (middle), after LiCl wetting (bottom).
표 Fig. 3.4.1.7 Li2O-U reaction Gibbs energy.
표 Fig. 3.4.1.8 U-Fe phase diagram.
표 Fig. 3.4.1.9 SEM images ((a) section A, (b) section B) and element analyses ((C) section A, (d) section B) results of SR004-B.
표 Fig. 3.4.1.10 Apparatus for distillation rate measurement.
표 Fig. 3.4.1.11 LiCl Weight decrease behavior by distillation.
표 Fig. 3.4.1.12 LiCl weight decrease behavior from porous MgO rods of 20% porosity and 10 cm length with different diameter
표 Fig. 3.4.1.13. LiCl weight decrease behavior from porous MgO rods of 20% porosity and 15 mm diameter with different length.
표 Fig. 3.4.1.14 LiCl weight decrease behavior from porous MgO rods of 15 mm diameter and 10 cm length with different porosity
표 Fig. 3.4.1.15 Schematic diagram of a batch-type cathode processor.
표 Fig. 3.4.1.17 Reactor after distillation at 700 oC and ∼200 Torr.
표 Fig. 3.4.1.16 Reactor after distillation at 700 oC and < 20 mTorr.
표 Fig. 3.4.1.18. Recovery of received LiCl.
표 Fig. 3.4.1.19 Microscopic images of recovered LiCl.
표 Fig. 3.4.1.20 Average distillation rate and the amount of distilled salt with time.
표 Fig. 3.4.2.1 Sketch of PRIDE electrolytic reducer.
표 Fig. 3.4.2.2 Design basis of PRIDE electrolytic reducer.
표 Fig. 3.4.2.3 Sketch of PRIDE cathode processor.
표 Fig. 3.5.1.2. 650 °C, LiCl (205 g)-1 wt.% Li2O 조건에서의 2.3 g UO2 전해환원시험
표 Fig. 3.5.1.1. 전극 표면적 영향 평가 시험에 사용된 전해환원장치 모사도.
표 Fig. 3.5.1.3. XRD 패턴과 사진
표 Fig. 3.5.1.4. 전류밀도와 음극 전위에 음극/양극 표면적비가 미치는 영향.
표 Fig. 3.5.1.5. 음극/양극 표면적비 효과를 조사하기 위한 전극배치
표 Fig. 3.5.1.6. 용융염 양이 전해환원 효율에 미치는 영향평가 위한 시험장치 모사도.
표 Fig. 3.5.1.7. 650 °C, LiCl (150 g)-1 wt.% Li2O 조건에서의 2.3 g UO2 전해환원시험
표 Fig. 3.5.1.8. 650 °C, LiCl (200 g)-1 wt.% Li2O 조건에서의 2.3 g UO2 전해환원시험
표 Fig. 3.5.1.9. 음극/양극 표면적비가 미치는 영향
표 Fig. 3.5.2.1. 음극-양극간 거리 효과를 조사하기 위한 장치의 상부 플랜지
표 Fig. 3.5.2.2. 음극-양극 위치 조정에 따른 다양한 음극-양극 거리
표 Fig. 3.5.3.1. 다양한 음극바스켓 형태가 전해환원 효율에 미치는 영향.
표 Fig. 3.5.3.2. 다양한 cathode basket
표 Fig. 3.5.3.3. 본 연구에서 사용된 음극 바스켓 (a) 3중 겹 (b) 단일 겹.
표 Fig. 3.5.3.4. 양극 shroud와 양극 길이비에 따른 전류밀도 분포 및 총 플럭스
표 Fig. 3.5.3.5. 양극 shroud 위치에 따른 전류밀도분포
표 Fig. 3.5.3.5. 양극 shroud 위치에 따른 총 플럭스
표 Fig. 3.5.4.1. 금속 튜브를 이용한 기준전극 제조.
표 Fig. 3.5.4.2. STS 튜브를 이용한 기준전극 test 결과.
표 Fig. 3.5.5.1. 희토류산화물의 전해환원반응에서 음극 전위 거동.
표 Fig. 3.5.5.2. 우라늄과 희토류 혼합산화물의 환원전위 거동.
표 Fig. 3.5.6.1. 전해환원시험에 도입된 산화물 원료형태.
표 Fig. 3.5.6.2. 전해환원시험 후 원료형상.
표 Fig. 3.5.6.3. ZrO2 전해환원 실험 장치 모식도.
표 Fig. 3.5.6.4. Zr과 Li2O의 화학반응에 의한 전해환원에 대한 저해 화합물 발생여부 검증 실험 절차
표 Fig. 3.5.6.5. ZrO2와 Li2O의 화학반응에 의한 전해환원에 대한 저해 화합물 발생여부 검증 실험 절차.
표 Fig. 3.5.6.6. 650 °C, LiCl (250 g)-1 wt.% Li2O 조건에서의 5.06 g ZrO2 시편 전해환원 실험 결과
표 Fig. 3.5.6.7. 전해환원 후 ZrO2 환원체에 대한 XRD 분석결과.
표 Fig. 3.5.6.8. ZrO2와 Li2O의 화학반응 후 XRD 분석결과. 반응온도 650oC.
표 Fig. 3.5.6.9. Zr와 Li2O의 화학반응 후 XRD 분석결과. 반응온도 650oC.
표 Fig. 3.5.6.10. 산화물 원료형태가 전해환원에 미치는 영향을 조사하기 위하여 사용된 전해환원 셀
표 Fig. 3.5.6.11. Schematic diagram of a model.
표 Fig. 3.5.6.12. 수치해석에 의해 계산된 우라늄 산화물 펠렛의 금속전환에 필요한 시간
표 Fig. 3.5.8.1. 다양한 Li2O 농도조건에서, Pt 양극의 Cyclic Voltammograms.
표 Fig. 3.5.8.2. Peak 전위이동 vs log[Li2O].
표 Fig. 3.5.8.4. CA에 의한 전류-시간 곡선.
표 Fig. 3.5.8.5. 전류 vs Li2O 농도.
표 Fig. 3.5.8.3. Peak 전류 vs log[Li2O].
표 Fig. 3.5.9.1. 전해환원장치 열 전산모사.
표 Fig. 3.5.9.2. 전해환원장치 양극 기체 배출 전산모사.
표 Fig. 3.5.9.3. 전해환원장치 전기장 전산모사.
표 Fig. 3.5.11.1. Lab-scale 전해환원 장치 플랜지에 level 측정센서 설치 사진.
표 Fig. 3.5.11.2. 용융염 level 측정 결과
표 Fig. 3.5.12.1. Lab scale과 PRIDE OR 내부 전류밀도분포 및 총 플럭스 분포
표 Fig. 3.5.12.2. PRIDE OR 양극 반응점.
표 Fig. 3.6.1.1. Bench scale 용융염 증발회수 장치.
표 Fig. 3.6.1.2. Bench-scale 용융염 증발 회수장치 설계 개선 및 장치제작.
표 Fig. 3.6.1.3. 용융염 증발 회수장치의 열 및 압력 분포 모사.
표 Fig. 3.6.1.4. 금속전환체의 잔류염 제거 시험.
표 Fig. 3.6.1.5. Cathode Processor Ar 재순환 시스템.
표 Fig. 3.6.2.1. Lab-scale 용융염 증발회수 장치.
표 Fig. 3.6.2.2. 조업 온도 profile.
표 Fig. 3.6.3.1. LiCl 용융염증발실험 온도곡선.
표 Fig. 3.6.2.3. Lab-scale 용융염 증발회수 시험 사진.
표 Fig. 3.6.3.2. LiCl 용융염 주입량의 변화에 따른 리시버의 온도 변화.
표 Fig. 3.6.3.3. LiCl 용융염 증발완료 소요시간.
표 Fig. 3.6.3.4. Li2O-LiCl 용융염 증발시의 리시버 온도 변화.
표 Fig. 3.6.4.1. 우라늄 금속전환체 증류시의 리시버 온도변화.

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