Abstract:The electrochemcal reactions of uranium trichloride on the surfaces of dimensionally very dissimilar carbon-based materials such as glassy carbon (GC) and graphene in LiCl-KCl eutectic melt were investigated using cyclic voltammetry (CV) and scanning electron microscopy (SEM). The cathodic scanning of CV displayed that the Li intercalation reaction into the GC electrode governs at the potential of approximately −1.45 V vs. Ag|Ag + where the electrodeposition reaction of uranium may occur. On the other hand, th… Show more
“…Recently pyrochemical processes have attracted significant attention, particularly in the context of recycling spent nuclear fuel. [1][2][3][4] Such pyrochemical processes concern a variety of elements associated with the spent nuclear fuel; 5 most of the uranium is collected in an electro-refining process, 6,7 whereas residual uranium, transuranium (TRU), and lanthanide ions are gathered in an electro-winning process. 8 The TRU and lanthanide elements are reduced at the liquid cadmium cathode, while counter oxidation reactions such as Cl 2 evolution, the oxidation of U 3+ , etc.…”
Electrochemical behavior of ytterbium cations in a LiCl-KCl melt was investigated by electrochemical and UV-VIS absorption spectroscopy methods. In the LiCl-KCl melt, ytterbium exists with divalent and trivalent oxidation states. The electrochemical results showed that the electrochemical reactions of the Yb2+/3+ are reversible and controlled by their diffusion rates. UV-VIS absorption spectroscopy results indicate that the Yb2+ and Yb3+ ions in the LiCl-KCl melt have a few strong absorption bands below 400 nm. Additionally, the molar absorptivities of these electronic transitions of Yb2+ and Yb3+ in LiCl-KCl melt are reported.
“…Recently pyrochemical processes have attracted significant attention, particularly in the context of recycling spent nuclear fuel. [1][2][3][4] Such pyrochemical processes concern a variety of elements associated with the spent nuclear fuel; 5 most of the uranium is collected in an electro-refining process, 6,7 whereas residual uranium, transuranium (TRU), and lanthanide ions are gathered in an electro-winning process. 8 The TRU and lanthanide elements are reduced at the liquid cadmium cathode, while counter oxidation reactions such as Cl 2 evolution, the oxidation of U 3+ , etc.…”
Electrochemical behavior of ytterbium cations in a LiCl-KCl melt was investigated by electrochemical and UV-VIS absorption spectroscopy methods. In the LiCl-KCl melt, ytterbium exists with divalent and trivalent oxidation states. The electrochemical results showed that the electrochemical reactions of the Yb2+/3+ are reversible and controlled by their diffusion rates. UV-VIS absorption spectroscopy results indicate that the Yb2+ and Yb3+ ions in the LiCl-KCl melt have a few strong absorption bands below 400 nm. Additionally, the molar absorptivities of these electronic transitions of Yb2+ and Yb3+ in LiCl-KCl melt are reported.
“…36 The observation of such shift should be due to the formation of insoluble products such as metallic chromium in this case. 37,38 It is worth noting that the anodic peak current A 2 is not linearly correlated with ν 1 / 2 , which is different from the case of the corresponding cathodic current. Similar deviations have been observed for the anodic behaviors of uranium in LiCl-KCl.…”
Section: Diffusion Coefficients Activation Energies and Apparent Stan...mentioning
The speciation and behavior of chromium ions in LiCl-KCl-CrF 3 and LiCl-KCl-LiF-CrF 3 melts were investigated by using cyclic voltammetry, square wave voltammetry, chronopotentiometry and Raman spectroscopy. Electrochemical reduction of Cr(III) to Cr(0) in LiCl-KCl-CrF 3 is a two-step process mediated by the formation of Cr(II). Most Cr(III) ions exist in the form of CrCl 6 3− while CrCl 6-x F x 3− (x ≤ 3) ions are minor in the molten salt medium. Based on the cyclic voltammetric results obtained at different potential scanning rates, the diffusion coefficients of Cr(III) and Cr(II) in LiCl-KCl-CrF 3 melt were determined between 723 and 873 K, and their dependence on temperature can be described as lnD Cr(III) = −4.90-4322.66/T and lnD Cr(II) = −4.71-4007.09/T respectively. The diffusion coefficients of chromium ions in LiCl-KCl-CrF 3 are higher than those in LiCl-KCl-CrCl 3 , which can be explained by the hopping mechanism. In addition, a series of apparent standard potentials of the Cr(III)/Cr(II) and Cr(II)/Cr(0) couples were obtained over the same temperature range using the open-circuit chronopotentiometry technique. With the addition of LiF into the LiCl-KCl-CrF 3 mixture, the dominant chromium species change from CrCl 6 3− to CrCl 6-x F x 3− (x ≤ 6), which is supported by the appearance of the new peaks in both square wave voltammograms and Raman spectra.
“…[22] at 450°C, limiting the potential window of the melt between both reactions [9]. The anodic reactions of the Np species occurred at 0.47 and 0.94 V versus Ag|Ag ?…”
Section: Chemical Reduction Of Npomentioning
confidence: 99%
“…Thus, many electrochemical studies on actinide and lanthanide chloride complexes in molten chloride baths have been performed to elucidate the electrochemical behaviors of such nuclides [4]. In particular, many studies have focused on uranium [5][6][7][8][9] because the pyroprocess was developed primarily for recovering uranium from spent nuclear fuel. However, from the viewpoint of long-term radiotoxicity management of spent nuclear fuel waste, removing long half-life transuraniums (TRUs) from the processing salt bath after uranium recovery is also very important.…”
We prepared neptunium chloride complexes electrochemically and performed spectroelectrochemical measurements of neptunium ions in LiCl-KCl eutectic melts at 450°C, where the neptunium concentrations studied were in the range of 0.1-1 mM. We observed a highly absorbing f-d transition band of Np 3? at 383 nm, which was used to determine an formal potential of the Np 4? |Np 3? redox couple (E°0 = 0.45 V vs. Ag|Ag ? ) with a solution of concentration as low as *0.1 mM. This result agreed well with the value (E°0 = 0.42 V vs. Ag|Ag ? ) determined by cyclic voltammetry with a *15 mM solution.
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