The Institute for Transuranium Elements ͑ITU͒ is building up an accurate database of actinide behavior in chloride melts in support of its nuclear fuel reprocessing development program. The electrochemical properties of uranium, dissolved in LiCl-KCl eutectic melt, were investigated by transient electrochemical techniques, such as cyclic voltammetry ͑CV͒ and chronopotentiometry on an inert tungsten electrode. It was shown that U 4+ is reduced to U 0 by a two-step mechanism corresponding to U 4+ /U 3+ and U 3+ /U 0 transitions. In the 400-550°C ͑673-823 K͒ range, the diffusion coefficients of U 3+ and U 4+ were similar and equal to: D͑U 3+ ͒ = 13.7 ϫ 10 −4 exp͕−24.2 ϫ 10 3 /RT͑K͖͒ and D͑U 4+ ͒ = 5.25 ϫ 10 −4 exp͕−19.8 ϫ 10 3 /RT͑K͖͒ cm 2 s −1 . The apparent standard potentials of U 4+ /U 3+ and U 3+ /U 0 redox systems were E o* ͑U 4+ /U 3+ ͒͑V͒ = −1.902 + 0.0006104T ͑K͒ vs. Cl 2 /Cl − and E o* ͑U 3+ /U 0 ͒͑V͒ = −3.099 + 0.0007689T ͑K͒ vs. Cl 2 /Cl − , respectively. Some thermochemical properties ͑⌬G * ,␥͒ of uranium solutions were also derived from the electrochemical measurements. The Gibbs free energies of dilute solution of UCl 3 and UCl 4 in the LiCl-KCl were determined to be: ⌬G * = −897.09 + 0.226T ͑K͒ and −183.53 + 0.0589T ͑K͒ in kJ mol −1 , respectively. In the 400-550°C ͑673-823 K͒ range, the activity coefficients ␥ of UCl 3 and UCl 4 range between 0.3 − 4.5 ϫ 10 −3 and 17.1 − 12.7 ϫ 10 −3 , respectively.Pyrochemical reprocessing is a promising method for recycling spent nuclear fuel. Uranium is the major element in most nuclear fuel cycles, thus the assessment of accurate thermochemical data for this element in molten salts is of high importance. Uranium behavior has been studied in many chloride-based melts: for example, MgCl 2 -NaCl-KCl, 1 NaCl-KCl, 2,3 LiCl-NaCl-CaCl 2 -BaCl 2 , 4 and LiCl-KCl eutectic. [5][6][7][8][9][10][11][12][13][14][15] In the literature, the first electrochemical studies on uranium behavior in molten chlorides appeared in 1959. 1,7,8 It was established that the reduction of UCl 4 to uranium metal proceeds via a two-step mechanism, i.e., U 4+ is reduced into U 3+ before forming uranium metal. In a MgCl 2 -NaCl-KCl mixture, Hill et al., 1 who used a platinum needle microelectrode, reported a threeelectron system for the U 3+ /U 0 transition. The apparent standard potential was close to −2.467 V vs. Cl 2 /Cl − at 450°C ͑723 K͒. In the NaCl-KCl eutectic, by electromotive force ͑emf͒ measurements, Flengas 2 measured E o* ͑U 3+ /U 0 ͒͑V͒ = 0.000592T ͑K͒ − 2.973522 vs. Cl 2 /Cl − and E o* ͑U 4+ /U 3+ ͒͑V͒ = 0.000492T ͑K͒ − 1.808311 vs. Cl 2 /Cl − in the 670-850°C ͑943-1123 K͒ range. In the NaCl-KCl eutectic, Serrano et al. 3 showed by cyclic voltammetry ͑CV͒ that the reduction U 3+ to uranium metal is reversible and proceeds through a three-electron mechanism. The diffusion coefficient of U 3+ was determined equal to 5.5 ϫ 10 −5 cm 2 s −1 at 715°C ͑983 K͒. Recently, in LiCl-NaCl-CaCl 2 -BaCl 2 baths, Poa et al. 4 studied the electrochemical reduction of uranium U 3+ to uranium metal b...

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U-Al alloy formation has been studied in the temperature range of 400 -550 °C by electrochemical techniques in the molten LiCl-KCl eutectic. Cyclic voltammetry showed that underpotential reduction of U(III) onto solid Al occurs at a potential about 0.35 V more anodic than pure U deposition. Open circuit potential measurements, recorded after small depositions of U metal onto the Al electrode, did not allow the distinction between potentials associated with UAl x alloys and the Al rest potential, as they were found to be practically identical. As a consequence, a spontaneous chemical reaction between dissolved UCl 3 and Al is thermodynamically possible and was experimentally observed.Galvanostatic electrolyses were carried out both on Al rods and Al plates. Stable and dense U-Al deposits were obtained with high faradic yields, and the possibility to load the whole bulk of a thin Al plate was demonstrated. The analyses (by SEM-EDX and XRD) of the deposits indicated the formation of different intermetallic phases (UAl 2 , UAl 3 and UAl 4 ) depending on the experimental conditions.