Electrochemical investigtion of solubility and chemical diffusion of lithium in aluminum

Chen, Wen; Weppner, W.; Boukamp, Bernard A.; Huggins, Robert A.

doi:10.1007/bf02657182

Cited by 104 publications

(92 citation statements)

References 13 publications

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“…During discharge some Li remains in the Al (the a-phase is kept, only the b-phase is cycled), so that the Li x Al is cycled within the stoichiometric range of~0.1 < x <~1 (~50 at.-% Li). [318] The matrix metal accepts negative charges during the insertion of Li + ). For this reason they are usually fairly brittle.…”

Section: Lithium Alloys As Negative Insertion Electrode Materialsmentioning

confidence: 99%

“…Also, in the case of pure aluminum, alloying with lithium occurs with several successive phase formations: the formation of the a-phase (up tõ 7 at.-% Li in LiAl), b-phase (a non-stoichiometric phase with~47 to~56 at.-% Li), and several lithium-rich phases. [309,318,322] The lithium alloy denoted in the technical literature as ªLiAlº is frequently used as an insertion electrode material. It is a two-phase mixture of the a-phase and the b-phase.…”

Section: Lithium Alloys As Negative Insertion Electrode Materialsmentioning

confidence: 99%

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Insertion Electrode Materials for Rechargeable Lithium Batteries

Winter¹,

et al. 1998

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Section: Lithium Alloys As Negative Insertion Electrode Materialsmentioning

confidence: 99%

Section: Lithium Alloys As Negative Insertion Electrode Materialsmentioning

confidence: 99%

Insertion Electrode Materials for Rechargeable Lithium Batteries

Winter¹,

et al. 1998

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“…Galvanostatic intermittent titration technique ͑GITT͒, potentiostatic intermittent titration technique ͑PITT͒, and electrochemical impedance spectroscopy ͑EIS͒ are frequently used methods to determine D of guest species in various inorganic hosts. [8][9][10] Recent advances regarding the analysis of these methods include correction for non-negligible charge transfer and Ohmic resistances in the PITT case 11 and introduction of anomalous diffusion when analyzing EIS data. 12 In chronopotentiometry ͑CP͒ and GITT experiments the quasi-steady-state potential is measured as ions are intercalated into the material.…”

Section: Introductionmentioning

confidence: 99%

Determination of solid phase chemical diffusion coefficient and density of states by electrochemical methods: Application to iridium oxide-based thin films

Backholm

Georén

Niklasson

2008

Journal of Applied Physics

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Potentiostatic intermittent titration technique ͑PITT͒ and electrochemical impedance spectroscopy ͑EIS͒ were investigated as methods to determine solid phase chemical diffusion coefficient ͑D͒ and electronic density of states ͑DOS͒. These techniques were then applied to iridium oxide ͑IrOx͒ and iridium-tantalum oxide ͑IrTaOx͒ thin films prepared by sputter deposition. The experiments, performed in 1M propionic acid between −0.2 and 0.8 V vs Ag/ AgCl, showed effects of interfacial side reactions, whose contribution to the electrochemical response could be identified and corrected for in the case of PITT as well as EIS. It was found that D is strongly underestimated when using PITT with the common Cottrell formalism, which follows from non-negligible interfacial charge transfer and Ohmic resistances. EIS indicated an anomalous diffusion mechanism, and D was determined to be in the 10 −11 -10 −10 cm 2 / s range for IrOx and IrTaOx. Both PITT and EIS showed that the intercalated charge as a function of potential exhibits a shape that resembles the theoretical DOS of crystalline iridium oxide, especially for IrTaOx.

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“…which can be written as: (14) In this equation Q is the integrated quantity of diffusing species in the whole matrix, which is related to the flux D dc/dx at the plane jc = 0, this means that the value of D corresponds to the concentration at the boundary of the electrode as it is defined by the potentiostatic signal. …”

Section: Frjmentioning

confidence: 99%

“…To this latter case belongs the technique of metalliding [7] which involves simultaneous electrodeposition and solid state intermetallic diffusion in molten salt systems at elevated temperatures [8][9][10][11][12][13][14], The subject has recently been reviewed by R. S. Sethi [15]. For reversible electrochemical reactions the activity of the electroactive material is obtained by e.m.f.…”

Section: Introductionmentioning

confidence: 99%

Chronoamperometric Determination of Solid State Diffusion Coefficients in Copper-Gold Alloys Using a Molten Salt Electrolyte

Lantelme

Chemla

1983

Zeitschrift Für Naturforschung A

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The intermetallic diffusion coefficient in Cu-Au alloy between 400 °C and 550 °C is measured by chronoamperometry using a Cu-Au electrode in a molten LiCl-KCl electrolyte containing small amounts of Cu+ ions. The current response to a defined constant potential step is controlled by the rate of diffusion in the alloy electrode. The mathematical treatment developed by introducing the Boltzman transformation shows that the current density is a linear function of the reciprocal square root of time whatever the dependence of D versus concentration is. The method is applied to cathodic as well as anodic potential pulses which correspond to surface alloying or dissolution i.e. diffusion "in" or "out" the sample. The shift of the interface due to the copper deposition or dissolution is considered according to the Oldham and Raleigh's method. By studying the electrochemical response at very short times the diffusion can be examined in the first atomic layers of the electrode interface.

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Electrochemical investigtion of solubility and chemical diffusion of lithium in aluminum

Cited by 104 publications

References 13 publications

Insertion Electrode Materials for Rechargeable Lithium Batteries

Insertion Electrode Materials for Rechargeable Lithium Batteries

Determination of solid phase chemical diffusion coefficient and density of states by electrochemical methods: Application to iridium oxide-based thin films

Chronoamperometric Determination of Solid State Diffusion Coefficients in Copper-Gold Alloys Using a Molten Salt Electrolyte

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