Performance of lithium-ion cells using 1 M LiPF6 in EC/DEC (v/v = 1/2) electrolyte with ethyl propionate additive

Kufian, M.Z.; Majid, S.R.

doi:10.1007/s11581-009-0413-6

Cited by 37 publications

(16 citation statements)

References 23 publications

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“…In the neat bulk electrolyte, the activation energy for both Li + diffusion and ferrocene diffusion are 0.12 eV and 0.11 eV, respectively. These values are in good agreement with literature reports on similar electrolytes . In the case of the SEI formed by slow‐scan cyclic voltammetry, the activation energy for Li + diffusion and ferrocene diffusion is also similar, namely 0.29 eV and 0.26 eV.…”

Section: Resultssupporting

confidence: 91%

Influence of the Formation Current Density on the Transport Properties of Galvanostatically Formed Model‐Type Solid Electrolyte Interphases

Kranz

Graubner

et al. 2019

Batteries & Supercaps

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During the production of commercial lithium-ion batteries, the solid electrolyte interphase (SEI) on the graphite particles of the negative electrode is typically formed through galvanostatic protocols with low current densities. Consequently, SEI formation is a time-consuming and rather expensive production step. In order to better understand the influence of the formation current density on the transport of ions and molecules across the SEI, we formed model-type SEIs on planar glassy carbon electrodes under galvanostatic control. In accordance with the expectations from electrochemical nucleation and growth theory, we find that the transport of both ions and molecule becomes slower with increasing formation current density. However, it is remarkable that the ion transport is slowed down more strongly than the molecule transport. We show that at high formation current densities of about À 71 μA cm À 2 , our model-type SEIs clearly exceed the area-specific resistance tolerable in commercial lithium-ion cells.

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Section: Resultssupporting

confidence: 91%

Influence of the Formation Current Density on the Transport Properties of Galvanostatically Formed Model‐Type Solid Electrolyte Interphases

Kranz

Graubner

et al. 2019

Batteries & Supercaps

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“…This lower ionic conductivity of the HCE correlates with its higher viscosity, measured to be 83.15 cP

\pm

0.2 %, consistent with a prior report [39] . Dilute (i.e, 1 m ) LiPF 6 electrolytes in binary carbonate‐based solvents exhibit viscosities <5 cP [40–42] . The Stokes‐Einstein equation establishes an inverse correlation between viscosity and mobility.…”

Section: Resultssupporting

confidence: 89%

Enabling High Capacity and Coulombic Efficiency for Li‐NCM811 Cells Using a Highly Concentrated Electrolyte

Philip

Haasch

Kim

et al. 2020

Batteries & Supercaps

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Lithium metal batteries suffer from dendrite formation and the associated safety hazards of thermal runaway reactions. In this study, we report the performances of a highly concentrated electrolyte (HCE) and a dilute LiPF6 electrolyte in lithium metal cells using LiNi0.8Co0.1Mn0.1O2. While the HCE exhibits lower bulk ionic conductivity than the dilute LiPF6 electrolyte, the cell conductivity is higher for the HCE system, indicating higher thermodynamic stability of the electrolyte against the electrodes. Full cell cycling demonstrates higher capacity for the HCE system, which declines as a function of cycle number due to the formation of decomposition products, similar to the dilute LiPF6 system. The origin of the enhanced performance is the higher stability of the HCE against a Li metal anode as compared to the dilute LiPF6 electrolyte. Cycling at higher temperatures further enhances the performance of the HCE, which is more thermally stable than the dilute LiPF6 electrolyte.

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“…for the production of some antimalarial drugs including pyrimethamine. Ethyl propionate has also other promising areas of application, for example, in the manufacture of lithium batteries [3]. The esterification is one of the main industrial methods of ester synthesis and the data on phase and chemical equilibria are necessary for the process design.…”

Section: Introductionmentioning

confidence: 99%

Chemical equilibrium for the reactive system propionic acid + ethanol + ethyl propionate + water at 303.15 and 313.15 K

Toikka

Sadaeva

Samarov

et al. 2017

Fluid Phase Equilibria

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a b s t r a c tChemical equilibrium for the quaternary system propionic acid þ ethanol þ ethyl propionate þ water was experimentally studied at 303.15 and 313.15 K and atmospheric pressure. The chemically equilibrium compositions were determined by gas chromatography and nuclear magnetic resonance analytical methods. It is shown that chemical equilibrium is reached both in homogeneous and heterogeneous area of composition of reactive mixture. The liquid e liquid equilibrium data for the surface of chemical equilibrium were obtained. The thermodynamic constants of chemical equilibrium at 303.15 and 313.15 K were determined.

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Performance of lithium-ion cells using 1 M LiPF6 in EC/DEC (v/v = 1/2) electrolyte with ethyl propionate additive

Cited by 37 publications

References 23 publications

Influence of the Formation Current Density on the Transport Properties of Galvanostatically Formed Model‐Type Solid Electrolyte Interphases

Influence of the Formation Current Density on the Transport Properties of Galvanostatically Formed Model‐Type Solid Electrolyte Interphases

Enabling High Capacity and Coulombic Efficiency for Li‐NCM811 Cells Using a Highly Concentrated Electrolyte

Chemical equilibrium for the reactive system propionic acid + ethanol + ethyl propionate + water at 303.15 and 313.15 K

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