21 research outputs found
Experimental and Computational Analysis of the Solvent-Dependent O2/Li+-O2ā Redox Couple: Standard Potentials, Coupling Strength, and Implications for Lithium-Oxygen Batteries
Understanding and controlling the kinetics of O[subscript 2] reduction in the presence of Li+-containing aprotic solvents, to either Li+-O[subscript 2]ā by one-electron reduction or Li[subscript 2]O[subscript 2] by two-electron reduction, is instrumental to enhance the discharge voltage and capacity of aprotic Li-O[subscript 2] batteries. Standard potentials of O[subscript 2]/Li+-O[subscript 2]ā and O[subscript 2]/O[subscript 2]ā were experimentally measured and computed using a mixed cluster-continuum model of ion solvation. Increasing combined solvation of Li+ and O[subscript 2]ā was found to lower the coupling of Li+-O[subscript 2]ā and the difference between O[subscript 2]/Li+-O[subscript 2]ā and O[subscript 2]/O[subscript 2]ā potentials. The solvation energy of Li+ trended with donor number (DN), and varied greater than that of O[subscript 2]ā ions, which correlated with acceptor number (AN), explaining a previously reported correlation between Li+-O[subscript 2]ā solubility and DN. These results highlight the importance of the interplay between ionāsolvent and ionāion interactions for manipulating the energetics of intermediate species produced in aprotic metalāoxygen batteries.National Science Foundation (U.S.) (NSF award no. ECS-0335765)China Clean Energy Research Center-Clean Vehicles Consortium (CERC-CVC)United States. Dept. of Energy (Award number DEPI0000012)National Science Foundation (U.S.) (Award number DMR-0819762)Robert Bosch GmbH (Bosch Energy Research Network (BERN) Grant)Skolkovo Institute of Science and Technology (Skoltech-MIT Center for Electochemical Energy Storage
Lithium peroxide crystal clusters as a natural growth feature of discharge products in LiāO2 cells
The often observed and still unexplained phenomenon of the growth of lithium peroxide crystal clusters during the discharge of LiāO2 cells is likely to happen because of self-assembling Li2O2 platelets that nucleate homogeneously right after the intermediate formation of superoxide ions by a single-electron oxygen reduction reaction (ORR). This feature limits the rechargeability of LiāO2 cells, but at the same time it can be beneficial for both capacity improvement and gain in recharge rate if a proper liquid phase mediator can be found
Mechanism of Oxygen Reduction in Aprotic LiāAir Batteries: The Role of Carbon Electrode Surface Structure
Electrochemical
oxygen reduction in aprotic media is a key process
that determines the operation of advanced metalāoxygen power
sources, e.g., LiāO<sub>2</sub> batteries. In such systems
oxygen reduction on carbon-based positive electrodes proceeds through
a complicated mechanism that comprises several chemical and electrochemical
steps involving either dissolved or adsorbed species, and as well
side reactions with carbon itself. Here, cyclic voltammetry was used
to reveal the effects of imperfections in the planar sp<sup>2</sup> surface structure of carbon on the Li oxygen reduction reaction
(Li-ORR) mechanism by means of different model carbon electrodes (highly
oriented pyrolytic graphite (HOPG), glassy carbon, basal, and edge
planes of pyrolytic graphite), in dimethyl sulfoxide (DMSO)-based
electrolyte. We show that the first electron transfer step O<sub>2</sub> + e<sup>ā</sup> ā O<sub>2</sub><sup>ā</sup> (followed by ion-coupling Li<sup>+</sup> + O<sub>2</sub><sup>ā</sup> ā LiO<sub>2</sub>) does not involve oxygen chemisorption
on carbon as evidenced by the independence of its rate on the carbon
electrode surface morphology. The second electron transfer leading
to Li<sub>2</sub>O<sub>2</sub> (Li<sup>+</sup> + LiO<sub>2</sub> +
e<sup>ā</sup> ā Li<sub>2</sub>O<sub>2</sub>) is strongly
affected by the electrode surface even in highly solvating DMSO. Formation
of Li<sub>2</sub>O<sub>2</sub> via the electrochemical reaction could
be observed only on the nearly ideal basal plane of graphite. In contrast,
for more disordered electrode surfaces, (and/or bulk) the only reduction
peak revealed on cyclic voltammograms corresponds to LiO<sub>2</sub> formation, supporting that solution-mediated mechanism for Li<sub>2</sub>O<sub>2</sub> growth is more favorable in that case. We also
show that increased defect concentrations on the carbon electrode
surface promote the formation of Li<sub>2</sub>CO<sub>3</sub> during
ORR, albeit relatively slower than Li<sub>2</sub>O<sub>2</sub> formation
Controlling Solution-Mediated Reaction Mechanisms of Oxygen Reduction Using Potential and Solvent for Aprotic LithiumāOxygen Batteries
Fundamental understanding of growth
mechanisms of Li<sub>2</sub>O<sub>2</sub> in LiāO<sub>2</sub> cells is critical for implementing
batteries with high gravimetric energies. Li<sub>2</sub>O<sub>2</sub> growth can occur first by 1e<sup>ā</sup> transfer to O<sub>2</sub>, forming Li<sup>+</sup>āO<sub>2</sub><sup>ā</sup> and then either chemical disproportionation of Li<sup>+</sup>āO<sub>2</sub><sup>ā</sup>, or a second electron transfer to Li<sup>+</sup>āO<sub>2</sub><sup>ā</sup>. We demonstrate that
Li<sub>2</sub>O<sub>2</sub> growth is governed primarily by disproportionation
of Li<sup>+</sup>āO<sub>2</sub><sup>ā</sup> at low overpotential,
and surface-mediated electron transfer at high overpotential. We obtain
evidence supporting this trend using the rotating ring disk electrode
(RRDE) technique, which shows that the fraction of oxygen reduction
reaction charge attributable to soluble Li<sup>+</sup>āO<sub>2</sub><sup>ā</sup>-based intermediates increases as the discharge
overpotential reduces. Electrochemical quartz crystal microbalance
(EQCM) measurements of oxygen reduction support this picture, and
show that the dependence of the reaction mechanism on the applied
potential explains the difference in Li<sub>2</sub>O<sub>2</sub> morphologies
observed at different discharge overpotentials: formation of large
(ā¼250 nmā1 Ī¼m) toroids, and conformal coatings
(<50 nm) at higher overpotentials. These results highlight that
RRDE and EQCM can be used as complementary tools to gain new insights
into the role of soluble and solid reaction intermediates in the growth
of reaction products in metalāO<sub>2</sub> batteries
Modified carbon nanotubes for water-based cathode slurries for lithiumāsulfur batteries
Notable reactivity of acetonitrile towards Li2O2/LiO2 probed by NAP XPS during LiāO2 battery discharge
One of the key factors responsible for the poor cycleability of LiāO2 batteries is a formation of byproducts from irreversible reactions between electrolyte and discharge product Li2O2 and/or intermediate LiO2. Among many solvents that are used as electrolyte component for LiāO2 batteries, acetonitrile (MeCN) is believed to be relatively stable towards oxidation. Using near ambient pressure X-ray photoemission spectroscopy (NAP XPS), we characterized the reactivity of MeCN in the LiāO2 battery. For this purpose, we designed the model electrochemical cell assembled with solid electrolyte. We discharged it first in O2 and then exposed to MeCN vapor. Further, the discharge was carried out in O2ā+āMeCN mixture. We have demonstrated that being in contact with LiāO2 discharge products, MeCN oxidizes. This yields species that are weakly bonded to the surface and can be easily desorbed. Thatās why they cannot be detected by the conventional XPS. Our results suggest that the respective chemical process most probably does not give rise to electrode passivation but can decrease considerably the Coulombic efficiency of the battery.This work of A.K-G., J.J.V-V. and D.M.I. was supported by the Russian Ministry of Science and Education (RFMEFI61614Ć0007) and Bundesministerium fĆ¼r Bildung and Forschung (Project No. 05K2014) in the framework of the joint Russian-German research project āSYnchrotron and NEutron STudies for Energy Storage (SYNESTESia)ā. T.K.Z acknowledges Center for Electrochemical Energy of Skolkovo Institute of Science and Technology for financial support. The work of O.O.K., A.I.B and L.V.Y. is performed within the joint project of the Russian Science Foundation (16-42-01093) and DFG (LA655-17/1). We are grateful to HZB for beamtime granted at ISISS and RGBL beamlines. T.K.Z. and A.S.F. thank to the Russian German laboratory at HZB for support provided. Authors are appreciated to Victor Vizgalov for solid electrolyte membrane preparation. Travelling of T.K.Z. was supported by German-Russian Interdisciplinary Science Center (G-RISC).Peer reviewe
Cover Feature: Extended Limits of Reversible Electrochemical Lithiation of Crystalline V 2
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