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  • 11
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    Evaluating the Thermodynamics of Electrochemical Ammonia Oxidation for Hydrogen Production
    The Electrochemical Society ; 2014
    In:  ECS Meeting Abstracts Vol. MA2014-01, No. 14 ( 2014-04-01), p. 655-655
    Details
    In: ECS Meeting Abstracts, The Electrochemical Society, Vol. MA2014-01, No. 14 ( 2014-04-01), p. 655-655
    Abstract: Objective Electrolysis of ammonia on platinum electrodes is a viable technology for wastewater remediation and hydrogen production[1]. Ammonia is oxidized at the anode, in the presence of hydroxide ions, and water is reduced at the cathode. The only products generated are nitrogen and hydrogen. While the anodic reaction is limited by slow kinetics and catalyst deactivation[2], improvements have been made using bimetallic catalysts[3,4] , especially at low concentrations of ammonia. This improved activity by empirical observation indicated a need for more fundamental analysis through a surface chemistry approach to the electrochemical reaction. This analysis will aid in designing improved catalysts and catalytic compositions. The use of density functional theory for characterizing chemical reactions, especially at the catalyst surface, has yielded valuable insight into the thermodynamics and kinetics of the reactions[5] and this method will be applied for this study. Methodology Density Functional Theory as applied in Gaussian 09[6] was used to generate the electronic and thermodynamic properties of the reactants, products and intermediates of ammonia electro-oxidation. Unrestricted spin calculations (due to unpaired electrons) were performed using the hybrid B3LYP functional[7] while the basis sets used were LANL2DZ[8-11] for platinum atoms and 6-311++G** for nitrogen, oxygen, and hydrogen atoms[12,13] . Using the computational hydrogen electrode[14], the effect of an applied potential was evaluated. Results The aforementioned species present during ammonia electro-oxidation are of the form: NH x (x = 0 – 3), OH y (y = 1 & 2) and N 2 H z (z = 0 – 4) when ammonia electrolysis occurs on platinum below the potential for oxide formation. The adsorption of these species has been previously investigated and characterized using the method above[15,16]. The following trend for adsorption was predicted: N 2 〈 H 2 O 〈 NH 3 〈 N 2 H 2 〈 N 2 H 4 〈 N 2 H 〈 N 2 H 3 〈 OH 〈 NH 2 〈 NH 〈 N . However, these calculations have not accounted for the effect of an applied potential, pH or the solvent environment. Using the method of Norskov et al. ,[14] the effect of these pertubations, which are essential to electrochemical reactions, have been investigated. These results will be presented at the meeting. References [1] F. Vitse, M. Cooper, and G. G. Botte, Journal of Power Sources 142, 18 (2005). [2] H. Gerischer and A. Mauerer, Journal of Electroanalytical Chemistry 25, 421 (1970). [3] E. P. Bonnin, E. J. Biddinger, and G. G. Botte, Journal of Power Sources 182(2008). [4] B. K. Boggs and G. G. Botte, Electrochimica Acta 55(2010). [5] J. Norskov, T. Bligaard, J. Rossmeisl, and C. Christensen, Nature Chemistry 1, 37 (2009). [6] M. J. Frisch et al., Gaussian 09, Revision B.01, Gaussian, Inc., 2009. [7] A. D. Becke, Journal of Chemical Physics 98, 5648 (1993). [8] T. H. Dunning, Journal of Chemical Physics 90, 1007 (1989). [9] P. J. Hay and W. R. Wadt, Journal of Chemical Physics 82, 299 (1985). [10] P. J. Hay and W. R. Wadt, Journal of Chemical Physics 82, 270 (1985). [11] W. R. Wadt and P. J. Hay, Journal of Chemical Physics 82, 284 (1985). [12] G. S. Chandler and A. D. McLean, Journal of Chemical Physics 71, 2175 (1979). [13] A. D. McLean and G. S. Chandler, Journal of Chemical Physics 72, 5639 (1980). [14] J. Norskov, J. Rossmeisl, A. Logadottir, L. Lindqvist, J. Kitchin, T. Bligaard, and H. Jonsson, Journal of Physical Chemistry B 108, 17886 (2004). [15] D. A. Daramola and G. G. Botte, Computational and Theoretical Chemistry 989, 7 (2012). [16] D. A. Daramola and G. G. Botte, Journal of Colloid and Interface Science 402, 204 (2013).
    Type of Medium: Online Resource
    ISSN: 2151-2043
    URL: Article
    DOI: 10.1149/MA2014-01/14/655
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    Publisher: The Electrochemical Society
    Publication Date: 2014
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  • 12
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    Instrument for Measuring Local Ionic Conductivity of Porous Electrodes
    The Electrochemical Society ; 2019
    In:  ECS Meeting Abstracts Vol. MA2019-02, No. 5 ( 2019-09-01), p. 255-255
    Details
    In: ECS Meeting Abstracts, The Electrochemical Society, Vol. MA2019-02, No. 5 ( 2019-09-01), p. 255-255
    Abstract: Due to the nature of how porous battery electrodes are fabricated, their microstructure is not uniform. For instance, there are variations in composition, effective electronic transport, and effective ionic transport. Such heterogeneity has been associated with several battery application issues. For example, variability in transport of ions can lead to a tendency for localized plating of lithium on anodes during fast charging [1-2]. Studying the heterogeneity of electrodes is a growing research topic. Our research group has previously developed a micro-four-line probe that successfully measured the variation of electronic conductivity of electrodes [3]. Another method to study the microstructure of electrodes is by means of SEM and X-ray tomography, and the variation of tortuosity (effective ionic resistance) in electrodes was computed by analyzing the tomographic data of microstructure [4] . We report here on a new technique to measure the local ionic resistance on a sub-mm length scale. A probe was made to detect the local transport of ions through a small aperture. The probe is scanned across the surface of a porous thin-film electrode in order to create maps of tortuosity or MacMullin number. The measurement was performed using electrochemical impedance spectroscopy, and an associated model is needed to invert the experimental results. [1] Harris et al., The Journal of Physical Chemistry C 117, 6481 (2013). [2] Vogel et al., Electrochimica Acta 297, 820 (2019). [3] Lanterman et al., Journal of the Electrochemical Society 162, A2145 (2015). [4] Kehrwald et al. Journal of The Electrochemical Society 158, A1393 (2011). Figure 1
    Type of Medium: Online Resource
    ISSN: 2151-2043
    URL: Article
    DOI: 10.1149/MA2019-02/5/255
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    Publisher: The Electrochemical Society
    Publication Date: 2019
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  • 13
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    Theoretical Investigations of Electrochemical CO 2 Reduction
    The Electrochemical Society ; 2017
    In:  ECS Meeting Abstracts Vol. MA2017-02, No. 45 ( 2017-09-01), p. 2008-2008
    Details
    In: ECS Meeting Abstracts, The Electrochemical Society, Vol. MA2017-02, No. 45 ( 2017-09-01), p. 2008-2008
    Abstract: The electrochemical reduction of CO 2 has the potential to store energy from intermittent renewable sources and to produce carbon-neutral fuels and chemicals[1]. In recent years, theoretical studies of CO 2 reduction have usually applied the computational hydrogen electrode model, which allows for the determination of the energies of reaction intermediates without explicitly treating the potential and the ions in solution[2]. This thermochemical approach has been shown to correlate well with experimental onset potentials [3, 4] and applied to computational screening of new catalysts [5, 6]. However, an understanding of charge transfer barriers, kinetics, selectivity, and pH effects all require explicit consideration of solvent and charge. In this talk, I will discuss new developments in the explicit treatment of the electrochemical interface, which is based on a simple capacitor model that uses the interfacial charge to obtain barriers at constant potential [7, 8] . I will then discuss the application of such a scheme to CO 2 reduction: the determination of reaction pathways on transition metals field and solvation effects[9, 10], the resultant kinetics, and the implications for catalyst design. 1. Whipple, D.T. and P.J.A. Kenis, Prospects of CO2 Utilization via Direct Heterogeneous Electrochemical Reduction. The Journal of Physical Chemistry Letters, 2010. 1 (24): p. 3451-3458. 2. Nørskov, J.K., et al., Origin of the Overpotential for Oxygen Reduction at a Fuel-Cell Cathode. J. Phys. Chem. B, 2004. 108 (46): p. 17886--17892. 3. Shi, C., et al., Chan, K., Yoo, J., Nørskov, J.K.  Trends in electrochemical CO2 reduction activity for open and close-packed metal surfaces. Physical Chemistry Chemical Physics, 2014. 16 (10): p. 4720-4727. 4. Kuhl, K.P., et al., Electrocatalytic Conversion of Carbon Dioxide to Methane and Methanol on Transition Metal Surfaces. Journal of the American Chemical Society, 2014. 5. Chan, K., et al., Molybdenum Sulfides and Selenides as Possible Electrocatalysts for CO2 Reduction. ChemCatChem, 2014. 6 (7): p. 1899-1905. 6. Asadi, M., et al., Robust carbon dioxide reduction on molybdenum disulphide edges. Nature communications, 2014. 5 . 7. Chan, K. and J.K. Nørskov, Electrochemical Barriers Made Simple. J. Phys. Chem. Lett., 2015: p. 2663--2668. 8. Chan, K. and J.K. Nørskov, Potential Dependence of Electrochemical Barriers from ab Initio Calculations. The Journal of Physical Chemistry Letters, 2016: p. 1686-1690. 9. Montoya, J.H., et al., Theoretical Insights into a CO Dimerization Mechanism in CO2 Electroreduction. The journal of physical chemistry letters, 2015. 6 (11): p. 2032--2037. 10. Chen, L.D., Urushihara, M., Chan, K., Nørskov, J.K.  Electric Field Effects in Electrochemical CO2 Reduction. ACS Catalysis, 2016. 11. Liu, X., Xiao, J., Peng, H., Hong, X., Chan, K., Nørskov, J.K.  Understanding trends in CO2 reduction on transition metals.  Nature Communications, 2017.
    Type of Medium: Online Resource
    ISSN: 2151-2043
    URL: Article
    DOI: 10.1149/MA2017-02/45/2008
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    Publisher: The Electrochemical Society
    Publication Date: 2017
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  • 14
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    Single-Ion-Conducting Glass-Polymer Hybrid Electrolytes for Lithium Batteries
    The Electrochemical Society ; 2016
    In:  ECS Meeting Abstracts Vol. MA2016-01, No. 1 ( 2016-04-01), p. 127-127
    Details
    In: ECS Meeting Abstracts, The Electrochemical Society, Vol. MA2016-01, No. 1 ( 2016-04-01), p. 127-127
    Abstract: Electrolytes used in lithium-ion batteries that power personal electronic devices and electric vehicles comprise lithium salts dissolved in flammable organic liquids. Catastrophic battery failure often begins with the electrolyte decomposition and combustion. Mixtures of liquids and salts have additional limitations. The passage of current results in an accumulation of salt in the vicinity of one electrode and depletion close to the other electrode, because only the cation participates in the electrochemical reactions. These effects are minimized in the case of single-ion-conducting-solid electrolytes due to the absent of concentration polarization and the limited solubility and slow diffusion (1). Therefore, non-flammable single-ion-conducting solid electrolytes have the potential to dramatically improve safety and performance of lithium batteries (2,3). Solid electrolytes such as inorganic sulfide glasses (Li 2 S–P 2 S 5 ) are single-ion-conductors with high shear moduli (18-25 GPa) and high ionic conductivity (over 10 −4 S/cm) at room temperature (4,5). However, these materials, on their own, cannot serve as efficient electrolytes as they cannot adhere to moving boundaries of the active particles in the battery electrode as they are charged and discharged. In this study, we describe hybrid single-ion-conducting electrolytes based on inorganic sulfide glasses and perfluoropolyether polymers for lithium batteries. Herein, it is demonstrated that hybrid electrolytes provide a compelling alternative to the traditional glass, ceramic, or polymer battery electrolytes. These electrolytes present high transference numbers, unprecedented ionic conductivities at room temperature, excellent electrochemical stability, and limit the dissolution of lithium polysulfides. The results in this work represent a significant step toward addressing the challenges of enabling the next generation cathodes such as lithium nickel manganese cobalt oxide and sulfur. _______________________ [1] J.M. Tarascon, M. Armand, Nature , 414 ( 2001 ) 359-367. [2] R. Bouchet, et al., Nature Materials , 12 ( 2013 ) 452-457. [3] N. Kamaya, et al., Nature Materials , 10 ( 2011 ) 682-686. [4] Z. Liu, et al., Journal of the American Chemical Society , 135 ( 2013 ) 975-978. [5] A. Sakuda, A. Hayashi, Y. Takigawa, K. Higashi, M. Tatsumisago, Journal of the Ceramic Society of Japan , 121 ( 2013 ) 946-949.
    Type of Medium: Online Resource
    ISSN: 2151-2043
    URL: Article
    DOI: 10.1149/MA2016-01/1/127
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    Publisher: The Electrochemical Society
    Publication Date: 2016
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  • 15
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    Effects of Non-Uniform Temperature Distribution on Degradation of Lithium-Ion Cells
    The Electrochemical Society ; 2018
    In:  ECS Meeting Abstracts Vol. MA2018-01, No. 3 ( 2018-04-13), p. 364-364
    Details
    In: ECS Meeting Abstracts, The Electrochemical Society, Vol. MA2018-01, No. 3 ( 2018-04-13), p. 364-364
    Abstract: Lithium-ion cells degrade much faster at temperatures higher than 25 °C mainly due to accelerated solid-electrolyte interface (SEI) growth in anode and degeneration of cathode [1, 2]. It is also known that temperature distributions in lithium-ion cells are not uniform [3] due to very low thermal conductivity of battery materials. The non-uniform temperature distributions could cause non-uniform degradation, thus exacerbating the thermal degradation problem, especially for large-format lithium-ion cells during high power operation. The effects of non-uniform temperature distributions on degradation of lithium-ion cells will be investigated and progress will be presented. References [1] C.Y. Wang, G. Zhang, S. Ge, T. Xu, Y. Ji, X.G. Yang, Y. Leng. Lithium-ion battery structure that self-heats at low temperatures, Nature , 529(7587) (2016) 515-518. [2] T. Waldmann, M. Wilka, M. Kasper, M. Fleischhammer, M. Wohlfahrt-Mehrens. Temperature dependent ageing mechanisms in lithium-ion batteries – A post-mortem study, Journal of Power Sources, 262 (2014) 129-135. [3] G. Zhang, L. Cao, S. Ge, C.Y. Wang, C.E. Shaffer, C.D. Rahn. In situ measurement of radial temperature distributions in cylindrical Li-ion cells, Journal of The Electrochemical Society , 161(10) (2014) A1499-A1507.
    Type of Medium: Online Resource
    ISSN: 2151-2043
    URL: Article
    DOI: 10.1149/MA2018-01/3/364
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    Publisher: The Electrochemical Society
    Publication Date: 2018
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  • 16
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    Metal-Air Batteries
    The Electrochemical Society ; 2016
    In:  ECS Meeting Abstracts Vol. MA2016-03, No. 1 ( 2016-06-10), p. 18-18
    Details
    In: ECS Meeting Abstracts, The Electrochemical Society, Vol. MA2016-03, No. 1 ( 2016-06-10), p. 18-18
    Abstract: Li-ion and related battery technologies will be important for years to come. However, society needs energy storage that exceeds that of Li-ion batteries. We must explore alternatives to Li-ion if we are to have any hope of meeting the long-term needs for energy storage. One alternative is the Li-air (O 2 ) battery, Fig. 1; its theoretical specific energy exceeds that of Li-ion, but many hurdles face its realization. [1-5] One spin-off of the recent interest in rechargeable Li-O 2 batteries, based on aprotic electrolytes is that it has highlighted the importance of understanding the fundamental oxygen redox processes at the positive electrode within the battery. [6-15] As a result of these fundamental studies it is generally accepted that a solution growth mechanism for Li 2 O 2 will be required to achieve high rates and capacities, avoiding the formation of passivating Li 2 O 2 films on the electrode surface.  Recent results exploring the electrochemical mechanism of O 2 reduction to form Li 2 O 2 at the positive electrode have identified new strategies to achieve this by exploiting the effect of the electrolyte solution. Moving to a solution phase discharge mechanism highlights the requirement for charge mediation between the electroactive species and the electrode, thus using solid Li 2 O 2 simply as a storage material for lithium ions and electrons. The implications of this will be discussed REFERENCES [1]. Bruce, P. G.; Freunberger, S. A.; Hardwick, L. J.; Tarascon, J.-M. Nature Materials 2012 , 11 , 19. [2]. Lu, Y. C.; Gallant, B. M.; Kwabi, D. G.; Harding, J. R.; Mitchell, R. R.; Whittingham, M. S.; Shao-Horn, Y. Energy & Environmental Science 2013 , 6 , 750. [3]. Black, R.; Adams, B.; Nazar, L. F. Advanced Energy Materials 2012 , 2 , 801. [4]. Girishkumar, G.; McCloskey, B.; Luntz, A. C.; Swanson, S.; Wilcke, W. The Journal of Physical Chemistry Letters 2010 , 1 , 2193. [5]. Li, F.; Zhang, T.; Zhou, H. Energy & Environmental Science 2013 , 6 , 1125. [6]. Adams, B. D.; Radtke, C.; Black, R.; Trudeau, M. L.; Zaghib, K.; Nazar, L. F. Energy & Environmental Science 2013 , 6 , 1772. [7]. Horstmann, B.; Gallant, B.; Mitchell, R.; Bessler, W. G.; Shao-Horn, Y.; Bazant, M. Z. The Journal of Physical Chemistry Letters 2013 , 4 , 4217. [8]. Hummelshoj, J. S.; Luntz, A. C.; Norskov, J. K. The Journal of Chemical Physics 2013 , 138 , 034703. [9]. McCloskey, B. D.; Scheffler, R.; Speidel, A.; Girishkumar, G.; Luntz, A. C. The Journal of Physical Chemistry C 2012 , 116 , 23897. [10]. Mitchell, R. R.; Gallant, B. M.; Shao-Horn, Y.; Thompson, C. V. The Journal of Physical Chemistry Letters 2013 , 4 , 1060. [11]. Trahan, M. J.; Mukerjee, S.; Plichta, E. J.; Hendrickson, M. A.; Abraham, K. M. Journal of The Electrochemical Society 2013 , 160 , A259. [12]. Sharon, D.; Etacheri, V.; Garsuch, A.; Afri, M.; Frimer, A. A.; Aurbach, D. The Journal of Physical Chemistry Letters 2012 , 4 , 127. [13]. Jung, H. G.; Kim, H. S.; Park, J. B.; Oh, I. H.; Hassoun, J.; Yoon, C. S.; Scrosati, B.; Sun, Y. K. Nano Letters 2012 , 12 , 4333. [14]. Peng, Z.; Freunberger, S. A.; Hardwick, L. J.; Chen, Y.; Giordani, V.; Barde, F.; Novak, P.; Graham, D.; Tarascon, J. M.; Bruce, P. G. Angewandte Chemie International Edition 2011 , 50 , 6351. [15]. Zhai, D.; Wang, H. H.; Yang, J.; Lau, K. C.; Li, K.; Amine, K.; Curtiss, L. A. Journal of the American Chemical Society 2013 , 135 , 15364.
    Type of Medium: Online Resource
    ISSN: 2151-2043
    URL: Article
    DOI: 10.1149/MA2016-03/1/18
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    Publisher: The Electrochemical Society
    Publication Date: 2016
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  • 17
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    Electrochemical Growth and OER Catalytic Activityof Ultrathin Epitaxial Cobalt Oxide Films
    The Electrochemical Society ; 2020
    In:  ECS Meeting Abstracts Vol. MA2020-01, No. 19 ( 2020-05-01), p. 1187-1187
    Details
    In: ECS Meeting Abstracts, The Electrochemical Society, Vol. MA2020-01, No. 19 ( 2020-05-01), p. 1187-1187
    Abstract: Iron-group oxides are among the best earth abundant catalysts for the oxygen evolution reaction (OER) in alkaline and neutral electrolytes [ 1 ],[ 2 ]. Such oxides have been prepared with an amorphous or a crystalline structure, using thermal salt decomposition [ 3 ], autoclave synthesis [ 4 ], photochemical reactions [ 5 ], sol-gel synthesis [ 6 ], metal electrodeposition and subsequent oxidation, [ 7 ] and direct oxide electrodeposition [ 1 ], [ 8 ]. This work focuses on well-defined epitaxial CoOx [ 9 ] electrocatalysts grown by direct electrodeposition on Au(111) according to an approach similar to that introduced by Switzer [ 8 ]. The growth modes of catalysts and the mechanisms of deposition will be discussed based on electrochemical characterizations, XRD characterizations and microscopic observations. In particular to explain that CoOOH may be obtained at a potential of +1V/RHE by oxidation of a Co(II) complex diluted in an alkaline solution while thermodynamics predicts that Co 3 O 4 should be formed. The electrochemical properties in pre-OER and within OER will be discussed as a function of the surface structure and morphology of layers. In particular to show that the large pseudocapacitance measured at the electrode is not related to its ECSA but to electrical charging within the bulk of the electrode. [1] M. W. Kanan and D. G. Nocera, Science 321 , 1072 (2008). [2] C. C. L. McCrory, S. Jung, I. M. Ferrer et al., Journal of the American Chemical Society 137 , 4347 (2015). [3] C. Pirovano and S. Trasatti, Journal of Electroanalytical Chemistry and Interfacial Electrochemistry 180 , 171 (1984). [4] D. Yuming, H. Kun, Y. Lin et al., Nanotechnology 18 , 435602 (2007). [5] S. R. Alvarado, Y. Guo, T. P. A. Ruberu et al., The Journal of Physical Chemistry C 116 , 10382 (2012). [6] A. Bergmann, E. Martinez-Moreno, D. Teschner et al., Nature Communications 6 , 8625 (2015). [7] M. W. Louie and A. T. Bell, Journal of the American Chemical Society 135 , 12329 (2013). [8] J. A. Koza, Z. He, A. S. Miller et al., Chem. Mat. 24 , 3567 (2012). [9] F. Reikowski, F. Maroun, I. Pacheco et al., ACS Catalysis 9 , 3811 (2019).
    Type of Medium: Online Resource
    ISSN: 2151-2043
    URL: Article
    DOI: 10.1149/MA2020-01191187mtgabs
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    Publisher: The Electrochemical Society
    Publication Date: 2020
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  • 18
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    Single- and Few-Layers MoSe 2 Nanoflowers: Synthesis, Characterization, and Their Piezoresponse
    The Electrochemical Society ; 2016
    In:  ECS Meeting Abstracts Vol. MA2016-01, No. 25 ( 2016-04-01), p. 1288-1288
    Details
    In: ECS Meeting Abstracts, The Electrochemical Society, Vol. MA2016-01, No. 25 ( 2016-04-01), p. 1288-1288
    Abstract: We demonstrate a hydrothermal process at temperature of 180 o C to synthesize a single to few layers MoSe2 nanoflowers which exhibit a high surface-to-volume ratio and is stable under room temperature in ambient air. The crystal structure of the MoSe2 nanoflowers has been confirmed by X-ray diffraction pattern, Raman, and High-resolution transmission electron microscopy (HRTEM). On the basis of the scanning electron microscope (SEM) image, the size of the MoSe2 nanoflowers is in the range of the 300-500nm. HRTEM image reveals that the MoSe2 nanoflowers possess a great number of the single- and few-layers, which further confirms that our nanoflowers display the plentiful amount of active surface sites. In addition, the lattice fringes between each single layer is about 0.66 nm, which is slightly larger than the reported value of 0.62 nm for the MoSe 2 . The piezoresponse force microscopy image further shows that the MoSe2 nanoflowers exhibits significantly piezoelectric potential which is generated from the active surface sites of the petals in the MoSe2 nanoflowers. Reference[1-6] 1.         Duerloo, K.-A.N., M.T. Ong, and E.J. Reed, Intrinsic piezoelectricity in two-dimensional materials. The Journal of Physical Chemistry Letters, 2012. 3 (19): p. 2871-2876. 2.         Kaasbjerg, K., K.S. Thygesen, and A.-P. Jauho, Acoustic phonon limited mobility in two-dimensional semiconductors: Deformation potential and piezoelectric scattering in monolayer MoS 2 from first principles. Physical Review B, 2013. 87 (23): p. 235312. 3.         Alyörük, M.M., et al., Promising Piezoelectric Performance of Single Layer Transition-Metal Dichalcogenides and Dioxides. The Journal of Physical Chemistry C, 2015. 119 (40): p. 23231-23237. 4.         Qi, J., et al., Piezoelectric effect in chemical vapour deposition-grown atomic-monolayer triangular molybdenum disulfide piezotronics. Nature communications, 2015. 6 . 5.         Wu, T. and H. Zhang, Piezoelectricity in Two ‐ Dimensional Materials. Angewandte Chemie International Edition, 2015. 54 (15): p. 4432-4434. 6.     Chhowalla, M., et al., The chemistry of two-dimensional layered transition metal dichalcogenide nanosheets. Nature chemistry, 2013. 5 (4): p. 263-275.
    Type of Medium: Online Resource
    ISSN: 2151-2043
    URL: Article
    DOI: 10.1149/MA2016-01/25/1288
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    Publisher: The Electrochemical Society
    Publication Date: 2016
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  • 19
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    Status and Targets for Polymer-Based Solid-State Batteries for Electric Vehicle Applications
    The Electrochemical Society ; 2019
    In:  ECS Meeting Abstracts Vol. MA2019-02, No. 7 ( 2019-09-01), p. 648-648
    Details
    In: ECS Meeting Abstracts, The Electrochemical Society, Vol. MA2019-02, No. 7 ( 2019-09-01), p. 648-648
    Abstract: As the market of electric vehicles (EVs) expands, numerous researchers and companies are focusing on the use of lithium metal anodes, which can enable higher energy densities required to extend the driving range of EVs and allow for lower cost [1]. However, the implementation of these metal anode batteries has several safety issues that emerge from dendrite growth in flammable liquid electrolytes. Solid polymer electrolyte has been studied as one of the promising candidates for lithium metal batteries because of the advantages of the non-flammability and relatively higher mechanical properties than liquid electrolytes [2, 3] . Compared to existing batteries based on liquid electrolytes, solid polymer electrolytes still have limitations, such as low ionic conductivity under room temperature conditions, which can significantly hinder its application in EVs. Hence, research on next-generation solid polymer electrolyte is being conducted to improve its transport properties. In this work, by using a model-based approach, the status of the present-day solid polymer electrolyte battery is examined, and compared with the traditional batteries with liquid electrolyte, with a focus on EVs. Using a mathematical model developed based on the macro-homogeneous approach pioneered by Newman and coworkers [4], we investigated Li-metal/LiFePO 4 (LFP) batteries containing three different electrolytes, namely (i) liquid electrolyte (ii) polystyrene-b-poly(ethylene oxide) (SEO) block copolymer electrolyte and (iii) a single-ion conducting block copolymer electrolyte. Concentrated solution theory and modified Ohm’s law are used to calculate the mass transport and potential gradient inside the electrolyte. In addition, the mass balance of lithium, potential drop in the active material, and the charge-transfer reactions are considered for a composite positive electrode that consists of LFP active particles. More detailed information about the continuum model is available in the literatures [4, 5] . All the transport parameters for the solid polymers, which include SEO and single-ion block copolymer, are adopted from the previously-published experimental results [3, 6-8]. For validation, model predicted results of the three Li/LFP batteries are compared with experimental data. Next, we compared the performance of the three different electrolytes operating at the same specified electrode thickness and weight percent of electrolyte. Optimal design points of each cell that provides the highest specific energy and power are determined. Finally, the results demonstrate how the specific energy and power of a solid polymer cell should be improved to achieve similar performance as that of a liquid electrolyte cell. This work provides directions for improvements in present-day solid polymer electrolytes for usage in electric vehicle. References Gallagher, K.G., et al., Quantifying the promise of lithium-air batteries for electric vehicles. Energy & Environmental Science, 2014. 7 (5): p. 1555-1563. Armand, M. and J.M. Tarascon, Building better batteries. Nature, 2008. 451 (7179): p. 652-657. Bouchet, R., et al., Single-ion BAB triblock copolymers as highly efficient electrolytes for lithium-metal batteries. Nature Materials, 2013. 12 (5): p. 452-457. Doyle, M., T.F. Fuller, and J. Newman, Modeling of Galvanostatic Charge and Discharge of the Lithium Polymer Insertion Cell. Journal of the Electrochemical Society, 1993. 140 (6): p. 1526-1533. Fuller, T.F., M. Doyle, and J. Newman, Simulation and Optimization of the Dual Lithium Ion Insertion Cell. Journal of the Electrochemical Society, 1994. 141 (1): p. 1-10. Bruce, P.G., et al., Li-O-2 and Li-S batteries with high energy storage. Nature Materials, 2012. 11 (1): p. 19-29. Devaux, D., et al., Failure Mode of Lithium Metal Batteries with a Block Copolymer Electrolyte Analyzed by X-Ray Microtomography. Journal of the Electrochemical Society, 2015. 162 (7): p. A1301-A1309. Pesko, D.M., et al., Comparing Two Electrochemical Approaches for Measuring Transference Numbers in Concentrated Electrolytes. Journal of the Electrochemical Society, 2018. 165 (13): p. A3014-A3021.
    Type of Medium: Online Resource
    ISSN: 2151-2043
    URL: Article
    DOI: 10.1149/MA2019-02/7/648
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    Publisher: The Electrochemical Society
    Publication Date: 2019
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    Incorporation of Conductive Internal Additives within Electrocuring Adhesives
    The Electrochemical Society ; 2017
    In:  ECS Meeting Abstracts Vol. MA2017-01, No. 20 ( 2017-04-15), p. 1083-1083
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    In: ECS Meeting Abstracts, The Electrochemical Society, Vol. MA2017-01, No. 20 ( 2017-04-15), p. 1083-1083
    Abstract: Low-voltage activated adhesives have recently been invented, aka ‘voltaglue’, leading to electrochemically mediated adhesive curing (electrocuring)[1]. Consisting of new and established adhesive crosslinking groups, formulations incorporate dendrimers that have a preference of intermolecular crosslinking while allowing flexible incorporation of functional groups. Upon voltage activation, specific functional groups are activated and covalently bond to a variety of surfaces, but this is highly dependent on bulk conductivity. To tailor the adhesive properties and adhesion strength, internal additives have been explored towards increasing conductivity and ultimately the ‘voltaglue’ crosslinking efficiency. Flexible electrocuring is sought to achieve a range of material properties, from viscous gels to hard set matrices. Ferrocene, a well-known redox active compound with reversible one-electron redox behaviour[2], is often incorporated in polymers/dendrimers due to its reversible nature and conductive aspects [3] . By integrating the ferrocene internal additive into dendrimer formulations combined with the electrically activated crosslinking additives we are able to mediate the electrocuring properties to a limited degree. In this work we present the synthesis of PAMAM-g-ferrocene-g-diazirine, an electrocuring adhesive that is able to adhere to a range of substrates, with adhesive strengths at the kPa scale. Real time electrorheology measurements chemistry evaluate the range of material properties available and demonstrate the synergistic performance ferrocene internal additives impart on the ‘voltaglue’ adhesives.     References   [1] J. Ping, F. Gao, J.L. Chen, R.D. Webster, T.W.J. Steele, Adhesive curing through low-voltage activation, Nature Communications 6 (2015). [2] M.E. N.P.R.A. Silva, A.J.L. Pombeiro, J.J.R. Fraústo da Silva, R. Herrmann, N. Deus, R. E.Bozak, Redox potential and substituent effects in ferrocene derivatives: II, Journal of Organometallic Chemistry 480 (1994). [3] R. Gracia, D. Mecerreyes, Polymers with redox properties: materials for batteries, biosensors and more, Polymer Chemistry 4 (2013). [4] C.M. Elson, M.T.H. Liu, C. Mailer, Electron-spin-resonance studies of diazirine anion radicals, Journal of the Chemical Society, Chemical Communications 7 (1986).
    Type of Medium: Online Resource
    ISSN: 2151-2043
    URL: Article
    DOI: 10.1149/MA2017-01/20/1083
    Language: Unknown
    Publisher: The Electrochemical Society
    Publication Date: 2017
    detail.hit.zdb_id: 2438749-6
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