Advances in Materials Design for All-Solid-State Batteries: from Bulk to Thin Films
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A Solid-State and Flexible Supercapacitor That Operates Across a Wide Temperature Range
A Solid-State and Flexible Supercapacitor that Operates Across a Wide Temperature Range Ardalan Chaichi1,†, Gokul Venugopalan2,†, Ram Devireddy1, Christopher Arges2,*, Manas Ranjan Gartia1,* 1Department of Mechanical Engineering, Louisiana State University, Baton Rouge, USA 70803 2Cain Department of Chemical Engineering, Louisiana State University, Baton Rouge, USA 70803 † Equal contribution * Correspondence: [email protected]; [email protected] Abstract Electrochemical properties of most supercapacitor devices degrade quickly when the operating temperature deviates from room temperature. In order to exploit the potential of rGO in supercapacitors at extreme temperatures, a resilient electrolyte that is functional over a wide- temperature range is also required. In this study, we have implemented a flexible, low-resistant solid-state electrolyte membrane (SSEM) into symmetric rGO electrodes to realize supercapacitor devices that operate in the temperature range of -70 °C to 220 °C. The SSEM consists of a polycation-polybenzimidazole blend that is doped with phosphoric acid (H3PO4) and this material displays uniquely high conductivity values that range from 50 mS cm-1 to 278 mS cm-1 in the temperature range of -25 °C to 220 °C. The fabricated supercapacitor produced a maximum capacitance of 6.8 mF cm-2 at 100 °C. Energy and power densities ranged from 0.83 to 2.79 mW h cm-2 and 90 to 125 mW cm-2, respectively. The energy storage mechanism with a SSEM occurs by excess H3PO4 migrating from the membrane host into the electrochemical double layer in rGO electrodes. The high temperature operation is enabled by the polycation in the SSEM anchoring phosphate type of anions preventing H3PO4 evaporation. -
Electrochemical Cells
Electrochemical cells = electronic conductor If two different + surrounding electrolytes are used: electrolyte electrode compartment Galvanic cell: electrochemical cell in which electricity is produced as a result of a spontaneous reaction (e.g., batteries, fuel cells, electric fish!) Electrolytic cell: electrochemical cell in which a non-spontaneous reaction is driven by an external source of current Nils Walter: Chem 260 Reactions at electrodes: Half-reactions Redox reactions: Reactions in which electrons are transferred from one species to another +II -II 00+IV -II → E.g., CuS(s) + O2(g) Cu(s) + SO2(g) reduced oxidized Any redox reactions can be expressed as the difference between two reduction half-reactions in which e- are taken up Reduction of Cu2+: Cu2+(aq) + 2e- → Cu(s) Reduction of Zn2+: Zn2+(aq) + 2e- → Zn(s) Difference: Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(aq) - + - → 2+ More complex: MnO4 (aq) + 8H + 5e Mn (aq) + 4H2O(l) Half-reactions are only a formal way of writing a redox reaction Nils Walter: Chem 260 Carrying the concept further Reduction of Cu2+: Cu2+(aq) + 2e- → Cu(s) In general: redox couple Ox/Red, half-reaction Ox + νe- → Red Any reaction can be expressed in redox half-reactions: + - → 2 H (aq) + 2e H2(g, pf) + - → 2 H (aq) + 2e H2(g, pi) → Expansion of gas: H2(g, pi) H2(g, pf) AgCl(s) + e- → Ag(s) + Cl-(aq) Ag+(aq) + e- → Ag(s) Dissolution of a sparingly soluble salt: AgCl(s) → Ag+(aq) + Cl-(aq) − 1 1 Reaction quotients: Q = a − ≈ [Cl ] Q = ≈ Cl + a + [Ag ] Ag Nils Walter: Chem 260 Reactions at electrodes Galvanic cell: -
3 PRACTICAL APPLICATION BATTERIES and ELECTROLYSIS Dr
ELECTROCHEMISTRY – 3 PRACTICAL APPLICATION BATTERIES AND ELECTROLYSIS Dr. Sapna Gupta ELECTROCHEMICAL CELLS An electrochemical cell is a system consisting of electrodes that dip into an electrolyte and in which a chemical reaction either uses or generates an electric current. A voltaic or galvanic cell is an electrochemical cell in which a spontaneous reaction generates an electric current. An electrolytic cell is an electrochemical cell in which an electric current drives an otherwise nonspontaneous reaction. Dr. Sapna Gupta/Electrochemistry - Applications 2 GALVANIC CELLS • Galvanic cell - the experimental apparatus for generating electricity through the use of a spontaneous reaction • Electrodes • Anode (oxidation) • Cathode (reduction) • Half-cell - combination of container, electrode and solution • Salt bridge - conducting medium through which the cations and anions can move from one half-cell to the other. • Ion migration • Cations – migrate toward the cathode • Anions – migrate toward the anode • Cell potential (Ecell) – difference in electrical potential between the anode and cathode • Concentration dependent • Temperature dependent • Determined by nature of reactants Dr. Sapna Gupta/Electrochemistry - Applications 3 BATTERIES • A battery is a galvanic cell, or a series of cells connected that can be used to deliver a self-contained source of direct electric current. • Dry Cells and Alkaline Batteries • no fluid components • Zn container in contact with MnO2 and an electrolyte Dr. Sapna Gupta/Electrochemistry - Applications 4 ALKALINE CELL • Common watch batteries − − Anode: Zn(s) + 2OH (aq) Zn(OH)2(s) + 2e − − Cathode: 2MnO2(s) + H2O(l) + 2e Mn2O3(s) + 2OH (aq) This cell performs better under current drain and in cold weather. It isn’t truly “dry” but rather uses an aqueous paste. -
Elements of Electrochemistry
Page 1 of 8 Chem 201 Winter 2006 ELEM ENTS OF ELEC TROCHEMIS TRY I. Introduction A. A number of analytical techniques are based upon oxidation-reduction reactions. B. Examples of these techniques would include: 1. Determinations of Keq and oxidation-reduction midpoint potentials. 2. Determination of analytes by oxidation-reductions titrations. 3. Ion-specific electrodes (e.g., pH electrodes, etc.) 4. Gas-sensing probes. 5. Electrogravimetric analysis: oxidizing or reducing analytes to a known product and weighing the amount produced 6. Coulometric analysis: measuring the quantity of electrons required to reduce/oxidize an analyte II. Terminology A. Reduction: the gaining of electrons B. Oxidation: the loss of electrons C. Reducing agent (reductant): species that donates electrons to reduce another reagent. (The reducing agent get oxidized.) D. Oxidizing agent (oxidant): species that accepts electrons to oxidize another species. (The oxidizing agent gets reduced.) E. Oxidation-reduction reaction (redox reaction): a reaction in which electrons are transferred from one reactant to another. 1. For example, the reduction of cerium(IV) by iron(II): Ce4+ + Fe2+ ! Ce3+ + Fe3+ a. The reduction half-reaction is given by: Ce4+ + e- ! Ce3+ b. The oxidation half-reaction is given by: Fe2+ ! e- + Fe3+ 2. The half-reactions are the overall reaction broken down into oxidation and reduction steps. 3. Half-reactions cannot occur independently, but are used conceptually to simplify understanding and balancing the equations. III. Rules for Balancing Oxidation-Reduction Reactions A. Write out half-reaction "skeletons." Page 2 of 8 Chem 201 Winter 2006 + - B. Balance the half-reactions by adding H , OH or H2O as needed, maintaining electrical neutrality. -
Reaction Engineering of Polymer Electrolyte Membrane Fuel Cells
Reaction Engineering of Polymer Electrolyte Membrane Fuel Cells A new approach to elucidate the operation and control of Polymer Electrolyte Membrane (PEM) fuel cells is being developed. A global reactor engineering approach is applied to PEM fuel cells to identify the essential physics that govern the dynamics in PEM fuel cells. Reaction engineering principles are employed to develop a one-dimensional differential PEM fuel cell suitable for elucidating the dynamic performance of PEM cells under well-defined conditions. Polymer Electrolyte Fuel Cells Polymer electrolyte membrane (PEM) fuel cells employ a polymer membrane with acid side groups to conduct protons from the anode to cathode. Water management in the fuel cell is critical for PEM fuel cell operation. Sufficient water must be absorbed into the membrane to ionize the acid groups; excess water can flood the cathode of the fuel cell diminishing fuel cell performance limiting the power output. A schematic of a polymer electrolyte membrane hydrogen-oxygen fuel cell is shown in Figure 1. load e- Figure 1. Hydrogen-oxygen PEM fuel cell. Hydrogen molecules hydrogen in oxygen in dissociatively adsorb at the anode and are oxidized to protons. Electrons travel through an external load resistance. Protons diffuse H+ through the PEM under an e t electrochemical gradient to the y l ro t c cathode. Oxygen molecules adsorb e l at the cathode, are reduced and react hydrogen r E oxygen e m y + water out with the protons to produce water. + water out l Po The product water is absorbed into the PEM, or evaporates into the gas anode cathode streams at the anode and cathode. -
Galvanic Cell Notation • Half-Cell Notation • Types of Electrodes • Cell
Galvanic Cell Notation ¾Inactive (inert) electrodes – not involved in the electrode half-reaction (inert solid conductors; • Half-cell notation serve as a contact between the – Different phases are separated by vertical lines solution and the external el. circuit) 3+ 2+ – Species in the same phase are separated by Example: Pt electrode in Fe /Fe soln. commas Fe3+ + e- → Fe2+ (as reduction) • Types of electrodes Notation: Fe3+, Fe2+Pt(s) ¾Active electrodes – involved in the electrode ¾Electrodes involving metals and their half-reaction (most metal electrodes) slightly soluble salts Example: Zn2+/Zn metal electrode Example: Ag/AgCl electrode Zn(s) → Zn2+ + 2e- (as oxidation) AgCl(s) + e- → Ag(s) + Cl- (as reduction) Notation: Zn(s)Zn2+ Notation: Cl-AgCl(s)Ag(s) ¾Electrodes involving gases – a gas is bubbled Example: A combination of the Zn(s)Zn2+ and over an inert electrode Fe3+, Fe2+Pt(s) half-cells leads to: Example: H2 gas over Pt electrode + - H2(g) → 2H + 2e (as oxidation) + Notation: Pt(s)H2(g)H • Cell notation – The anode half-cell is written on the left of the cathode half-cell Zn(s) → Zn2+ + 2e- (anode, oxidation) + – The electrodes appear on the far left (anode) and Fe3+ + e- → Fe2+ (×2) (cathode, reduction) far right (cathode) of the notation Zn(s) + 2Fe3+ → Zn2+ + 2Fe2+ – Salt bridges are represented by double vertical lines ⇒ Zn(s)Zn2+ || Fe3+, Fe2+Pt(s) 1 + Example: A combination of the Pt(s)H2(g)H Example: Write the cell reaction and the cell and Cl-AgCl(s)Ag(s) half-cells leads to: notation for a cell consisting of a graphite cathode - 2+ Note: The immersed in an acidic solution of MnO4 and Mn 4+ reactants in the and a graphite anode immersed in a solution of Sn 2+ overall reaction are and Sn . -
Advancing Focused Ion Beam Characterization for Next Generation Lithium-Ion Batteries
UC San Diego UC San Diego Electronic Theses and Dissertations Title Advancing Focused Ion Beam Characterization for Next Generation Lithium-Ion Batteries Permalink https://escholarship.org/uc/item/3sh5k04b Author Lee, Jungwoo Publication Date 2018 Peer reviewed|Thesis/dissertation eScholarship.org Powered by the California Digital Library University of California UNIVERSITY OF CALIFORNIA SAN DIEGO Advancing Focused Ion Beam Characterization for Next Generation Lithium-Ion Batteries A dissertation submitted in partial satisfaction of the requirements for the degree Doctor of Philosophy in NanoEngineering by Jungwoo Zema Lee Committee in charge: Professor Ying Shirley Meng, Chair Professor David P. Fenning Professor Eric E. Fullerton Professor Olivia A. Graeve Professor Ping Liu 2018 Copyright Jungwoo Zema Lee, 2018 All rights reserved. The Dissertation of Jungwoo Zema Lee is approved, and it is acceptable in quality and form for publication on microfilm and electronically: Chair University of California San Diego 2018 iii DEDICATION To my given and chosen family iv TABLE OF CONTENTS Signature Page ..................................................................................................................... iii Dedication ............................................................................................................................ iv Table of Contents ................................................................................................................ v List of Abbreviations ......................................................................................................... -
Chapter 13: Electrochemical Cells
March 19, 2015 Chapter 13: Electrochemical Cells electrochemical cell: any device that converts chemical energy into electrical energy, or vice versa March 19, 2015 March 19, 2015 Voltaic Cell -any device that uses a redox reaction to transform chemical potential energy into electrical energy (moving electrons) -the oxidizing agent and reducing agent are separated -each is contained in a half cell There are two half cells in a voltaic cell Cathode Anode -contains the SOA -contains the SRA -reduction reaction -oxidation takes place takes place - (-) electrode -+ electrode -anions migrate -cations migrate towards the anode towards cathode March 19, 2015 Electrons move through an external circuit from the anode to cathode Electricity is produced by the cell until one of the reactants is used up Example: A simple voltaic cell March 19, 2015 When designing half cells it is important to note the following: -each half cell needs an electrolyte and a solid conductor -the electrode and electrolyte cannot react spontaneously with each other (sometimes carbon and platinum are used as inert electrodes) March 19, 2015 There are two kinds of porous boundaries 1. Salt Bridge 2. Porous Cup · an unglazed ceramic cup · tube filled with an inert · separates solutions but electrolyte such as NaNO allows ions to pass 3 through or Na2SO4 · the ends are plugged so the solutions are separated, but ions can pass through Porous boundaries allow for ions to move between two half cells so that charge can be equalized between two half cells 2+ 2– electrolyte: Cu (aq), SO4 (aq) 2+ 2– electrolyte: Zn (aq), SO4 (aq) electrode: zinc electrode: copper March 19, 2015 Example: Metal/Ion Voltaic Cell V Co(s) Zn(s) Co2+ SO 2- 4 2+ SO 2- Zn 4 Example: A voltaic cell with an inert electrode March 19, 2015 Example Label the cathode, anode, electron movement, ion movement, and write the half reactions taking place at each half cell. -
Development and Fabrication of a 1.5 F – 5 V Solid State Supercapacitor
Development and fabrication of a 1.5 F – 5 V solid state supercapacitor Pietro Staiti and Francesco Lufrano CNR-ITAE, ISTITUTO DI TECNOLOGIE AVANZATE PER L’ENERGIA “NICOLA GIORDANO” Via Salita S. Lucia sopra Contesse n. 5 Messina, Italy Phone: 0039 090 624226 / fax: 0039 090 624247 E-mail: [email protected] Acknowledgments The authors acknowledge the Consiglio Nazionale delle Ricerche that has financially supported the research project for the development of this type of supercapacitor. Keywords Supercapacitor, energy storage, solid electrolyte, acidic electrolyte. Abstract A five cells supercapacitor prototype with special electrolyte is designed and fabricated at the Institute CNR-ITAE of Messina. It has a nominal capacitance of 1.5 F and a maximum voltage of 5 V. The electrodes of prototype are formed of high surface area carbon material and Nafion ionomer. Nafion is used as an electrolyte membrane separator between the electrodes of each single cell and as a binder/ion conductor in the electrodes. The fabricated prototype achieves specific capacitance of 114 F/g (referred to the weight of active carbon materials for single electrode), that is comparable to the specific capacitance previously obtained from a smaller scale single cell of same type of supercapacitor. A power density of 1.4 kW/l and a RC-time constant of 0.3 s have been calculated for the device. Introduction Electric double layer capacitors (EDLCs) or supercapacitors (SCs) are promising energy storage devices, which are being considered for applications such as electric vehicles, uninterruptible power systems, and computer memory protection. Their main characteristic is the excellent high-rate charging-discharging ability that makes these devices, referring to this specific aspect, more efficient than batteries and fuel cells. -
Fabrication and Testing of All-Solid-State Nanoscale Lithium Batteries Using Lipon for Electrolytes
E3S Web of Conferences 53, 01008 (2018) https://doi.org/10.1051/e3sconf/20185301008 ICAEER 2018 Fabrication and Testing of All-solid-state Nanoscale Lithium Batteries Using LiPON for Electrolytes Feihu Tan1, XiaoPing Liang1, Feng Wei1 and Jun Du2, * 1State Key Laboratory of Advanced Materials for Smart Sensing, General Research Institute for Nonferrous Metals, Beijing, China. 2General Research Institute for Nonferrous Metals, Beijing, China. Abstract. The amorphous LiPON thin film was obtained by using the crystalline Li3PO4 target and the RF magnetron sputtering method at a N2 working pressure of 1 Pa. and then the morphology and composition of LiPON thin films are analysed by SEM and EDS. SEM shows that the film was compact and smooth, while EDS shows that the content of N in LiPON thin film was about 17.47%. The electrochemical properties of Pt/LiPON/Pt were analysed by EIS, and the ionic conductivity of LiPON thin films was -7 3.8×10 S/cm. By using the hard mask in the magnetron sputtering process, the all-solid-state thin film battery with Si/Ti/Pt/LiCoO2/LiPON/Li4Ti5O12/Pt structure was prepared, and its electrical properties were studied. As for this thin film battery, the open circuit voltage was 1.9 V and the first discharge specific capacity was 34.7 μAh/cm2·μm at a current density of 5 μA/cm-2,indicating that is promising in all-solid- state thin film batteries. 1 Introduction conductivity, [13-15] the ionic conductivity of LiPON films prepared by magnetron sputtering is up to ~10-6 S/cm, Lithium ion battery is a common energy supply unit in therefore, LiPON films were prepared by magnetron the current equipment. -
Bipolar Nickel-Metal Hydride Battery Being Developed
Bipolar Nickel-Metal Hydride Battery Being Developed Electro Energy's bipolar nickel-metal hydride battery design layout-two parallel, 24-cell stacks. (Copyright Electro Energy; used with permission.) The NASA Lewis Research Center has contracted with Electro Energy, Inc., to develop a bipolar nickel-metal hydride battery design for energy storage on low-Earth-orbit satellites (NASA contract NAS3-27787). The objective of the bipolar nickel-metal hydride battery development program is to approach advanced battery development from a systems level while incorporating technology advances from the lightweight nickel electrode field, hydride development, and design developments from nickel-hydrogen systems. This will result in a low-volume, simplified, less-expensive battery system that is ideal for small spacecraft applications. The goals of the program are to develop a 1-kilowatt, 28-volt (V), bipolar nickel-metal hydride battery with a specific energy of 100 watt-hours per kilogram (W-hr/kg), an energy density of 250 W-hr/liter and a 5-year life in low Earth orbit at 40- percent depth-of-discharge. Electro Energy has teamed with Rhône-Poulenc, Eagle-Picher Industries, Inc., Rutgers University, and Design Automation Associates to provide a well-integrated battery design. Electro Energy is the prime contractor responsible for the overall management of the program, battery design and development, component development and testing, and cell and battery testing. Rhône-Poulenc is responsible for the metal hydride component development and improvement. Eagle-Picher is supporting component and hardware development, battery design, fabrication procedures, trade studies, and documentation. Rutgers is providing treated material for the nickel electrodes in the batteries as well as analytical support for new and cycled cell components. -
Thin-Film Lithium and Lithium-Ion Batteries
Solid State Ionics 135 (2000) 33±45 www.elsevier.com/locate/ssi Thin-®lm lithium and lithium-ion batteries J.B. Bates, N.J. Dudney* , B. Neudecker, A. Ueda, C.D. Evans Oak Ridge National Laboratory, P.O. Box 2008, Oak Ridge, TN 37831-6030, USA Abstract Research over the last decade at Oak Ridge National Laboratory has led to the development of solid-state thin-®lm lithium and lithium-ion batteries. The batteries, which are less than 15 mm thick, have important applications in a variety of consumer and medical products, and they are useful research tools in characterizing the properties of lithium intercalation compounds in thin-®lm form. The batteries consist of cathodes that are crystalline or nanocrystalline oxide-based lithium intercalation compounds such as LiCoO224 and LiMn O , and anodes of lithium metal, inorganic compounds such as silicon±tin oxynitrides, Sn34 N and Zn 32 N , or metal ®lms such as Cu in which the anode is formed by lithium plating on the initial charge. The electrolyte is a glassy lithium phosphorus oxynitride (`Lipon'). Cells with crystalline LiCoO2 cathodes can deliver up to 30% of their maximum capacity between 4.2 and 3 V at discharge currents of 10 mA/cm2 , and at more moderate discharge±charge rates, the capacity decreases by negligible amounts over thousands of cycles. Thin ®lms of crystalline lithium manganese oxide with the general composition Li11x Mn22y O4 exhibit on the initial charge signi®cant capacity at 5 V and, depending on the deposition process, at 4.6 V as well, as a consequence of the manganese de®ciency±lithium excess.