Iron-Based Flow Batteries: Improving Lifetime and Performance
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In-Situ Tools Used in Vanadium Redox Flow Battery Research—Review
batteries Review In-Situ Tools Used in Vanadium Redox Flow Battery Research—Review Purna C. Ghimire 1,*, Arjun Bhattarai 1,*, Tuti M. Lim 2, Nyunt Wai 3 , Maria Skyllas-Kazacos 4 and Qingyu Yan 5,* 1 V-flow Tech Pte Ltd., Singapore, 1 Cleantech Loop, Singapore 637141, Singapore 2 School of Civil and Environmental Engineering, Nanyang Technological University, 50 Nanyang Avenue, Singapore 639798, Singapore; [email protected] 3 Energy Research Institute @Nanyang Technological University, 1 Cleantech Loop, Singapore 637141, Singapore; [email protected] 4 School of Chemical Engineering, The University of New South Wales, Sydney 2052, Australia; [email protected] 5 School of Material Science and Engineering, Nanyang Technological University, Singapore 637141, Singapore * Correspondence: purna.ghimire@vflowtech.com (P.C.G.); arjun.bhattarai@vflowtech.com (A.B.); [email protected] (Q.Y.); Tel.: +65-85153215 (P.C.G.) Abstract: Progress in renewable energy production has directed interest in advanced developments of energy storage systems. The all-vanadium redox flow battery (VRFB) is one of the attractive technologies for large scale energy storage due to its design versatility and scalability, longevity, good round-trip efficiencies, stable capacity and safety. Despite these advantages, the deployment of the vanadium battery has been limited due to vanadium and cell material costs, as well as supply issues. Improving stack power density can lower the cost per kW power output and therefore, intensive research and development is currently ongoing to improve cell performance by increasing electrode activity, reducing cell resistance, improving membrane selectivity and ionic conductivity, etc. In order Citation: Ghimire, P.C.; Bhattarai, A.; to evaluate the cell performance arising from this intensive R&D, numerous physical, electrochemical Lim, T.M.; Wai, N.; Skyllas-Kazacos, and chemical techniques are employed, which are mostly carried out ex situ, particularly on cell M.; Yan, Q. -
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: -
Characterization of Battery for Energy Storage Applications – Lead Acid
Abstract #1672, 224th ECS Meeting, © 2013 The Electrochemical Society Characterization of battery for energy storage applications curves of a lead acid battery (YUASA, NP4-6). It has a – lead acid battery, lithium battery, vanadium redox normal voltage of 6 V and capacity of 4 Ah. The battery flow battery, and capacitor power was drained at 0.5 A till the cell voltage down to 3.0 V. The E-I curve was recorded by linear scanning Chih-Lung Hsieh1, Yen-Ting Liu2, Kan-Lin Hsueh2, amperometry at scanning rate of 0.01 A/s. The battery is Ju-Shei Hung3 then charge at 0.5 A for 2 hours. The SOC was assumed reached 25%. The E-I curve was then recorded. This 1. Institute of Nuclear Energy Research, Taoyuan, Taiwan procedure was carried out for SOC at 50%, 75%, and 2. Dept. Energy Eng., National United University, Miaoli, 100%. When cell voltage reached 7.0 V during charge Taiwan was considered as 100% SOC. Curves shown on Fig. 2 3. Dept. Chem. Eng., National United University, Miaoli, was measured result of laed acid battery. These curves Taiwan can be described by following equations. Where the IR accounts for internal resistance. Last term of equation [1] is the voltage cahge due to acitvation over-potential. The purpose of this study is to measure the charge/discharge characteristics of four different During Charge components for energy storage application. They are lead RT nF E E 1 iRI o ln o exp[ )]( [1] acid battery, lithium battery, vanadium redox flow battery, nF SO 2 H 4 RT [ 4 [] ] and capacitor. -
On the Electrochemical Stability of Nanocrystalline La0.9Ba0.1F2.9 Against Metal Electrodes
nanomaterials Article Fluoride-Ion Batteries: On the Electrochemical Stability of Nanocrystalline La0.9Ba0.1F2.9 against Metal Electrodes Maria Gombotz 1,* , Veronika Pregartner 1, Ilie Hanzu 1,2,* and H. Martin R. Wilkening 1,2 1 Institute for Chemistry and Technology of Materials, Technical Universtiy of Graz, Graz 8010, Austria; [email protected] (V.P.); [email protected] (H.M.R.W.) 2 ALISTORE—European Research Institute, CNRS FR3104, Hub de l’Energie, Rue Baudelocque, 80039 Amiens, France * Correspondence: [email protected] (M.G.); [email protected] (I.H.) Received: 27 September 2019; Accepted: 23 October 2019; Published: 25 October 2019 Abstract: Over the past years, ceramic fluorine ion conductors with high ionic conductivity have stepped into the limelight of materials research, as they may act as solid-state electrolytes in fluorine-ion batteries (FIBs). A factor of utmost importance, which has been left aside so far, is the electrochemical stability of these conductors with respect to both the voltage window and the active materials used. The compatibility with different current collector materials is important as well. In the course of this study, tysonite-type La0.9Ba0.1F2.9, which is one of the most important electrolyte in first-generation FIBs, was chosen as model substance to study its electrochemical stability against a series of metal electrodes viz. Pt, Au, Ni, Cu and Ag. To test anodic or cathodic degradation processes we carried out cyclic voltammetry (CV) measurements using a two-electrode set-up. We covered a voltage window ranging from −1 to 4 V, which is typical for FIBs, and investigated the change of the response of the CVs as a function of scan rate (2 mV/s to 0.1 V/s). -
Current State and Future Prospects for Electrochemical Energy Storage and Conversion Systems
energies Review Current State and Future Prospects for Electrochemical Energy Storage and Conversion Systems Qaisar Abbas 1 , Mojtaba Mirzaeian 2,3,*, Michael R.C. Hunt 1, Peter Hall 2 and Rizwan Raza 4 1 Centre for Materials Physics, Department of Physics, Durham University, Durham DH1 3LE, UK; [email protected] (Q.A.); [email protected] (M.R.H.) 2 School of Computing, Engineering and Physical Sciences, University of the West of Scotland, Paisley PA1 2BE, UK; [email protected] 3 Faculty of Chemistry and Chemical Technology, Al-Farabi Kazakh National University, Al-Farabi Avenue, 71, Almaty 050040, Kazakhstan 4 Clean Energy Research Lab (CERL), Department of Physics, COMSATS University Islamabad, Lahore 54000, Pakistan; [email protected] * Correspondence: [email protected] Received: 30 September 2020; Accepted: 26 October 2020; Published: 9 November 2020 Abstract: Electrochemical energy storage and conversion systems such as electrochemical capacitors, batteries and fuel cells are considered as the most important technologies proposing environmentally friendly and sustainable solutions to address rapidly growing global energy demands and environmental concerns. Their commercial applications individually or in combination of two or more devices are based on their distinguishing properties e.g., energy/power densities, cyclability and efficiencies. In this review article, we have discussed some of the major electrochemical energy storage and conversion systems and encapsulated their technological advancement in recent years. Fundamental working principles and material compositions of various components such as electrodes and electrolytes have also been discussed. Furthermore, future challenges and perspectives for the applications of these technologies are discussed. -
Recent Progress in Vanadium Redox-Flow Battery Katsuji Emura1 Sumitomo Electric Industries, Ltd., Osaka, Japan
Recent Progress in Vanadium Redox-Flow Battery Katsuji Emura1 Sumitomo Electric Industries, Ltd., Osaka, Japan 1. Introduction Vanadium Redox Flow Battery (VRB) is an energy storage system that employs a rechargeable vanadium fuel cell technology. Since 1985, Sumitomo Electric Industries Ltd (SEI) has developed VRB technologies for large-scale energy storage in collaboration with Kansai Electric power Co. In 2001, SEI has developed 3MW VRB system and delivered it to a large liquid crystal display manufacturing plant. The VRB system provides 3MW of power for 1.5 seconds as UPS (Uninterruptible Power Supply) for voltage sag compensation and 1.5MW of power for 1hr as a peak shaver to reduce peak load. The VRB system has successfully compensated for 50 voltage sag events that have occurred since installation up until September 2003. 2. Principle of VRB The unique chemistry of vanadium allows it to be used in both the positive and negative electrolytes. Figure 1 shows a schematic configuration of VRB system. The liquid electrolytes are circulated through the fuel cells in a similar manner to that of hydrogen and oxygen in a hydrogen fuel cell. Similarly, the electrochemical reactions occurring within the cells can produce a current flow in an external circuit, alternatively reversing the current flow results in recharging of the electrolytes. These cell reactions are balanced by a flow of protons or hydrogen ions across the cell through a selective membrane. The selective membrane also serves as a physical barrier keeping the positive and negative vanadium electrolytes separate. Figure 2 shows a cell stack which was manufactured by SEI. -
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 . -
Electrochemical Cells - Redox Reactions Can Be Used in a Controlled Manner to Make a Battery
Chapter 17 Worksheet #2 Name __________________________ Electrochemical Cells - Redox reactions can be used in a controlled manner to make a battery. A galvanic cell (voltaic cell or battery) converts the chemical energy of the reactants into electrical energy. BATTERY: Anode - AN OX, RED CAT Cathode - Salt Bridge - A tube containing a salt (such as KCl or NaNO3) solution that is used to connect two half-cells in an electrochemical cell; allows the passage of ions (maintains charge neutrality), but prevents the mixing of half-cell electrolytes. Shorthand notation for a galvanic cell: Zn(s)│Zn2+(aq)║Cu2+(aq)│Cu(s) where the anode is on the left, the cathode on the right, │ indicates the interface between the metal and solution, and ║ indicates the salt bridge. In many cells, the electrode itself does not react but serves only as a channel to direct electrons to or from the solution where a reaction involving other species takes place. The electrode itself is unaffected. Platinum and graphite are inert in most (but not all) electrochemical reactions. The Cu electrode could be replaced by a platinum or graphite electrode in the Zn/Cu battery: Zn(s)│Zn2+(aq)║Cu2+(aq)│Pt(s) Construct a battery from the reaction: Cr(s) + Pb2+(aq) Cr3+(aq) + Pb(s) Construct a galvanic cell using platinum electrodes and the reaction: - - + 2+ 10 Br (aq) + 2 MnO4 (aq) + 16 H (aq) 5 Br2(ℓ) + 2 Mn (aq) + 8 H2O(ℓ) A salt bridge is not required in a battery in which the reactants are physically separated from each other. -
Electrochemistry: Elektrolytic and Galvanic Cell Co08 Galvanic Series (Beketov, Cca 1860)
1/26 Electrochemistry: Elektrolytic and galvanic cell co08 Galvanic series (Beketov, cca 1860): Li, Ca, Al, Mn, Cr Zn, Cd Fe, Pb, [H2], Cu, Ag, Au ≈ ≈ ⊕ Cell = system composed of two electrodes and an electrolyte. electrolytic cell: electric energy chemical reaction ! galvanic cell: chemical reaction electric energy ! reversible galvanic cell (zero current) Electrodes anode = electrode where oxidation occurs Cu Cu2+ + 2 e ! − 2 Cl Cl2 + 2 e − ! − cathode = electrode where reduction occurs 2 Cu + + 2 e Cu credit: Wikipedia (free) − ! Cl2 + 2 e 2 Cl − ! − Oxidation and reduction are separated in a cell. The charge flows through the circuit. 2/26 Anode and cathode co08 electrolytic cell galvanic cell '$ '$ - - ⊕&% &% ⊕ Cl2 Cu2+ Cu2+ Pt Cl ! ! 2 Cu Cl Cl − Cu − CuCl2(aq) CuCl2(aq) anode cathode anode cathode “anions go to the anode” 3/26 Galvanic cells: electrodes, convention co08 Electrodes(= half-cells) may be separated by a porous separator, polymeric mem- brane, salt bridge. Cathode is right (reduction) ⊕ Anode is left (oxidation) negative electrode (anode) positive electrode (cathode) ⊕ liquid junction phase boundary . (porous separator) j salt bridge .. semipermeable membrane k Examples: 3 Cu(s) CuCl2(c = 0.1 mol dm ) Cl2(p = 95 kPa) Pt j − j j ⊕ Ag s AgCl s NaCl m 4 mol kg 1 Na(Hg) ( ) ( ) ( = − ) j j j 1 NaCl(m = 0.1 mol kg ) AgCl(s) Ag(s) j − j j ⊕ 2 3 4 3 3 3 Pt Sn +(0.1 mol dm ) + Sn +(0.01 mol dm ) Fe +(0.2 mol dm ) Fe j − − jj − j ⊕ 4/26 Equilibrium cell potential co08 Also: electromotive potential/voltage, electromo- tive force (EMF). -
Thin Films of Lithium Ion Conducting Garnets and Their Properties
Thin films of lithium ion conducting garnets and their properties dem Fachbereich Biologie und Chemie der Justus-Liebig-Universität Gießen vorgelegte Dissertation zur Erlangung des Grades Doktor der Naturwissenschaften – Dr. rer. nat. – von Jochen Reinacher geboren am 07.09.1984 Gießen 2014 II Dekan / Dean Prof. Dr. Holger Zorn 1. Gutachter / Reviewer Prof. Dr. Jürgen Janek 2. Gutachter / Reviewer Prof. Dr. Bruno K. Meyer Arbeit eingereicht: 10.06.2014 Tag der mündlichen Prüfung: 11.07.2014 III IV Abstract Different lithium ion conducting garnet-type thin films were prepared by pulsed laser deposition. Of these garnet-type thin films Li6BaLa2Ta2O12, cubic Li6.5La3Zr1.5Ta0.5O12 (additionally stabilized by Al2O3) and cubic Li7La3Zr2O12 stabilized by Ga2O3 were investigated in more detail. Conductivity measurements of these thin films performed in lateral geometry showed total conductivities of σ = 1.7∙10–6 S∙cm–1, σ = 2.9∙10–6 S∙cm–1 and σ = 1.2∙10–6 S∙cm–1, respectively. Electrochemical impedance spectroscopy was performed in axial geometry (orthogonal to the substrate), revealing conductivities of –5 –1 σ = 3.3∙10 S∙cm for Li6BaLa2Ta2O12 which is comparable to the bulk conductivity of –5 –1 Li6BaLa2Ta2O12 (σ = 4∙10 S∙cm ). The comparatively low lateral conductivity of the garnet-type material could be increased to a maximum of σ = 2.8∙10–5 S∙cm–1 for multilayer structures of two different alternating garnet-type materials (Li6.5La3Zr1.5Ta0.5O12:Al2O3, Li7La3Zr2O12:Ga2O3). These investigations revealed a strong influence of the thin film microstructure on the total conductivity. Additionally the electronic partial conductivity of Li6BaLa2Ta2O12 as bulk and thin film material was determined. -
Electrochemistry –An Oxidizing Agent Is a Species That Oxidizes Another Species; It Is Itself Reduced
Oxidation-Reduction Reactions Chapter 17 • Describing Oxidation-Reduction Reactions Electrochemistry –An oxidizing agent is a species that oxidizes another species; it is itself reduced. –A reducing agent is a species that reduces another species; it is itself oxidized. Loss of 2 e-1 oxidation reducing agent +2 +2 Fe( s) + Cu (aq) → Fe (aq) + Cu( s) oxidizing agent Gain of 2 e-1 reduction Skeleton Oxidation-Reduction Equations Electrochemistry ! Identify what species is being oxidized (this will be the “reducing agent”) ! Identify what species is being •The study of the interchange of reduced (this will be the “oxidizing agent”) chemical and electrical energy. ! What species result from the oxidation and reduction? ! Does the reaction occur in acidic or basic solution? 2+ - 3+ 2+ Fe (aq) + MnO4 (aq) 6 Fe (aq) + Mn (aq) Steps in Balancing Oxidation-Reduction Review of Terms Equations in Acidic solutions 1. Assign oxidation numbers to • oxidation-reduction (redox) each atom so that you know reaction: involves a transfer of what is oxidized and what is electrons from the reducing agent to reduced 2. Split the skeleton equation into the oxidizing agent. two half-reactions-one for the oxidation reaction (element • oxidation: loss of electrons increases in oxidation number) and one for the reduction (element decreases in oxidation • reduction: gain of electrons number) 2+ 3+ - 2+ Fe (aq) º Fe (aq) MnO4 (aq) º Mn (aq) 1 3. Complete and balance each half reaction Galvanic Cell a. Balance all atoms except O and H 2+ 3+ - 2+ (Voltaic Cell) Fe (aq) º Fe (aq) MnO4 (aq) º Mn (aq) b. -
Battery Technologies for Small Scale Embeded Generation
Battery Technologies for Small Scale Embedded Generation. by Norman Jackson, South African Energy Storage Association (SAESA) Content Provider – Wikipedia et al Small Scale Embedded Generation - SSEG • SSEG is very much a local South African term for Distributed Generation under 10 Mega Watt. Internationally they refer to: Distributed generation, also distributed energy, on-site generation (OSG) or district/decentralized energy It is electrical generation and storage performed by a variety of small, grid- connected devices referred to as distributed energy resources (DER) Types of Energy storage: • Fossil fuel storage • Thermal • Electrochemical • Mechanical • Brick storage heater • Compressed air energy storage • Cryogenic energy storage (Battery Energy • Fireless locomotive • Liquid nitrogen engine Storage System, • Flywheel energy storage • Eutectic system BESS) • Gravitational potential energy • Ice storage air conditioning • Hydraulic accumulator • Molten salt storage • Flow battery • Pumped-storage • Phase-change material • Rechargeable hydroelectricity • Seasonal thermal energy battery • Electrical, electromagnetic storage • Capacitor • Solar pond • UltraBattery • Supercapacitor • Steam accumulator • Superconducting magnetic • Thermal energy energy storage (SMES, also storage (general) superconducting storage coil) • Chemical • Biological • Biofuels • Glycogen • Hydrated salts • Starch • Hydrogen storage • Hydrogen peroxide • Power to gas • Vanadium pentoxide History of the battery This was a stack of copper and zinc Italian plates,