Thin Film Micro-Batteries by Nancy J

Total Page:16

File Type:pdf, Size:1020Kb

Thin Film Micro-Batteries by Nancy J Thin Film Micro-Batteries by Nancy J. Dudney tags, and smarter cards. In principle Most of the thin films used in current Building a Battery by with a large deposition system, a thin commercial variations of this thin Vapor Deposition film battery might cover a square meter, film battery are deposited in vacuum but in practice, most development is chambers by RF and DC magnetron hin film batteries are built layer targeting individual cells with active sputtering and by thermal evaporation by layer by vapor deposition. areas less than 25 cm2. For very small onto unheated substrates. In addition, The resulting battery is formed battery areas, <1 mm2, microfabrication many publications report exploring a T 2 of parallel plates, much as an ordinary processes have been developed. variety of other physical and chemical battery construction, just much thinner. Typically the assembled batteries have vapor deposition processes, such as pulsed The figure (Fig. 1) shows an example of a capacities from 0.1 to 5 mAh. laser deposition, electron cyclotron thin film battery layout where films are The operation of a thin film battery resonance sputtering, and aerosol spray deposited symmetrically onto both sides is depicted in the schematic diagram coating, for one or more components of of a supporting substrate. The full stack (Fig. 2). Very simply, when the battery is the battery. The active materials used of films is only 10 to 15 µm thick, but allowed to discharge, a Li+ ion migrates for the thin film cathodes and anodes including the support at least doubles from the anode to the cathode film by are familiar intercalation compounds, the overall battery thickness. When diffusing through the solid electrolyte. but the microstructures and often the the support is thin, the entire battery When the anode and cathode reactions cycling properties of the thin films may can be flexible. At least six companies are reversible, as for an intercalation be quite distinct from those of battery have commercialized or are very close compound or alloy, the battery can electrodes formed from powders. The to commercializing such all-solid-state be recharged by reversing the current. thin film cathodes are dense and thin film batteries and market research1 The difference in the electrochemical homogeneous with no added phases predicts a growing market and a variety potential of the lithium determines the such as binders or electrolytes. When of applications including sensors, RFID cell voltage. deposited at ambient temperatures, the films of cathodes, such as LiCoO2, V2O5, LiMn2O4, LiFePO4 are amorphous or nanocrystalline. But even in this form, they often act as excellent cathodes with large specific capacities and good stability for hundreds to thousands of cycles.3 Annealing the cathode films at temperatures of 300° to 800°C may be used to induce crystallization and grain growth of the desired intercalation compound. Crystallizing the cathode film generally improves the Li chemical diffusivity in the electrode material, and hence the power delivered by the 10-15µm battery, by 1-2 orders of magnitude. The microstructure is also tailored by the deposition and heat treatment. Figure 3 shows a fracture edge of an annealed LiCoO2 cathode film on an alumina FIG. 1. Schematic cross section of a thin film battery fabricated by vapor substrate. The columnar microstructure, deposition onto both sides of a substrate support. which is typical of a vapor deposited film, sinters at high temperatures leaving small fissures between the dense columns. Such crystalline films also may have a preferred crystallographic orientation. For LiCoO2 films the crystallographic texture differs for films deposited by sputtering4 versus pulse laser ablation processes.5 To improve the manufacturability of the thin film batteries, it would be beneficial to eliminate or minimize the temperature or duration of the annealing step. Several efforts have lead to low temperature fabrication of thin film batteries on polyimide substrates, but the battery capacity and rate are lower than those treated at high temperatures.6,7 For the battery anode, many designs use a vapor-deposited metallic lithium film as both the anode and current collector. When used with a FIG. 2. Schematic illustration of a thin film battery. The arrows indicate the mechanically and chemically stable discharge reaction where a Li ion diffuses from the lithium metal anode to solid electrolyte, the lithium anodes fill a vacancy in an intercalation compound that serves as the cathode. The give excellent charge–discharge compensating electron is conducted through the device. 44 The Electrochemical Society Interface • Fall 2008 1 µm-thick films are adequate for a pinhole-free barrier over most thin film electrodes. Further, the electronic resistivity of Lipon is very high, greater than 1014 Ωcm. The ternary composition diagram (Fig 4) shows the composition range giving the highest lithium ion conductivity. The lithium content is slightly below that for the orthophosphate structure and spectroscopic studies indicate that much of the nitrogen substitutes for oxygen and forms links between two or three phosphate groups.14 The diagram also shows that the Lipon composition is well outside of the normal glass forming region. So far, synthesis of this material is limited to vapor deposition with an energetic FIG. 3. Schematic cross section of a thin film battery fabricated by vapor source of nitrogen. When deposited by deposition onto both sides of a substrate support. magnetron sputtering, film deposition rates can exceed 10 nm/m with good cycling at high rates, and long battery microstructure or boundaries. Al- results. Higher Lipon deposition rates life with no lithium dendrites. The chief though the nitrogen partial pressure are reported for alternative processes drawback for metallic lithium anodes over-whelms that of the oxygen in the such as plasma enhanced chemical is the restricted maximum operating plasma, only a small amount of N re- vapor deposition16 and nitrogen ion temperature to <180°C, which avoids places the oxygen in the composition, beam assisted deposition.17 melting of the lithium. Alternatives that but this nitrogen has a profound A variety of other inorganic and allow higher fabrication and operating effect on the ion conductivity and polymer electrolytes are being evaluated, temperatures include a Li-ion battery electrochemical stability. With a but none have been as widely tested anode or a “Li-free” construction. For N/O ratio as small as 0.1, the ionic as the Lipon electrolyte in thin film lithium-free batteries, the metallic conductivity is 1 to 2 µS/cm, which is rechargeable batteries. Inorganic glasses lithium anode is omitted during the about 40-fold higher than glassy films include binary and ternary mixes of fabrication, but is subsequently plated of N-free Li3PO4. More importantly, lithium borate, phosphate, silicate, and at the anode current collector when the the ionic transport number of Lipon is vanadate, but most compositions do not battery is charged for the first time.8 one, the electrochemical window is en- appear to meet conductivity or stability Lithium-ion anodes that have been hanced to 5.5V versus Li/Li+, and Lipon standards. Glass-ceramics with higher proposed include single-phase and is stable at both elevated temperatures ionic conductivities18 might be attractive composite films based on reversible and in contact with metallic lithium.15 as a self supporting electrolyte if reactions of lithium with Sn, Si, Ge, The lithium ion conductivity, although fabricated as <100 µm sheets. Promising and C. For the pure metals, only very 100X less than for many liquid polymer electrolytes are based on block thin films, ~50 nm, can tolerate the electrolytes, is sufficient because just copolymer compositions.19 extreme volume changes associated with insertion and extraction of large amounts of lithium.9,10 Good cycling has been reported for various oxide, nitride and oxynitrides of Si, Sn, and Zn3,11 which likely form composite films upon cycling. Intercalation 12 compounds, such as Li4Ti5O12, might also be used for thin film lithium-ion batteries. Lipon, a Glassy Electrolyte The thin film solid electrolyte invented at Oak Ridge National Laboratory in the early 1990s is the most widely used solid electrolyte for thin film batteries. The key insight by J. B. Bates was that addition of nitrogen to the glass structure might enhance the chemical and thermal stability of a lithium glass, as it does for sodium phosphate and sodium silicate glasses. The lithium phosphorus oxynitride electrolyte, which is now known as Lipon, is deposited by RF magnetron FIG. 4. Expanded region the LiO0.5-PO2.5-PN1.67 composition diagram (mole percentages) showing results of thin electrolyte films obtained by magnetron sputtering from a ceramic target of sputtering. The orange shaded areas indicates the compositions giving increasing Li3PO4 using a nitrogen process gas ionic conductivities exceeding 0.5, 1.0, and 2.0 µS/cm. Dashed lines indicate 13,14 to form the plasma. The films are constant ratios of (N+O)/P. The blue shading indicates the approximate amorphous and free of any columnar compositions for glasses formed from a melt. The Electrochemical Society Interface • Fall 2008 45 Dudney (continued from previous page) Cycle Life, Self Discharge, and Temperature Performance Thin film batteries with several different cathode and anode materials have been cycled to hundreds and many thousands of deep cycles with little loss of capacity. This is attributed to: the stability of the Lipon electrolyte film, the ability of the thin film materials to accommodate the volume changes associated with the charge-discharge reactions, and the uniformity of the current and charge distribution in the thin film structure. With cycling, the batteries gradually become more resistive with aging rates that depend FIG. 5. Ragone plot for thin film lithium batteries comparing the energy and on the particular electrode materials, power delivered by constant current discharge.
Recommended publications
  • Electrolyte Panel
    Lab Dept: Chemistry Test Name: ELECTROLYTE PANEL General Information Lab Order Codes: LYTE Synonyms: Electrolytes; Lytes CPT Codes: 80051 – Electrolyte panel Test Includes: Carbon Dioxide, Chloride, Potassium, Sodium concentrations reported in mEq/L, and AGAP (Anion Gap). Logistics Test Indications: The maintenance of osmotic pressure and water distribution in the various body fluid compartments is primarily a function of the four major electrolytes, Na+, K+, Cl-, and HCO3-. In addition to water homeostasis, these electrolytes play an important part in the maintenance of pH, regulation of proper heart and muscle functions, involvement in electron transfer reactions, and participation in catalysis as cofactors for enzymes. Lab Testing Sections: Chemistry Phone Numbers: MIN Lab: 612-813-6280 STP Lab: 651-220-6550 Test Availability: Daily, 24 hours Turnaround Time: 30 minutes Special Instructions: N/A Specimen Specimen Type: Blood Container: Green top (Li Heparin) tube, preferred Alternate tube: Red, marble or gold top tube Draw Volume: 0.6 mL blood Processed Volume: 0.2 mL serum/plasma Collection: Routine blood collection. Mix tubes containing anticoagulant by gentle inversion. Note: Venipuncture samples are preferred, but capillary specimens will be accepted. Special Processing: Lab Staff: Sample must be run within one hour of collection for CO2 stability. Centrifuge specimen, remove serum/plasma aliquot into a plastic sample cup. Avoid prolonged contact with separated cells. Store at refrigerated temperatures. Patient Preparation: None Sample Rejection: Mislabeled or unlabeled specimens Interpretive Reference Range: See individual analyte procedures Critical Values: See individual analyte procedures Limitations: See individual analyte procedures Methodology: See individual analyte procedures References: See individual analyte procedures Updates: 2/8/2016: Update alt tube types .
    [Show full text]
  • 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.
    [Show full text]
  • All-Carbon Electrodes for Flexible Solar Cells
    applied sciences Article All-Carbon Electrodes for Flexible Solar Cells Zexia Zhang 1,2,3 ID , Ruitao Lv 1,2,*, Yi Jia 4, Xin Gan 1,5 ID , Hongwei Zhu 1,2 and Feiyu Kang 1,5,* 1 State Key Laboratory of New Ceramics and Fine Processing, School of Materials Science and Engineering, Tsinghua University, Beijing 100084, China; [email protected] (Z.Z.); [email protected] (X.G.); [email protected] (H.Z.) 2 Key Laboratory of Advanced Materials (MOE), School of Materials Science and Engineering, Tsinghua University, Beijing 100084, China 3 School of Physics and Electronic Engineering, Xinjiang Normal University, Urumqi 830046, Xinjiang Province, China 4 Qian Xuesen Laboratory of Space Technology, China Academy of Space Technology, Beijing 100094, China; [email protected] 5 Graduate School at Shenzhen, Tsinghua University, Shenzhen 518055, Guangdong Province, China * Correspondences: [email protected] (R.L.); [email protected] (F.K.) Received: 16 December 2017; Accepted: 20 January 2018; Published: 23 January 2018 Abstract: Transparent electrodes based on carbon nanomaterials have recently emerged as new alternatives to indium tin oxide (ITO) or noble metal in organic photovoltaics (OPVs) due to their attractive advantages, such as long-term stability, environmental friendliness, high conductivity, and low cost. However, it is still a challenge to apply all-carbon electrodes in OPVs. Here, we report our efforts to develop all-carbon electrodes in organic solar cells fabricated with different carbon-based materials, including carbon nanotubes (CNTs) and graphene films synthesized by chemical vapor deposition (CVD). Flexible and semitransparent solar cells with all-carbon electrodes are successfully fabricated.
    [Show full text]
  • A Review of Cathode and Anode Materials for Lithium-Ion Batteries
    A Review of Cathode and Anode Materials for Lithium-Ion Batteries Yemeserach Mekonnen Aditya Sundararajan Arif I. Sarwat IEEE Student Member IEEE Student Member IEEE Member Department of Electrical & Department of Electrical & Department of Electrical & Computer Engineering Computer Engineering Computer Engineering Florida International University Florida International University Florida International University Email: [email protected] Email: [email protected] Email: [email protected] Abstract—Lithium ion batteries are one of the most technologies such as plug-in HEVs. For greater application use, commercially sought after energy storages today. Their batteries are usually expensive and heavy. Li-ion and Li- based application widely spans from Electric Vehicle (EV) to portable batteries show promising advantages in creating smaller, devices. Their lightness and high energy density makes them lighter and cheaper battery storage for such high-end commercially viable. More research is being conducted to better applications [18]. As a result, these batteries are widely used in select the materials for the anode and cathode parts of Lithium (Li) ion cell. This paper presents a comprehensive review of the common consumer electronics and account for higher sale existing and potential developments in the materials used for the worldwide [2]. Lithium, as the most electropositive element making of the best cathodes, anodes and electrolytes for the Li- and the lightest metal, is a unique element for the design of ion batteries such that maximum efficiency can be tapped. higher density energy storage systems. The discovery of Observed challenges in selecting the right set of materials is also different inorganic compounds that react with alkali metals in a described in detail.
    [Show full text]
  • 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 .
    [Show full text]
  • Demonstrating Solar Conversion Using Natural Dye Sensitizers
    Demonstrating Solar Conversion Using Natural Dye Sensitizers Subject Area(s) Science & Technology, Physical Science, Environmental Science, Physics, Biology, and Chemistry Associated Unit Renewable Energy Lesson Title Dye Sensitized Solar Cell (DSSC) Grade Level (11th-12th) Time Required 3 hours / 3 day lab Summary Students will analyze the use of solar energy, explore future trends in solar, and demonstrate electron transfer by constructing a dye-sensitized solar cell using vegetable and fruit products. Students will analyze how energy is measured and test power output from their solar cells. Engineering Connection and Tennessee Careers An important aspect of building solar technology is the study of the type of materials that conduct electricity and understanding the reason why they conduct electricity. Within the TN-SCORE program Chemical Engineers, Biologist, Physicist, and Chemists are working together to provide innovative ways for sustainable improvements in solar energy technologies. The lab for this lesson is designed so that students apply their scientific discoveries in solar design. Students will explore how designing efficient and cost effective solar panels and fuel cells will respond to the social, political, and economic needs of society today. Teachers can use the Metropolitan Policy Program Guide “Sizing The Clean Economy: State of Tennessee” for information on Clean Economy Job Growth, TN Clean Economy Profile, and Clean Economy Employers. www.brookings.edu/metro/clean_economy.aspx Keywords Photosynthesis, power, electricity, renewable energy, solar cells, photovoltaic (PV), chlorophyll, dye sensitized solar cells (DSSC) Page 1 of 10 Next Generation Science Standards HS.ESS-Climate Change and Human Sustainability HS.PS-Chemical Reactions, Energy, Forces and Energy, and Nuclear Processes HS.ETS-Engineering Design HS.ETS-ETSS- Links Among Engineering, Technology, Science, and Society Pre-Requisite Knowledge Vocabulary: Catalyst- A substance that increases the rate of reaction without being consumed in the reaction.
    [Show full text]
  • Solid Electrolyte Batteries
    SOLID ELECTROLYTE BATTERIES John B. Goodenough and Yuhao Lu Texas Materials Institute The University of Texas at Austin Project ID: ES060 DOE Vehicle Technologies Annual Merit Review Meeting May 9-13, 2011 This presentation does not contain any proprietary or confidential information. 1 The University of Texas at Austin Overview Timeline Barriers • Project Start Date-Oct. 2009 • Lithium-ion solid electrolyte. • Project End Date- Sept. 2010 • Choice of redox couples. • Percent complete: 100% complete • Flow-through- cathode cell design Budget Partners • Funding received in FY09-FY10 – $315K • Karim Zaghib of Hydro Quebec • Funding received in FY10-FY11 – $315K 2 The University of Texas at Austin Milestones Develop and test a suitable test cell. (Jan. 10) Completed Optimize components of the cell. (Apr. 10) Completed Develop a lithium/Fe(NO3)3 cell. (July. 10) Completed Design of a new cell (Sept. 10) Completed Test flow-through cell (Jan. 11) Completed 3 The University of Texas at Austin Typical Lithium Ion Battery (LIB) Cell e- e- - Separator + Li+ Anode Li+ Cathode (Reducing Agent) (Oxidizing Agent) Li+ SEI layer Electrolyte Capacity limited by Li solid solution in cathode and loss in SEI layer Voltage limited by Eg of carbonate electrolyte. 4 The University of Texas at Austin Why Oxides? E E Co: 4s0 Co: 4s0 Co(II): t4e2 µLi 4.0 eV Co(IV): t5e0 EFC EFC (pinned) Co(III): t6e0 Co(III): t6e0 O: 2p6 O: 2p6 N(E) N(E) Li CoO (0<x<0.55) LiCoO2 1-x 2 2- + Holes form peroxide (O2) for x> 0.55 or H inserted from electrolyte.
    [Show full text]
  • 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.
    [Show full text]
  • Operation, Manufacturing, and Supply Chain of Lithium-Ion Batteries for Electric Vehicles
    ORNL/TM-2020/1729 Operation, Manufacturing, and Supply Chain of Lithium-ion Batteries for Electric Vehicles Ilias Belharouak Jagjit Nanda Ethan Self W. Blake Hawley David Wood Zhijia Du Jianlin Li Approved for public release. Ronald L. Graves Distribution is unlimited. August 2020 DOCUMENT AVAILABILITY Reports produced after January 1, 1996, are generally available free via US Department of Energy (DOE) SciTech Connect. Website www.osti.gov Reports produced before January 1, 1996, may be purchased by members of the public from the following source: National Technical Information Service 5285 Port Royal Road Springfield, VA 22161 Telephone 703-605-6000 (1-800-553-6847) TDD 703-487-4639 Fax 703-605-6900 E-mail [email protected] Website http://classic.ntis.gov/ Reports are available to DOE employees, DOE contractors, Energy Technology Data Exchange representatives, and International Nuclear Information System representatives from the following source: Office of Scientific and Technical Information PO Box 62 Oak Ridge, TN 37831 Telephone 865-576-8401 Fax 865-576-5728 E-mail [email protected] Website http://www.osti.gov/contact.html This report was prepared as an account of work sponsored by an agency of the United States Government. Neither the United States Government nor any agency thereof, nor any of their employees, makes any warranty, express or implied, or assumes any legal liability or responsibility for the accuracy, completeness, or usefulness of any information, apparatus, product, or process disclosed, or represents that its use would not infringe privately owned rights. Reference herein to any specific commercial product, process, or service by trade name, trademark, manufacturer, or otherwise, does not necessarily constitute or imply its endorsement, recommendation, or favoring by the United States Government or any agency thereof.
    [Show full text]
  • 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.
    [Show full text]
  • 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,
    [Show full text]
  • Effect of Stratification of Cathode Catalyst Layers on Durability of Proton Exchange Membrane Fuel Cells
    energies Article Effect of Stratification of Cathode Catalyst Layers on Durability of Proton Exchange Membrane Fuel Cells Zikhona Nondudule 1, Jessica Chamier 2,* and Mahabubur Chowdhury 1 1 Department of Chemical Engineering, Faculty of Engineering, Cape Peninsula University of Technology, Cape Town 7530, South Africa; [email protected] (Z.N.); [email protected] (M.C.) 2 Department of Chemical Engineering, Centre for Catalysis Research, HySA Catalysis, University of Cape Town, Cape Town 7700, South Africa * Correspondence: [email protected]; Tel.: +27-(0)-21-650-2515 Abstract: To decrease the cost of fuel cell manufacturing, the amount of platinum (Pt) in the catalyst layer needs to be reduced. In this study, ionomer gradient membrane electrode assemblies (MEAs) were designed to reduce Pt loading without sacrificing performance and lifetime. A two-layer stratification of the cathode was achieved with varying ratios of 28 wt. % ionomer in the inner layer, on the membrane, and 24 wt. % on the outer layer, coated onto the inner layer. To study the MEA performance, the electrochemical surface area (ECSA), polarization curves, and electrochemical impedance spectroscopy (EIS) responses were evaluated under 20, 60, and 100% relative humidity (RH). The stratified MEA Pt loading was reduced by 12% while maintaining commercial equivalent performance. The optimal two-layer design was achieved when the Pt loading ratio between the layers was 1:6 (inner:outer layer). This MEA showed the highest ECSA and performance at 0.65 V with reduced mass transport losses. The integrity of stratified MEAs with lower Pt loading was evaluated with potential cycling and proved more durable than the monolayer MEA equivalent.
    [Show full text]