Demonstrating Solar Conversion Using Natural Dye Sensitizers
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A HISTORY of the SOLAR CELL, in PATENTS Karthik Kumar, Ph.D
A HISTORY OF THE SOLAR CELL, IN PATENTS Karthik Kumar, Ph.D., Finnegan, Henderson, Farabow, Garrett & Dunner, LLP 901 New York Avenue, N.W., Washington, D.C. 20001 [email protected] Member, Artificial Intelligence & Other Emerging Technologies Committee Intellectual Property Owners Association 1501 M St. N.W., Suite 1150, Washington, D.C. 20005 [email protected] Introduction Solar cell technology has seen exponential growth over the last two decades. It has evolved from serving small-scale niche applications to being considered a mainstream energy source. For example, worldwide solar photovoltaic capacity had grown to 512 Gigawatts by the end of 2018 (representing 27% growth from 2017)1. In 1956, solar panels cost roughly $300 per watt. By 1975, that figure had dropped to just over $100 a watt. Today, a solar panel can cost as little as $0.50 a watt. Several countries are edging towards double-digit contribution to their electricity needs from solar technology, a trend that by most accounts is forecast to continue into the foreseeable future. This exponential adoption has been made possible by 180 years of continuing technological innovation in this industry. Aided by patent protection, this centuries-long technological innovation has steadily improved solar energy conversion efficiency while lowering volume production costs. That history is also littered with the names of some of the foremost scientists and engineers to walk this earth. In this article, we review that history, as captured in the patents filed contemporaneously with the technological innovation. 1 Wiki-Solar, Utility-scale solar in 2018: Still growing thanks to Australia and other later entrants, https://wiki-solar.org/library/public/190314_Utility-scale_solar_in_2018.pdf (Mar. -
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. -
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. -
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. -
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 . -
Thin Film Cdte Photovoltaics and the U.S. Energy Transition in 2020
Thin Film CdTe Photovoltaics and the U.S. Energy Transition in 2020 QESST Engineering Research Center Arizona State University Massachusetts Institute of Technology Clark A. Miller, Ian Marius Peters, Shivam Zaveri TABLE OF CONTENTS Executive Summary .............................................................................................. 9 I - The Place of Solar Energy in a Low-Carbon Energy Transition ...................... 12 A - The Contribution of Photovoltaic Solar Energy to the Energy Transition .. 14 B - Transition Scenarios .................................................................................. 16 I.B.1 - Decarbonizing California ................................................................... 16 I.B.2 - 100% Renewables in Australia ......................................................... 17 II - PV Performance ............................................................................................. 20 A - Technology Roadmap ................................................................................. 21 II.A.1 - Efficiency ........................................................................................... 22 II.A.2 - Module Cost ...................................................................................... 27 II.A.3 - Levelized Cost of Energy (LCOE) ....................................................... 29 II.A.4 - Energy Payback Time ........................................................................ 32 B - Hot and Humid Climates ........................................................................... -
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. -
Fabrication Procedure of Dye-Sensitized Solar Cells
Fabrication procedure of dye-sensitized solar cells K.Takechi, R.Muszynski and P.V.Kamat Materials - ITO(Indium doped Tin Oxide) glass (2 x 2 cm, 2 slides for 1 cell) - Dye (Eosin Y, Eosin B, etc.) - Ethanol - TiO2 paste ¾ Suspend 3.5g of TiO2 nano-powder P25 in 15ml of ethanol. ¾ Sonicate it at least for 30 min. ¾ Add 0.5ml of titanium(IV) tetraisopropoxide into the suspension. ¾ Mix until the suspension is uniform. (D.S. Zhang, T. Yoshida, T. Oekermann, K. Furuta, H. Minoura, Adv. Functional Mater., 16, 1228(2006).) - Spacer ¾ Cut a plastic film (like as Parafilm or Scotch tape) having dimensions of 1.5 cm by 2 cm. ¾ Make a hole(s) on the film. 2 cm (Example) 1 cm 1.5 cm Hole 0.6 cm - Liquid electrolyte ¾ 0.5M lithium iodide and 0.05M iodine in acetonitrile. γ-Butyrolactone or 3-methoxypropionitrile is also recommended as a solvent to improve its volatility. - Binder clips (small, 2 pieces for 1 cell) Tools - Hot plate - Pipets - Tweezers - Spatulas - Scotch tape 1. Put Scotch tape on the conducting side of ITO glass. about 10 mm 2. Put TiO2 paste and flatten it with a razor blade on the same side of the ITO glass. 3. Put this electrode on top of a hot plate and heat it at approximately 150 °C for 10 min. 4. Prepare a dye solution. (Ex. 20mL of 1 mM eosin Y in ethanol) Eosin Y Eosin B Eosin B in ethanol (Mw=691.85) (Mw=624.06) 5. Dip the TiO2 electrode into the dye solution for 10 min. -
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. -
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. -
Review of the Development of Thermophotovoltaics
International Research Journal of Engineering and Technology (IRJET) e-ISSN: 2395-0056 Volume: 06 Issue: 04 | Apr 2019 www.irjet.net p-ISSN: 2395-0072 REVIEW OF THE DEVELOPMENT OF THERMOPHOTOVOLTAICS Surya Narrayanan Muthukumar1, Krishnar Raja2, Sagar Mahadik3, Ashwini Thokal4 1,2,3UG Student, Department of Chemical Engineering, Bharati Vidyapeeth College of Engineering, Kharghar, Navi Mumbai, Maharashtra India 4Assistant Professor, Department of Chemical Engineering, Bharati Vidyapeeth College of Engineering, Kharghar, Navi Mumbai, Maharashtra India ---------------------------------------------------------------------------***--------------------------------------------------------------------------- Abstract:- Thermophotovoltaic (TPV) systems have 2. PRINCIPLE slowly started gaining traction in the global sustainable energy generation realm. It was earlier believed to be a To understand the working principle of TPVs, let us break flawed method whose energy conversion efficiency was not down the term into three parts: Thermo (meaning Heat), high enough for commercial use. However, in recent times, Photo (meaning Light) and Voltaic (meaning Electricity research has picked up, addressing the need of increasing produced by chemical action). Thus, a Thermophotovoltaic the energy conversion efficiency while making it system uses light to heat up a thermal emitter, which in economically viable for commercial applications. This paper turn emits radiation (Infrared) on a photovoltaic (PV) will throw light on the various advancements in the field of diode to produce electricity. Conventional photovoltaics TPV systems and investigate the potential avenues where exploit only the visible band of solar rays for electricity TPVs may be used in the future. We will also be looking at generation. The visible band contains less than half the the history of development of TPVs so that we may be aware total radiation of solar energy. -
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,