ENERGY STORDE DEVICES
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The document discusses different types of batteries, including primary batteries that are not rechargeable and secondary batteries that are rechargeable. It provides examples of the lead acid battery, a secondary battery, and dry cells, a primary battery. It describes the basic components of cells, including electrodes, electrolyte, and separators. It also covers how batteries can be connected in series or parallel configurations and the chemical reactions that occur during charging and discharging of batteries. The document discusses new types of flexible paper batteries and applications of lithium batteries in wearable electronics and other innovative devices.
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This document discusses different types of batteries including primary batteries, secondary batteries, and fuel cells. It provides definitions and examples of each type. Primary batteries include lithium cells and Leclanche cells which produce electricity through a non-reversible chemical reaction and cannot be recharged. Secondary batteries like lead-acid and nickel-cadmium batteries allow for recharging through a reversible reaction. Fuel cells like hydrogen-oxygen continuously produce electricity through redox reactions as long as fuel and oxidant are supplied.
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This document discusses various battery technologies including primary and secondary cells. It provides details on dry cells, lead-acid batteries, nickel-cadmium batteries, and fuel cells. The key points are:
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Exide Industries Ltd is India's largest lead acid battery manufacturer. It produces lead acid storage batteries that convert chemical energy into electrical energy through reversible chemical reactions. There are two main types of batteries: primary batteries that directly convert chemical energy and are not rechargeable, and secondary batteries that must be charged with electrical energy before converting chemical energy and are rechargeable, such as lead acid batteries. The document then provides details on the components and chemical reactions that occur during the discharging and charging of lead acid batteries.
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This document discusses different types of batteries including primary batteries, secondary batteries, and fuel cells. It provides definitions and examples of each type. Primary batteries include lithium cells and Leclanche cells which produce electricity through a non-reversible chemical reaction and cannot be recharged. Secondary batteries like lead-acid and nickel-cadmium batteries allow for recharging through a reversible reaction. Fuel cells like hydrogen-oxygen continuously produce electricity through redox reactions as long as fuel and oxidant are supplied.
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This document discusses various battery technologies including primary and secondary cells. It provides details on dry cells, lead-acid batteries, nickel-cadmium batteries, and fuel cells. The key points are:
- Primary cells cannot be recharged while secondary cells can be recharged by passing current in the opposite direction.
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There are several main types of rechargeable batteries. Lead-acid batteries use lead and lead-oxide electrodes and sulfuric acid electrolyte; they are commonly used in cars. Nickel-cadmium batteries contain nickel-hydroxide and cadmium electrodes with potassium hydroxide electrolyte. Nickel-metal hydride batteries are similar but do not contain cadmium. Lithium-ion batteries have carbon anodes and metal oxide cathodes with an organic electrolyte, and are used in devices like laptops and phones. Rechargeable batteries can be restored to full charge through applying electrical energy to reverse the chemical reactions.
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2. Balancing redox reactions is important, and the document outlines the step-by-step process for balancing both acidic and basic redox reactions.
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A battery produces electricity through electrochemical reactions between its electrodes and electrolyte. In a galvanic cell, which is the basic unit of a battery, oxidation occurs at the anode while reduction occurs at the cathode. Common battery types include zinc-carbon batteries, which use zinc and manganese dioxide electrodes with an ammonium chloride electrolyte, and alkaline batteries, which use a potassium hydroxide electrolyte. Lithium-ion batteries are rechargeable and power many portable electronic devices. A battery functions by facilitating redox reactions through the movement of electrons from the anode to the cathode.
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- They contain two half-cells, each with a different metal electrode, separated by a salt bridge or semipermeable membrane to allow ion flow.
- During operation, electrons flow from the metal being oxidized at the anode through an external circuit to the metal being reduced at the cathode.
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A galvanic cell consists of two half-cells with different metal electrodes immersed in electrolyte solutions, connected by a salt bridge or porous membrane. Chemical reactions at the electrodes produce a spontaneous flow of electrons through an external circuit. For example, in a Daniell cell zinc undergoes oxidation and copper undergoes reduction. The overall cell reaction is Zn + Cu
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Conductors and Non-Conductors
Substances can be classified as conductors and non-conductors based on their ability to conduct electricity.
Conductors: Substances that allow electric current to flow through them are called conductors. For example, Plastic, Wood, etc.
Non-Conductors: Non-conductors are insulators that do not allow electricity to pass through them. For example, Copper, Iron, etc.
Types of Conductors
Conductors are divided into two groups: Metallic conductors and Electrolytes.
Metallic Conductors: These conductors conduct electricity by the movement of electrons without any chemical change during the process. This type of conduction happens in solids and in the molten state.
Electrolytes: They conduct electricity by the movement of the ions in the solutions. It is present in the aqueous solution.
Distinguish between Metallic and Electrolytic Conduction
Metallic Conduction Electrolytic Conduction
The movement of electrons causes the electric current The movement of ions causes the electric current
There is no chemical reaction Ions get ionised or reduced at the electrodes
There is no transfer of matter It involves the transfer of matter in the form of ions
Follows Ohm’s law Follows Ohm’s law
Resistance increases with an increase in temperature Resistance decreases with an increase in temperature
Faraday’s law is not followed Follows Faraday’s law
Electrolytes
(a) Substances whose aqueous solutions allow the conductance of electric current and are chemically decomposed are called electrolytes.
(b) The positively charged ions furnished by the electrolyte are called cations, while the negatively charged ions furnished by the electrolyte are called anions.
Types of Electrolytes
(a) Weak electrolytes: Electrolytes that are decomposable to a very small extent in their dilute solutions are called weak electrolytes. For example, organic acids, inorganic acids and bases etc.
(b) Strong electrolytes: Electrolytes that are highly decomposable in aqueous solution and conduct electricity frequently are called electrolytes. For example, mineral acid and salts of strong acid.
Electrode
For the electric current to pass through an electrolytic conductor, the two rods or plates called electrodes are always needed. These plates are connected to the terminals of the battery to form a cell. The electrode through which the electric current flows into the electrolytic solution is called the anode, also called the positive electrode, and anions are oxidised here.
An electrode through which the electric current flows out of the electrolytic solution is called the cathode, also called the negative electrode, and cations are reduced there.
Electrolysis
Electrolysis is the process of chemical deposition of the electrolyte by passing an electric current. Electrolysis takes place in an electrolytic cell. This cell will convert the electrical energy to chemical energy.
3rd Lecture on Electrochemistry | Chemistry Part I | 12th Std
This document summarizes key aspects of electrochemistry including:
1) An electrochemical cell consists of two electrodes immersed in an electrolyte that allows ionic conduction. Oxidation occurs at the anode and reduction at the cathode.
2) There are two types of cells - electrolytic cells use an external power source to drive nonspontaneous reactions, while galvanic/voltaic cells generate power from spontaneous reactions.
3) The electrolysis of molten NaCl produces chlorine gas at the anode and deposits metallic sodium at the cathode, while electrolysis of aqueous NaCl produces hydrogen and chlorine gas due to the lower standard potentials of sodium and chlorine ions compared to water.
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This document provides an overview of electrochemistry concepts including:
- Types of electrochemical processes including reversible and irreversible processes.
- Oxidation-reduction reactions and how they involve oxidation and reduction half-reactions.
- Galvanic/voltaic cells and how they generate electricity from spontaneous redox reactions.
- Components of electrochemical cells including electrodes, salt bridges, and how they allow indirect redox reactions.
- Standard electrode potentials and how they are used to determine if a reaction is spontaneous.
- The Nernst equation and how it describes the dependence of electrode potential on ion concentration.
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This document provides information on oxidation-reduction (redox) reactions and electrochemistry:
[1] Redox reactions involve the transfer of electrons between oxidizing and reducing agents. Common examples are corrosion reactions.
[2] Galvanic (voltaic) cells generate electricity through spontaneous redox reactions. The anode is where oxidation occurs and electrons are released. The cathode is where reduction occurs and electrons are gained.
[3] Cell potential depends on the relative tendencies of substances to be oxidized or reduced, as measured by standard reduction potentials. More negative potentials indicate greater reducing ability; more positive potentials indicate greater oxidizing ability.
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ENERGY STORDE DEVICES
- 1. Created by,
- 2. A Cell Or Connected Group Of Cells That Converts Chemical Energy Into Electrical Energy By Reversible Chemical Reactions And That May Be Recharged By Passing A Current Through It In The Direction Opposite To That Of Its Discharge – Called Also Storage Cell. THE BATTERY
- 4. TYPES OF BATTERIES The primary battery The secondary battery
- 5. The secondary battery must first be charged with electrical energy before it can convert chemical energy to electrical energy . It is rechargeable. Example-Lead Acid Battery The primary battery converts chemical energy to electrical energy directly, using the chemical materials within the cell to start the action. It is not rechargeable. Example-Dry Cell THE PRIMARY BATTERY THE SECONDARY BATTERY
- 6. Uses An electrolytic paste. The electrolytic paste reacts with the electrodes to produce a negative charge on one electrode and a positive charge on the other. The difference of potential between the two Electrodes is the output voltage. DRY CELL
- 7. A Hard plastic container. Positive and negative internal plates made of lead. Plate separators made of porous synthetic material. Electrolyte, a dilute solution of sulfuric acid and water, better known as battery acid. Lead terminals, the connection point between the battery and whatever it powers. LEAD ACID BATTERY
- 9. Series circuits, the total voltage is equal to the sum of the individual voltages. The current is constant. Parallel circuits, the voltage is constant. The current is equal to the sum of the individual currents OHM’S LAW R=V/I
- 10. SERIES CONNECTED BATTERIES a. Positive terminal of one cell is connected to the negative terminal of the next, is called a series connected battery. b. The voltage of this type of battery is the sum of a individual cell voltages.
- 11. PARALLEL CONNECTED BATTERIES o Connect the negative terminal from one cell to the negative of the next cell o Connect the positive terminal to the positive terminal, is parallel connected. o Voltage remains constant and the current is cumulative.
- 12. Negative plate reaction: PbSO4(s) + H+(aq) + 2-e → Pb(s) + HSO4(aq) Positive plate reaction: PbSO4(s) + 2H2O(l) → PbO2(s) + HSO4(aq) + 3H+(aq) + 2e The total reaction can be written: 2PbSO4(s) + 2H2O(l) → Pb(s) + PbO2(s) + 2H2SO4(aq) CHARGING
- 13. Negative plate reaction: Pb(s) + HSO4(aq) → PbSO4(s) + H+(aq) + 2-e Positive plate reaction: PbO2(s) + HSO4(aq) + 3H+(aq) + 2-e → PbSO4(s) + 2H2O(l) The total reaction can be written: Pb(s) + PbO2(s) + 2H2SO4(aq) → 2PbSO4(s) + 2H2O(l) DISCHARGING
- 14. • Clean Battery Terminals. • Attach clamps to the battery in proper polarity. • Keep open flames and sparks away from battery. • Ventilate the battery well while charging. CHARGING
- 15. WHY ADD ELECTRONICS TO BATTERIES? REQUIRED ELECTRONICS ON NEW CHEMISTRIES: Energy density has increased with each advancement in chemistry making cells less stable. Requiring: – Safety circuits – Cell balancing – Secondary safeties
- 16. Added Value Electronics: Wireless Power (charging) Using the Qi (inductive power standard),Epec can embed wireless charging electronics in your battery to work with off-the-shelf wireless charging Pads that already exist, or develop a custom pad for your product.
- 17. BUILD TO PRINT ELECTRONICS
- 18. PAPER BATTERY Battery takes large amount of space and consumes more weight. researchers show interest in Ultrathin, Flexible , safe energy storage device. Nano scale. INTRODUCTION
- 19. CARBON NANO TUBES A carbon Nanotube is a tube- shaped material, made of carbon, diameter measures on the nanometer scale also known as Bucky tubes. A nanometer is one billionth of the meter. Carbon Nanotubes have many structures, differing in length, thickness, and in the type of felicity and number of layers.
- 21. APPLICATION
- 22. PRINTABLE BATTERY Imprint Energy Founded in 2010 Develop zinc-based rechargeable battery technology
- 23. Bendable Electronics LG and Samsung Flexible phones and watches CUSTOMER SELECTION
- 24. CUSTOMER SELECTION Bioelectronics MC10 Medical patch Digital Health
- 28. LITHIUM BATTERY