Electrochemistry class 12 ( a continuation of redox reaction of grade 11)ritik
Electrochemistry involves the study of chemical reactions that produce electricity and chemical reactions produced by electricity. A galvanic (voltaic) cell converts the chemical energy of a spontaneous redox reaction into electrical energy. Daniell's cell uses the redox reaction of zinc oxidizing copper ions to produce a cell potential of 1.1 V. An electrolytic cell uses an applied voltage to drive a nonspontaneous redox reaction in the opposite direction of the natural reaction in a galvanic cell. Standard reduction potentials allow prediction of the tendency of half-reactions to occur and their oxidizing or reducing power.
I Hope You all like it very much. I wish it is beneficial for all of you and you can get enough knowledge from it. Clear and appropriate objectives, in terms of what the audience ought to feel, think, and do as a result of seeing the presentation. Objectives are realistic – and may be intermediate parts of a wider plan.
Class XII Electrochemistry - Nernst equation.Arunesh Gupta
This document provides an overview of electrochemistry and some key concepts. It begins by defining electrochemistry as the study of how spontaneous chemical reactions can produce electricity and how electrical energy can drive non-spontaneous reactions. It then discusses several applications of electrochemistry including metal production, electroplating, and batteries. The document goes on to define conductors and the differences between metallic and electrolytic conduction. It also introduces concepts like galvanic cells, salt bridges, standard electrode potentials, and the electrochemical series. In summary, the document provides a broad introduction to fundamental electrochemistry topics and concepts.
This document discusses electrochemistry and provides definitions and examples of key concepts. It defines oxidation as the loss of electrons and reduction as the gain of electrons. An electrochemical reaction is one where a chemical reaction produces an electric current or where an electric current causes a chemical reaction. There are two types of electrochemical cells - galvanic cells where a chemical reaction produces a current, and electrolytic cells which use electricity to drive a non-spontaneous reaction. The document also discusses standard electrode potentials and how they are used to calculate cell emf and predict reaction spontaneity. Industrial applications of electrochemical cells mentioned include electrolysis, chloralkali production, and metal extraction from ores.
1. Electrolysis is the process of using an electric current to drive nonspontaneous chemical reactions. It involves electrochemical cells with an electrolyte solution and two electrodes connected to an external power source.
2. During electrolysis, ions migrate within the electrolyte - positive ions move toward the negatively charged cathode and negative ions move toward the positively charged anode. Reduction occurs at the cathode as ions gain electrons, while oxidation occurs at the anode as ions lose electrons.
3. Applications of electrolysis include electroplating metals onto surfaces, extracting reactive metals like aluminum from their ores, and producing chlorine and sodium hydroxide via the chlor-alkali process. Factors like electrode material and electrolyte concentration
This document discusses electrochemical cells and how they convert chemical energy to electrical energy. It provides details on galvanic cells specifically, including how they work and examples like the Daniel cell. Key points covered include:
- Galvanic cells utilize a redox reaction to generate an electromotive force (emf) and produce electrical energy.
- 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.
Saman Tanoli will present on electrochemical cells. The presentation will define electrochemical cells, describe their components and types, including voltaic/galvanic cells and electrolytic cells. It will explain the differences between galvanic and electrolytic cells and provide examples of their applications. Voltaic cells generate electricity from spontaneous redox reactions, while electrolytic cells use electricity to drive non-spontaneous reactions. Common examples are batteries and electroplating/electrorefining of metals.
This document provides an overview of electrochemical cells. It defines oxidation and reduction reactions and describes how electrons are transferred in these reactions. It explains the basic components and workings of electrolytic cells, which use an external power source to drive non-spontaneous chemical reactions, and galvanic cells, which generate electricity from spontaneous reactions. Reversible and irreversible electrodes are also discussed. Thermodynamics relationships for electrochemical cells are outlined.
Electrochemistry class 12 ( a continuation of redox reaction of grade 11)ritik
Electrochemistry involves the study of chemical reactions that produce electricity and chemical reactions produced by electricity. A galvanic (voltaic) cell converts the chemical energy of a spontaneous redox reaction into electrical energy. Daniell's cell uses the redox reaction of zinc oxidizing copper ions to produce a cell potential of 1.1 V. An electrolytic cell uses an applied voltage to drive a nonspontaneous redox reaction in the opposite direction of the natural reaction in a galvanic cell. Standard reduction potentials allow prediction of the tendency of half-reactions to occur and their oxidizing or reducing power.
I Hope You all like it very much. I wish it is beneficial for all of you and you can get enough knowledge from it. Clear and appropriate objectives, in terms of what the audience ought to feel, think, and do as a result of seeing the presentation. Objectives are realistic – and may be intermediate parts of a wider plan.
Class XII Electrochemistry - Nernst equation.Arunesh Gupta
This document provides an overview of electrochemistry and some key concepts. It begins by defining electrochemistry as the study of how spontaneous chemical reactions can produce electricity and how electrical energy can drive non-spontaneous reactions. It then discusses several applications of electrochemistry including metal production, electroplating, and batteries. The document goes on to define conductors and the differences between metallic and electrolytic conduction. It also introduces concepts like galvanic cells, salt bridges, standard electrode potentials, and the electrochemical series. In summary, the document provides a broad introduction to fundamental electrochemistry topics and concepts.
This document discusses electrochemistry and provides definitions and examples of key concepts. It defines oxidation as the loss of electrons and reduction as the gain of electrons. An electrochemical reaction is one where a chemical reaction produces an electric current or where an electric current causes a chemical reaction. There are two types of electrochemical cells - galvanic cells where a chemical reaction produces a current, and electrolytic cells which use electricity to drive a non-spontaneous reaction. The document also discusses standard electrode potentials and how they are used to calculate cell emf and predict reaction spontaneity. Industrial applications of electrochemical cells mentioned include electrolysis, chloralkali production, and metal extraction from ores.
1. Electrolysis is the process of using an electric current to drive nonspontaneous chemical reactions. It involves electrochemical cells with an electrolyte solution and two electrodes connected to an external power source.
2. During electrolysis, ions migrate within the electrolyte - positive ions move toward the negatively charged cathode and negative ions move toward the positively charged anode. Reduction occurs at the cathode as ions gain electrons, while oxidation occurs at the anode as ions lose electrons.
3. Applications of electrolysis include electroplating metals onto surfaces, extracting reactive metals like aluminum from their ores, and producing chlorine and sodium hydroxide via the chlor-alkali process. Factors like electrode material and electrolyte concentration
This document discusses electrochemical cells and how they convert chemical energy to electrical energy. It provides details on galvanic cells specifically, including how they work and examples like the Daniel cell. Key points covered include:
- Galvanic cells utilize a redox reaction to generate an electromotive force (emf) and produce electrical energy.
- 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.
Saman Tanoli will present on electrochemical cells. The presentation will define electrochemical cells, describe their components and types, including voltaic/galvanic cells and electrolytic cells. It will explain the differences between galvanic and electrolytic cells and provide examples of their applications. Voltaic cells generate electricity from spontaneous redox reactions, while electrolytic cells use electricity to drive non-spontaneous reactions. Common examples are batteries and electroplating/electrorefining of metals.
This document provides an overview of electrochemical cells. It defines oxidation and reduction reactions and describes how electrons are transferred in these reactions. It explains the basic components and workings of electrolytic cells, which use an external power source to drive non-spontaneous chemical reactions, and galvanic cells, which generate electricity from spontaneous reactions. Reversible and irreversible electrodes are also discussed. Thermodynamics relationships for electrochemical cells are outlined.
This document provides an overview of electrochemistry. It begins by defining electrochemistry as the study of chemical reactions at the interface of an electrode and electrolyte involving the interaction of electrical and chemical changes. The document then discusses the history and founders of electrochemistry, including Faraday's two laws of electrolysis. It explains key concepts such as oxidation-reduction reactions, balancing redox equations, and the Nernst equation. The document also covers applications including batteries, corrosion, electrolysis, and branches of electrochemistry like bioelectrochemistry and nanoelectrochemistry.
Standard electrode potentials measure the tendency of a redox system to gain or lose electrons compared to the standard hydrogen electrode, which is assigned 0 volts. The potential is defined as the difference in potential between a metal electrode and a standard hydrogen electrode, both immersed in 1 M solutions at 298 K and 1 atm pressure. Systems with more negative potentials can lose electrons more easily than hydrogen, while those with positive potentials can lose electrons less easily. Electrode potentials allow prediction of whether electrons will flow from one redox system to another when combined in an electrochemical cell.
ELECTRO CHEMISTRY l electrolytic cell std 12 lec 1MAYURI SOMPURA
This document discusses electrochemistry and different types of electrochemical cells. It explains that in an electrolytic cell, electrical energy is used to drive a non-spontaneous redox reaction to produce a chemical energy output. The cathode is where reduction occurs through electron gain, and the anode is where oxidation occurs through electron loss. An electrolytic solution contains molecules bound by ionic bonds that allow conduction when an electrical current is applied to the cell.
Electrode potential and its applicationsSaba Shahzadi
This document provides an overview of electrode potential and electrochemistry. It defines electrode potential as the voltage at an electrode that must be measured versus a reference electrode. Electrochemistry involves the interconversion of electrical and chemical energy through electrochemical cells, which contain two electrodes where oxidation and reduction reactions occur. The potential difference between the electrodes is known as the electromotive force (EMF) or cell potential. Electrode potential can be used to determine various properties including the strengths of oxidizing/reducing agents, thermodynamic potentials, concentrations, and equilibrium constants.
This document provides an overview of electrochemistry concepts including:
- Types of cells like reversible cells where equilibrium exists and irreversible cells where it does not.
- Different types of electrodes such as metal-metal ion electrodes containing a metal and its ions, gas electrodes containing a gas, and oxidation-reduction electrodes containing ions in different oxidation states.
- Key electrode reactions involving oxidation where electrons are removed from metals and reduction where electrons are gained by metal ions.
- Terminology used in electrochemistry like electrode, anode, cathode, and cell reactions.
The document discusses various topics in electrochemistry including: ionic motion in electrolytic conduction; electrolytes and electrolysis; electrolytic cells; conductance; specific conductance; equivalent conductance; molar conductance; variation of molar conductance with dilution; ionic mobility; Faraday's laws of electrolysis; and Ohm's law as applied to electrolytic conductors. It also describes migration of ions and the factors that influence ionic mobility such as size, charge, hydration, and temperature.
Introduction to electrochemistry 2 by t. haraToru Hara
This document provides an overview of electrochemistry concepts including:
1. Electrochemistry involves redox reactions where electrons are gained or lost at electrode interfaces.
2. Thermodynamics and kinetics control redox reactions based on potential differences and charge/mass transfer limitations.
3. The electric double layer forms at electrode interfaces and can be modeled by the Helmholtz and Stern models.
Electrochemistry studies chemical reactions at the interface between an electrode and an electrolyte. Oxidation occurs when an element loses electrons and reduction occurs when an element gains electrons. Galvanic cells produce electrical energy from spontaneous redox reactions. The Nernst equation relates cell potential to concentration. Faraday's laws state that the amount of reaction is proportional to charge and equivalent weights determine amounts deposited. Electrolysis is used industrially to refine and deposit metals.
The document discusses various types of electrochemical cells and batteries. It begins by introducing electrochemical cells and describing common battery types like alkaline batteries for household use and lithium-ion batteries that power electric vehicles and devices. The document then explains the basic components and functioning of electrochemical cells, including that oxidation occurs at the anode and reduction at the cathode. Examples are given of analyzing the copper-tin and hydrogen-silver electrochemical cells by identifying the half-reactions and cell potential. Instructions are provided on how to draw and analyze these example electrochemical cells.
F.Sc. Part 1 Chemistry.Ch.10.Test (Malik Xufyan)Malik Xufyan
The document contains information about chemistry test series books published by Malik Xufyan of JIAS Academy, Jhang Institute for Advanced Studies. It lists the titles of 9 books covering chemistry courses from 9th class to F.Sc. Part II, which are available in both chapter-wise and board paper-wise test series formats. It also provides the contact information of the publisher.
Electrochemistry involves redox reactions in galvanic cells that convert chemical energy to electrical energy. In a galvanic cell, oxidation occurs at the anode and reduction occurs at the cathode. A salt bridge completes the circuit between the two half cells and maintains electrical neutrality. When a zinc rod is used as the anode in a copper sulfate solution with a copper cathode, the zinc rod loses weight as it oxidizes while copper precipitates and the solution warms due to heat released, demonstrating the spontaneous conversion of chemical to electrical energy in a galvanic cell.
This document is a chemistry demonstration file that summarizes an experiment on the electrolysis of potassium iodide. It includes an index, certificate of completion, acknowledgements, aim, apparatus used, theory on electrolysis and Faraday's laws of electrolysis. It describes the reactions involved including the preferential oxidation of iodide ions at the anode and hydrogen evolution at the cathode. Observations of violet color at the anode due to iodine and pink color at the cathode due to hydroxide ions are reported. Precautions for the experiment and conclusions that match the observations are provided.
This document provides an overview of electrochemistry. It begins by defining electrochemistry as the study of chemical reactions at the interface of an electrode and electrolyte involving the interaction of electrical and chemical changes. The document then discusses the history and founders of electrochemistry, including Faraday's two laws of electrolysis. It explains key concepts such as oxidation-reduction reactions, balancing redox equations, and the Nernst equation. The document also covers applications including batteries, corrosion, electrolysis, and branches of electrochemistry like bioelectrochemistry and nanoelectrochemistry.
Standard electrode potentials measure the tendency of a redox system to gain or lose electrons compared to the standard hydrogen electrode, which is assigned 0 volts. The potential is defined as the difference in potential between a metal electrode and a standard hydrogen electrode, both immersed in 1 M solutions at 298 K and 1 atm pressure. Systems with more negative potentials can lose electrons more easily than hydrogen, while those with positive potentials can lose electrons less easily. Electrode potentials allow prediction of whether electrons will flow from one redox system to another when combined in an electrochemical cell.
ELECTRO CHEMISTRY l electrolytic cell std 12 lec 1MAYURI SOMPURA
This document discusses electrochemistry and different types of electrochemical cells. It explains that in an electrolytic cell, electrical energy is used to drive a non-spontaneous redox reaction to produce a chemical energy output. The cathode is where reduction occurs through electron gain, and the anode is where oxidation occurs through electron loss. An electrolytic solution contains molecules bound by ionic bonds that allow conduction when an electrical current is applied to the cell.
Electrode potential and its applicationsSaba Shahzadi
This document provides an overview of electrode potential and electrochemistry. It defines electrode potential as the voltage at an electrode that must be measured versus a reference electrode. Electrochemistry involves the interconversion of electrical and chemical energy through electrochemical cells, which contain two electrodes where oxidation and reduction reactions occur. The potential difference between the electrodes is known as the electromotive force (EMF) or cell potential. Electrode potential can be used to determine various properties including the strengths of oxidizing/reducing agents, thermodynamic potentials, concentrations, and equilibrium constants.
This document provides an overview of electrochemistry concepts including:
- Types of cells like reversible cells where equilibrium exists and irreversible cells where it does not.
- Different types of electrodes such as metal-metal ion electrodes containing a metal and its ions, gas electrodes containing a gas, and oxidation-reduction electrodes containing ions in different oxidation states.
- Key electrode reactions involving oxidation where electrons are removed from metals and reduction where electrons are gained by metal ions.
- Terminology used in electrochemistry like electrode, anode, cathode, and cell reactions.
The document discusses various topics in electrochemistry including: ionic motion in electrolytic conduction; electrolytes and electrolysis; electrolytic cells; conductance; specific conductance; equivalent conductance; molar conductance; variation of molar conductance with dilution; ionic mobility; Faraday's laws of electrolysis; and Ohm's law as applied to electrolytic conductors. It also describes migration of ions and the factors that influence ionic mobility such as size, charge, hydration, and temperature.
Introduction to electrochemistry 2 by t. haraToru Hara
This document provides an overview of electrochemistry concepts including:
1. Electrochemistry involves redox reactions where electrons are gained or lost at electrode interfaces.
2. Thermodynamics and kinetics control redox reactions based on potential differences and charge/mass transfer limitations.
3. The electric double layer forms at electrode interfaces and can be modeled by the Helmholtz and Stern models.
Electrochemistry studies chemical reactions at the interface between an electrode and an electrolyte. Oxidation occurs when an element loses electrons and reduction occurs when an element gains electrons. Galvanic cells produce electrical energy from spontaneous redox reactions. The Nernst equation relates cell potential to concentration. Faraday's laws state that the amount of reaction is proportional to charge and equivalent weights determine amounts deposited. Electrolysis is used industrially to refine and deposit metals.
The document discusses various types of electrochemical cells and batteries. It begins by introducing electrochemical cells and describing common battery types like alkaline batteries for household use and lithium-ion batteries that power electric vehicles and devices. The document then explains the basic components and functioning of electrochemical cells, including that oxidation occurs at the anode and reduction at the cathode. Examples are given of analyzing the copper-tin and hydrogen-silver electrochemical cells by identifying the half-reactions and cell potential. Instructions are provided on how to draw and analyze these example electrochemical cells.
F.Sc. Part 1 Chemistry.Ch.10.Test (Malik Xufyan)Malik Xufyan
The document contains information about chemistry test series books published by Malik Xufyan of JIAS Academy, Jhang Institute for Advanced Studies. It lists the titles of 9 books covering chemistry courses from 9th class to F.Sc. Part II, which are available in both chapter-wise and board paper-wise test series formats. It also provides the contact information of the publisher.
Electrochemistry involves redox reactions in galvanic cells that convert chemical energy to electrical energy. In a galvanic cell, oxidation occurs at the anode and reduction occurs at the cathode. A salt bridge completes the circuit between the two half cells and maintains electrical neutrality. When a zinc rod is used as the anode in a copper sulfate solution with a copper cathode, the zinc rod loses weight as it oxidizes while copper precipitates and the solution warms due to heat released, demonstrating the spontaneous conversion of chemical to electrical energy in a galvanic cell.
This document is a chemistry demonstration file that summarizes an experiment on the electrolysis of potassium iodide. It includes an index, certificate of completion, acknowledgements, aim, apparatus used, theory on electrolysis and Faraday's laws of electrolysis. It describes the reactions involved including the preferential oxidation of iodide ions at the anode and hydrogen evolution at the cathode. Observations of violet color at the anode due to iodine and pink color at the cathode due to hydroxide ions are reported. Precautions for the experiment and conclusions that match the observations are provided.
Electric cells produce electric current through a chemical reaction and can be dry or wet types. A dry cell has a metallic cylinder body with a flat base and cap, producing 1.5V of current. A torch bulb contains a filament inside a glass sphere attached to a metallic base, with the side as negative and bottom as positive terminals. For a torch to light, the positive pole of the cell must connect to the positive terminal of the bulb and negative pole to negative terminal. A torch may fail to light if the connections are loose, the bulb is fused, or the cell's energy is depleted.
The document discusses basic concepts of chemistry including atoms, molecules, mixtures, elements, compounds, laws of chemical combinations, Dalton's atomic theory, the mole concept, percentage composition, empirical and molecular formulas, stoichiometry, mass percent, mole fraction, molarity, and molality. It is presented by Studyduniya, an educational social network, to provide an overview of fundamental topics in physical chemistry.
Molecular Mean Field Theory of ions in Bulk and ChannelsBob Eisenberg
Life and most of chemistry occurs in ionic solutions, but ionic solutions have only recently been recognized as the complex fluids that they are. The molecular view shows ions interacting with surrounding water and nearby ions. Everything is correlated in a complex way because ions and water have diameters comparable to their interaction length. The molecular scale shows only a small part of the correlation enforced by electrodynamics. Current defined as Maxwell did to include the ethereal current is exactly conserved, and therefore correlated, over all scales reaching to macroscopic boundary conditions some 10^9× larger than atoms crucial in batteries and nerve cells.
Jinn Liang Liu and I have built a molecular field theory PNPB Poisson Nernst Planck Bikerman that deals with water as molecules and describes local interactions with a steric potential that depends on the volume fraction of molecules and voids between them. The correlations of electrodynamics are described by a fourth-order differential operator that gives (as outputs) ion-ion and ion-water correlations; the dielectric response (permittivity) of ionic solutions; and the polarization of water molecules, all using a single correlation length parameter. The theory fits experimental data on activity and differential capacitance in ionic solutions of varying composition and content, including mixtures. Potassium channels, Gramicidin, L-type calcium channels, and the Na/Ca transporter are computed in three dimensions from structures in the Protein Data Bank.
Numerical analysis faces challenges
Geometric singularities of molecular surfaces
strong electric fields (100 mV/nm) and resulting exponential nonlinearities, and the
enormous concentrations (> 10 M) often found where ions are important, for example, near electrodes in batteries, in ion channels, and in active sites of proteins.
Wide ranging concentrations of Ca^(2+) in (> 10M) and near (10^(-2) to 10^(-8)M) almost every protein in biological cells make matters worse.
Challenges have been overcome using methods developed over many decades by the large community that works on the computational electronics of semiconductors.
This document discusses electroanalytical techniques and provides an introduction to fundamental concepts. It describes why electroanalysis has become an important analytical tool, noting its wide range of applications from environmental monitoring to biomedical analysis. Advances in recent decades have increased the popularity of electroanalysis, such as the development of ultramicroelectrodes, tailored interfaces, coupling of biological components with electrochemical transducers, and microfabrication of molecular devices and detectors.
1) Electrochemistry is the science that combines electricity and chemistry, studying the transfer of electrons during chemical reactions driven by an external voltage or voltage created by a chemical reaction.
2) An electrochemical cell pairs an anode and cathode electrode in an electrolyte solution, allowing spontaneous redox reactions to generate an electric current in galvanic cells or using an applied current to drive non-spontaneous reactions in electrolytic cells.
3) In a Daniell cell, zinc undergoes oxidation at the anode to produce electrons, while copper is reduced at the cathode by the electrons, with both half-reactions occurring spontaneously to generate a current through an external load.
This document provides an overview of an educational website called Electrical Safety World. The website contains resources for teachers to teach students about electricity and electrical safety, including standards-based content, experiments, and worksheets. It uses games, activities, and experiments to teach students the principles of electricity and safety practices. The site is designed for elementary and middle school students and features areas for games, content for kids, tips for parents, and tools for teachers. It also includes features like a glossary and links to related sites.
This document discusses conducting materials used in dye-sensitized solar cells. It begins by providing background on solar cells and photovoltaics, and describes dye-sensitized solar cells. It then focuses on different types of conducting materials used in these cells, including conductive polymers and electrolyte systems using ionic liquids. The document concludes by discussing the promising results of using ionic liquid electrolytes to optimize the performance of dye-sensitized solar cells.
This document discusses a lecture on electrochemistry. It covers key concepts like electrolysis, Faraday's laws of electrolysis, and electrochemical cells.
Some key points covered include that electrolysis is the decomposition of a compound by an electric current, and involves oxidation and reduction reactions. Faraday's first law states the mass of a substance produced by electrolysis is directly proportional to the quantity of electricity used. Faraday's second law relates the masses of different substances deposited to their equivalent masses. An electrochemical cell uses a redox reaction to produce an electrical current.
This document provides an overview of electricity and electrical circuits. It defines electricity as the flow of electric current and notes that electricity is caused by an imbalance of positive and negative charges. It then explains that an electrical circuit provides a complete path for electricity to flow through devices. Common examples of circuits include household wiring and car batteries. The document discusses the differences between open and closed circuits and how switches are used to open and close circuits to control the flow of electricity.
The document discusses various topics related to electricity and electrotherapy. It defines electrotherapy as medical therapy using electric currents, also called electrotherapeutics. It then covers topics like atoms and ions, chemical bonds, insulators and conductors, static electricity, electric fields, electrical current, voltage, and resistance. Key points like Ohm's law relating current, voltage and resistance are also summarized.
The document discusses various topics related to the solid state including classification of solids, crystalline and amorphous structures, unit cells, point defects, magnetic properties, and more. Solids are classified as molecular, ionic, metallic, covalent and further divided based on their crystalline structure. Crystalline solids have definite geometric arrangements while amorphous solids have irregular particle shapes. Unit cells are the basic repeating units that make up crystal lattices. There are various types of unit cells including primitive, body-centered, and face-centered cells. Point defects refer to irregularities in the positions of atoms in crystalline solids. Magnetic properties of materials include paramagnetism, diamagnetism, ferromag
The document discusses the classification and properties of different types of polymers. Polymers are classified based on their mode of polymerization into addition polymers and condensation polymers. They are also classified based on molecular forces into elastomers, fibers, thermoplastic polymers, thermosetting polymers, and natural rubber. Examples of various polymers are provided along with their common uses such as nylon 6 for tire cords and fabrics and nylon 6,6 for textiles. Teflon is noted for its chemical inertness and use in non-stick coatings.
General Principle and Process of Isolation (Metallurgy)Shivani Jadhav
An In-Depth Concept of General Principle and Process of Isolation (Metallurgy) For IIT JEE (CHEMISTRY) Exams.
Join Studyduniya.com for More.
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The document discusses different types of hydrocarbons including alkanes, alkenes, and alkynes. It describes their general formulas, properties, reactions, and methods of preparation. Alkanes contain single bonds between carbons and do not react easily. Alkenes contain double bonds and participate in reactions like halogenation and oxidation. Alkynes contain triple bonds and undergo addition reactions with dihydrogen, halogens, and hydrogen halides. The document is from an educational social network providing chemistry content for IIT JEE preparation.
The document discusses reactions of haloalkanes and haloarenes. It describes various nucleophilic substitution, elimination, and electrophilic substitution reactions of haloalkanes. For haloarenes, it discusses that nucleophilic substitution is less favorable due to resonance effects. It also outlines electrophilic substitution reactions like halogenation, nitration, sulfonation, and Friedel-Crafts reactions that are possible for haloarenes. Reaction of haloarenes with metals like Wurtz-Fittig and Fittig reactions are additionally summarized.
How to Manage Your Lost Opportunities in Odoo 17 CRMCeline George
Odoo 17 CRM allows us to track why we lose sales opportunities with "Lost Reasons." This helps analyze our sales process and identify areas for improvement. Here's how to configure lost reasons in Odoo 17 CRM
A review of the growth of the Israel Genealogy Research Association Database Collection for the last 12 months. Our collection is now passed the 3 million mark and still growing. See which archives have contributed the most. See the different types of records we have, and which years have had records added. You can also see what we have for the future.
it describes the bony anatomy including the femoral head , acetabulum, labrum . also discusses the capsule , ligaments . muscle that act on the hip joint and the range of motion are outlined. factors affecting hip joint stability and weight transmission through the joint are summarized.
Introduction to AI for Nonprofits with Tapp NetworkTechSoup
Dive into the world of AI! Experts Jon Hill and Tareq Monaur will guide you through AI's role in enhancing nonprofit websites and basic marketing strategies, making it easy to understand and apply.
This presentation includes basic of PCOS their pathology and treatment and also Ayurveda correlation of PCOS and Ayurvedic line of treatment mentioned in classics.
How to Add Chatter in the odoo 17 ERP ModuleCeline George
In Odoo, the chatter is like a chat tool that helps you work together on records. You can leave notes and track things, making it easier to talk with your team and partners. Inside chatter, all communication history, activity, and changes will be displayed.
June 3, 2024 Anti-Semitism Letter Sent to MIT President Kornbluth and MIT Cor...Levi Shapiro
Letter from the Congress of the United States regarding Anti-Semitism sent June 3rd to MIT President Sally Kornbluth, MIT Corp Chair, Mark Gorenberg
Dear Dr. Kornbluth and Mr. Gorenberg,
The US House of Representatives is deeply concerned by ongoing and pervasive acts of antisemitic
harassment and intimidation at the Massachusetts Institute of Technology (MIT). Failing to act decisively to ensure a safe learning environment for all students would be a grave dereliction of your responsibilities as President of MIT and Chair of the MIT Corporation.
This Congress will not stand idly by and allow an environment hostile to Jewish students to persist. The House believes that your institution is in violation of Title VI of the Civil Rights Act, and the inability or
unwillingness to rectify this violation through action requires accountability.
Postsecondary education is a unique opportunity for students to learn and have their ideas and beliefs challenged. However, universities receiving hundreds of millions of federal funds annually have denied
students that opportunity and have been hijacked to become venues for the promotion of terrorism, antisemitic harassment and intimidation, unlawful encampments, and in some cases, assaults and riots.
The House of Representatives will not countenance the use of federal funds to indoctrinate students into hateful, antisemitic, anti-American supporters of terrorism. Investigations into campus antisemitism by the Committee on Education and the Workforce and the Committee on Ways and Means have been expanded into a Congress-wide probe across all relevant jurisdictions to address this national crisis. The undersigned Committees will conduct oversight into the use of federal funds at MIT and its learning environment under authorities granted to each Committee.
• The Committee on Education and the Workforce has been investigating your institution since December 7, 2023. The Committee has broad jurisdiction over postsecondary education, including its compliance with Title VI of the Civil Rights Act, campus safety concerns over disruptions to the learning environment, and the awarding of federal student aid under the Higher Education Act.
• The Committee on Oversight and Accountability is investigating the sources of funding and other support flowing to groups espousing pro-Hamas propaganda and engaged in antisemitic harassment and intimidation of students. The Committee on Oversight and Accountability is the principal oversight committee of the US House of Representatives and has broad authority to investigate “any matter” at “any time” under House Rule X.
• The Committee on Ways and Means has been investigating several universities since November 15, 2023, when the Committee held a hearing entitled From Ivory Towers to Dark Corners: Investigating the Nexus Between Antisemitism, Tax-Exempt Universities, and Terror Financing. The Committee followed the hearing with letters to those institutions on January 10, 202
Biological screening of herbal drugs: Introduction and Need for
Phyto-Pharmacological Screening, New Strategies for evaluating
Natural Products, In vitro evaluation techniques for Antioxidants, Antimicrobial and Anticancer drugs. In vivo evaluation techniques
for Anti-inflammatory, Antiulcer, Anticancer, Wound healing, Antidiabetic, Hepatoprotective, Cardio protective, Diuretics and
Antifertility, Toxicity studies as per OECD guidelines
How to Build a Module in Odoo 17 Using the Scaffold MethodCeline George
Odoo provides an option for creating a module by using a single line command. By using this command the user can make a whole structure of a module. It is very easy for a beginner to make a module. There is no need to make each file manually. This slide will show how to create a module using the scaffold method.
How to Build a Module in Odoo 17 Using the Scaffold Method
ElectroChemistry for IIT JEE
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Electrolytic cell is a device for using
electrical energy to carry non-spontaneous
chemical reactions.
ELECTROLYTIC CELL
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ELECTROLYTIC CELL
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The cell converts the chemical energy
liberated during the redox reaction to
electrical energy and has an electrical
potential equal to 1.1 V. when concentration
of Zn2+ and Cu2+ ions is unity. Such a device
is called a galvanic or a voltaic cell.
DANIELL CELL
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DANIELL CELL
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The reduction half reaction occurs on the
copper electrode while the oxidation half
reaction occurs on the zinc electrode. These
two portions of the cell are also called half-
cells or redox couples.
DANIELL CELL
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The standard hydrogen electrode consists of
a platinum electrode coated with platinum
black. The electrode is dipped in an acidic
solution and pure hydrogen gas is bubbled
through it.
STANDARD ELECTRODE POTENTIAL
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NERNST EQUATION
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RELATIONS FROM NERNST EQUATION
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(i) the nature of the electrolyte added
(ii) size of the ions produced and their
solvation
(iii) the nature of the solvent and its viscosity
(iv) concentration of the electrolyte
(v) temperature
CONDUCTANCE OF
ELECTROLYTIC SOLUTIONS
The conductivity of electrolytic (ionic)
solutions depends on:
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The SI unit of conductance is siemens,
represented by the symbol ‘S’ and is equal
to ohm
CONDUCTANCE OF
ELECTROLYTIC SOLUTIONS
-1
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CONDUCTIVITY OF IONIC SOLUTIONS
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Kohlrausch law of independent migration of
ions states that limiting molar conductivity
of an electrolyte can be represented as the
sum of the individual contributions of the
anion and cation of the electrolyte.
KOHLRAUSCH LAW
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WEAK ELECTROLYTES
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The amount of chemical reaction which
occurs at any electrode during electrolysis
by a current is proportional to the quantity
of electricity passed through the electrolyte
FARADAY’S LAWS OF ELECTROLYSIS
First Law:
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The amounts of different substances
liberated by the same quantity of electricity
passing through the electrolytic solution are
proportional to their chemical equivalent
weights.
FARADAY’S LAWS OF ELECTROLYSIS
Second Law:
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Fuel cell using H2 and O2 produces electricity.
FUEL CELLS