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The document discusses electrolysis and electrolytic cells. Electrolysis is a process that uses an external energy source to drive a non-spontaneous reaction. In an electrolytic cell, electrons flow in the opposite direction compared to a galvanic cell. An example reaction and calculation of the standard cell potential is provided for an electrolytic cell containing NaCl. Electrolysis is used in processes like electroplating to coat one metal onto another.
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Electrolytes are substances that can conduct electricity in the molten or liquid state and undergo chemical changes. Electrolysis is a process where electrolytes are broken down into their constituent elements by passing electricity through them. During electrolysis, ions migrate to the oppositely charged electrodes. At the anode, ions lose electrons and form gases or dissolve. At the cathode, ions gain electrons and form solid elements. Examples of electrolysis of molten lead(II) bromide and lead(II) oxide are described through their half reactions at the anode and cathode and overall reactions.
Conservation Of Energy
The document discusses the conservation of energy. It defines energy as the ability to do work and explains that energy cannot be created or destroyed, only transformed from one form to another. The law of conservation of energy states that the total amount of energy in an isolated system remains constant over time. The document provides examples of potential energy, which depends on an object's position in a force field, and kinetic energy, which depends on an object's mass and motion. It then demonstrates how the conservation of energy applies to a falling body, where the potential energy due to gravity is transformed into kinetic energy.
MICHAEL FARADAY PPT..
life style of great scientist Michael Faraday .....!
Michael Faraday, who came from a very poor family, became one of the greatest scientists in history. His achievement was remarkable in a time when science was the preserve of people born into privileged families. The unit of electrical capacitance is named the farad in his honor, with the symbol F.
The faraday is a dimensionless unit of electric charge quantity, equal to approximately 6.02 x 10 23 electric charge carriers. This is equivalent to one mole , also known as Avogadro's constant .
Education and Early Life
Michael Faraday was born on September 22, 1791 in London, England, UK. He was the third child of James and Margaret Faraday. His father was a blacksmith who had poor health. Before marriage, his mother had been a servant. The family lived in a degree of poverty.
Michael Faraday attended a local school until he was 13, where he received a basic education. To earn money for the family he started working as a delivery boy for a bookshop. He worked hard and impressed his employer. After a year, he was promoted to become an apprentice bookbinder
Michael Faraday’s Scientific Achievements and Discoveries:
It would be easy fill a book with details of all of Faraday’s discoveries – in both chemistry and physics. It is not an accident that Albert Einstein used to keep photos of three scientists in his office: Isaac Newton, James Clerk Maxwell and Michael Faraday.
Funnily enough, although in Faraday’s lifetime people had started to use the word physicist, Faraday disliked the word and always described himself as a philosopher. 1821: Discovery of Electromagnetic Rotation
This is a glimpse of what would eventually develop into the electric motor, based on Hans Christian Oersted’s discovery that a wire carrying electric current has magnetic properties.
1823: Gas Liquefaction and Refrigeration
In 1802 John Dalton had stated his belief that all gases could be liquified by the use of low temperatures and/or high pressures. Faraday provided hard evidence for Dalton’s belief by applying pressure to liquefy chlorine gas and ammonia gas for the first time.
1825: Discovery of Benzene
Historically, benzene is one of the most important substances in chemistry, both in a practical sense – i.e. making new materials; and in a theoretical sense – i.e. understanding chemical bonding. Michael Faraday discovered benzene in the oily residue left behind from producing gas for lighting in London.
1831: Discovery of Electromagnetic Induction
Faraday discovered that a varying magnetic field causes electricity to flow in an electric circuit.
1834: Faraday’s Laws of Electrolysis
This is the science of understanding what happens at the interface of an electrode with an ionic substance. Electrochemistry is the science that has produced the Li ion batteries and metal hydride batteries capable of powering modern mobile technology. Faraday’s laws are vital to our understanding of electrode reactions.
Electrolysis and Electroplating
The document discusses electroplating, which involves using electrolysis to coat a thin layer of one metal onto another. It explains that electroplating can be used to protect against corrosion or improve appearance. It then provides details on the electroplating process, where the metal to be plated is the cathode and connects to the negative terminal, while the metal used for plating is the anode and connects to the positive terminal. Ions of the anode metal dissolve and deposit onto the cathode. Copper plating of other metals like copper is provided as an example.
Electrolysis of brine
Electrolysis of brine PPT, from my chemistry teacher. Mr.Bedford. For anyone who can use this for help. This is for IGCSE /GCSE Level.
2012 topic 7.1
This document discusses chemical equilibrium. It defines equilibrium as a state where there are no observable changes over time and the concentrations of reactants and products remain constant. There are two types of equilibrium systems - physical/phase equilibrium and chemical equilibrium. Chemical equilibrium is achieved when the rates of the forward and reverse reactions are equal, resulting in constant concentrations. For the reaction of N2O4 decomposing to 2NO2, at equilibrium there is a mixture of both compounds as the forward and reverse reactions proceed at equal rates.
Tang 04 periodic trends
1) Atomic radius generally increases down a group and decreases across a period due to shielding effects of additional electron shells and increasing nuclear charge, respectively.
2) Ionization energy generally increases down a group and across a period as it becomes increasingly difficult to remove an electron due to greater nuclear attraction from less shielding and more protons. Exceptions occur when removing an electron would destabilize a full shell.
3) Electronegativity generally increases across a period as the effective nuclear charge felt by valence electrons increases with fewer shielding shells and more protons.
Mole concept numerical ..........
1. The document provides examples of solved problems on solutions involving calculations of molarity, molality, mole fractions, and other concentration units.
2. Problem 1 calculates the molarity of an ethyl alcohol solution. Problem 2 calculates the normality and molarity of a sulfuric acid solution.
3. Problem 3 calculates the molality and mole fractions of a glucose solution. The remaining problems provide additional examples of calculations involving concentration units for various chemical solutions.
Electrolysis
Electrolysis is a process where an electric current is passed through an electrolyte solution or molten salt, causing ions to migrate to the electrodes and undergo chemical reactions. During electrolysis, ions react at the electrodes by either gaining or losing electrons. Michael Faraday discovered that the mass of substance produced at the electrodes is directly proportional to the quantity of electricity passed through the electrolyte. His two laws of electrolysis state that the mass of substance liberated is directly proportional to the current over time, and that for the same quantity of electricity, the masses produced are proportional to the substances' equivalent masses. Electrolysis has many applications including metal extraction and coating materials with thin metal layers.
Topic 7 Concept Electrolysis
The document describes the electrolysis of a copper chloride solution using a voltage of 6V. During the process, chlorine gas is produced at one electrode while solid copper forms at the other electrode, as electrons are involved in the transfer of copper and chlorine between electrode reactions. Key reactions include the formation of chlorine gas at the anode from chloride ions and copper metal at the cathode from copper ions gaining electrons.
Aluminium Extraction
The document summarizes the process of extracting aluminium from bauxite ore. Bauxite ore is dissolved in cryolite to lower its melting point before being electrolyzed in a molten electrolyte. During electrolysis, positively charged aluminium ions move to the negatively charged carbon cathode, gaining electrons and forming aluminium atoms. Negatively charged oxide ions move to the positively charged carbon anode, losing electrons and forming oxygen gas. Some oxygen reacts with the carbon anode to form carbon dioxide, requiring frequent anode replacement. The overall process uses electrolysis to extract aluminium from bauxite ore dissolved in cryolite.
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ELECTROCHEMISTRY-1.pdf
Electrochemistry is the study of electron movement in an oxidation or reduction reaction at a polarized electrode surface. Each analyte is oxidized or reduced at a specific potential and the current measured is proportional to concentration. This technique is a powerful methodology towards bioanalysis.
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This document provides an introduction to electroanalytical chemistry. It discusses key concepts such as oxidation, reduction, and different types of electrochemical cells including galvanic and electrolytic cells. Examples of half-reactions and standard reduction potentials are given. The document also describes components of electrochemical cells such as electrodes, salt bridges, and electron flow. Diagrams illustrate electrolysis processes including the electrolysis of molten sodium chloride and aqueous sodium chloride. Standard cell notation for writing electrode reactions is also defined.
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This document provides an overview of the key concepts in electrochemistry including oxidation-reduction reactions, galvanic cells, standard reduction potentials, the Nernst equation, electrolysis, batteries, corrosion, and commercial electrolytic processes. It defines important terms, describes experimental set ups and calculations for electrochemical cells, and summarizes fundamental electrochemical principles and laws such as Faraday's laws of electrolysis.
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This document provides an overview of electrochemistry. It discusses electron transfer reactions, oxidation and reduction, voltaic cells, cell potentials, and balancing redox reactions. Key points include:
- Electron transfer reactions are oxidation-reduction or redox reactions that result in the generation of an electric current.
- Oxidation is the loss of electrons and reduction is the gain of electrons. Reduction cannot occur without oxidation providing electrons.
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Module 2_S7 and S8_Electrochemical Cells.pptx
An electrochemical cell consists of two electrodes separated by an electrolyte. There are two types: galvanic cells and electrolytic cells. A galvanic cell converts the chemical energy of a spontaneous redox reaction directly into electrical energy. The Nernst equation relates the cell potential (E) of a galvanic cell to the standard potential (E0), temperature, and reaction quotient through the concentrations of reactants and products. It allows calculation of cell potential under non-standard conditions.
Class XII Electrochemistry - Nernst equation.
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.
unit 3-electrochemistry.pptx
Electrochemistry deals with chemical reactions caused by electric currents or electric currents produced by chemical reactions. Galvanic cells convert chemical energy to electrical energy through redox reactions. Reversible cells like Daniel cells can undergo reactions in both directions while irreversible cells like zinc-silver cells cannot. Protective metal coatings through electroplating or electroless plating prevent corrosion by depositing a noble metal layer on a substrate.
Electro chemistry.docx
The document discusses electrochemistry and Daniel cells. It provides details on:
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- The components of a Daniel cell including zinc and copper electrodes, zinc sulfate and copper sulfate solutions, and a salt bridge to maintain electrical neutrality.
- How the cell produces a voltage through the oxidation of zinc and reduction of copper ions.
- How the voltage depends on the concentration of ions, as described by the Nernst equation.
Lecture 21- Electrochemical cells
This document discusses electrochemical cells and how they produce electric current from redox reactions. It explains that a voltaic cell separates the oxidation and reduction half-reactions into different compartments connected by a salt bridge and wire. The document provides examples of how to construct half-cells for zinc-copper and aluminum-nickel voltaic cells and calculates cell voltage using reduction potentials from a table.
Class XII Electrochemistry
CONTENTS
Electrochemistry: definition & importance
Conductors: metallic & electrolytic conduction,
Electrolytes, Electrochemical cell & electrolytic cell
A simple electrochemical cell: Galvanic cell or (Daniell Cell)
Cell reaction, cell representation, Salt bridge & its use,
Electrode potential, standard electrode potential, SHE,
Standard cell potential or standard electromotive force of a cell
Electrochemical series (Standard reduction potential values)
Nernst Equation, Relationship with Standard cell potential with Gibbs energy & also equilibrium constant
Resistance (R) & conductance (G) of a solution of an electrolyte
Conductivity (k) of solution, Cell constant (G*) & their units,
Molar conductivity (Λm) & its variation with concentration & temperature,
Debye Huckel Onsager equation & Limiting molar conductivity,
Kohlrausch’s law & its application & numerical problems.
Electrolytic cells & electrolysis.
Some examples of electrolysis of electrolytes in molten / aq. state.
Faraday’s laws of electrolysis: First & second law- numerical problems. Corrosion, Electrochemical theory of rusting.
Prevention of rusting.
1-Electrochemistry.pptx
This document provides an overview of electrochemistry. It defines electrochemistry as the branch of chemistry dealing with the transformation of electrical and chemical energy. It describes the key topics that will be covered, including conductors, electrochemical cells, electrode potentials, and how to predict spontaneity of reactions. It also summarizes the basic components and functions of electrolytic and galvanic (voltaic) cells, including how they convert between electrical and chemical energy.
Lecture 5-6: Hydrogen, Storage & Batteries
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presentation_electrochemistry_part_i_1651145702_423484.pdf
Electrochemistry is the study of chemical reactions that produce electricity and electrical energy's ability to cause non-spontaneous reactions. There are two types of electrochemical cells: galvanic cells that convert chemical energy to electrical energy, and electrolytic cells that use electrical energy to drive non-spontaneous reactions. Galvanic cells contain a spontaneous redox reaction like in Daniel cells where zinc oxidizes and copper reduces. Electrolytic cells use an external voltage to force nonspontaneous redox reactions. Standard electrode potentials allow prediction of reaction spontaneity based on the cell potential relative to the standard hydrogen electrode.
Electrochemical Cell or EC Cells which will generate electric current spontan...
Electrochemical Cell or EC Cells which will generate electric current spontan...janmarkdalutpittaban
In this PowerPoint presentation entitled “Electrochemical Cell” explains one of the topic of Inorganic Chemistry which means, a cell which generate electric current spontaneously. This includes features about objectives of the lesson, definition itself, other features of electrochemical cell, and also derivation of formulas and solution of the topic.GALVANIC AND ELECTROLYTIC CELL
A Daniell cell is a galvanic cell that uses the spontaneous redox reaction between zinc and copper(II) ions to produce an electric current. It consists of an outer copper vessel containing a copper electrode in a copper(II) sulfate solution and an inner amalgamated zinc electrode in a zinc sulfate solution, separated by a salt bridge. Electrons flow from the zinc anode through the external circuit to the copper cathode. The cell reactions involve the oxidation of zinc to zinc ions at the anode and the reduction of copper ions to copper at the cathode.
G12A Chapter 5 Section 5.1 Voltaic cell (1).pptx
chapter 5 volatic battery,chemistry third grade for chemistry department english section explain in details, slide share document
090643 Electrochemistry presentation.pdf
Electrochemistry is the study of chemical reactions caused by the movement of electric charge. Electrochemical cells produce electricity through spontaneous redox reactions. Galvanic cells produce electricity, while electrolytic cells use electricity to drive non-spontaneous reactions. The electrode potential and cell potential can be measured and related through the Nernst equation. Standard electrode potentials allow prediction of reaction spontaneity and oxidizing/reducing capabilities. Conductivity of electrolyte solutions depends on properties of the ions and solvent.
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This document provides information on wave quantum mechanics and electron configurations. It discusses:
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23 gases
- Gases have negligible volume and molecules are far apart with mostly empty space between them. Gas molecules move randomly in straight lines and collide elastically.
- The kinetic molecular theory describes gas properties including high translational energy of gas molecules that move randomly in all directions.
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04 periodic trends v2
- Elements in the same group have similar properties due to having the same number of valence electrons. Atoms get smaller from left to right in a period as protons are added, and larger from top to bottom in a group as energy levels are added.
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This document discusses acids and bases. It defines their key properties including reacting with metals, carbonates, conducting electricity, turning litmus paper colors, and neutralizing each other. It explains the theories of Arrhenius, Brønsted-Lowry, and Lewis on acids and bases. It also covers acid-base reactions, indicators, pH, titrations, strong/weak acids and bases, and acid-base stoichiometry.
23 gases
Gases are composed of molecules that are far apart from each other and occupy the entire volume of their container. Gas molecules move randomly in straight lines and collide elastically with each other and the container walls. The kinetic molecular theory describes gases as having negligible intermolecular forces and volume. Pressure, volume, temperature of a gas are related by the combined gas law and ideal gas law. Gas calculations involve using stoichiometry, the ideal gas law, and gas laws like Boyle's, Charles', and Gay-Lussac's to determine volume, pressure, amount, or temperature changes.
22 acids + bases
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This document provides an overview of solution stoichiometry and includes 3 sample problems demonstrating how to use a balanced chemical equation to solve for unknown quantities. The general steps are: 1) Write the balanced equation, 2) Convert given amounts to moles, 3) Use the mole ratio to calculate moles of the unknown, 4) Convert moles to the required unit. Sample Problem 1 calculates molar concentration of sulfuric acid. Sample Problem 2 determines the minimum volume of sodium carbonate needed. Sample Problem 3 calculates the mass of silver chromate precipitate formed.
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22 acids + bases
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For the full video of this presentation, please visit: https://www.edge-ai-vision.com/2024/06/building-and-scaling-ai-applications-with-the-nx-ai-manager-a-presentation-from-network-optix/
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