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.
Class XII Electrochemistry - Nernst equation.Arunesh Gupta
Introduction, application of electrochemistry, metallic conduction & electrolytic conduction, electrolytes, electrochemical cell & electrolytic cell, Galvanic cell (Daniell cell), Standard reduction & oxidation potential, SHE as reference electrode, Standard emf of a cell or standard cell potential, Electrochemical series & its application, Nernst equation, Relationship between (i) Standard cell potential & equilibrium constant (ii) standard cell potential & standard Gibbs energy, some numerical problems.
Class XII Electrochemistry - Nernst equation.Arunesh Gupta
Introduction, application of electrochemistry, metallic conduction & electrolytic conduction, electrolytes, electrochemical cell & electrolytic cell, Galvanic cell (Daniell cell), Standard reduction & oxidation potential, SHE as reference electrode, Standard emf of a cell or standard cell potential, Electrochemical series & its application, Nernst equation, Relationship between (i) Standard cell potential & equilibrium constant (ii) standard cell potential & standard Gibbs energy, some numerical problems.
Includes a discussion of Voltaic and electrolytic cells, the Nernst equation and the relationship between electrochemical processes, chemical equilibrium and free energy.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
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.
Electrolytes also known as polar molecules are bonded by ionic bond. They conduct electricity in molten or dissolved state.TatvaChintan Pharma Chem is a renowned company that manufactures electrolytic chemicals.
Includes a discussion of Voltaic and electrolytic cells, the Nernst equation and the relationship between electrochemical processes, chemical equilibrium and free energy.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
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.
Electrolytes also known as polar molecules are bonded by ionic bond. They conduct electricity in molten or dissolved state.TatvaChintan Pharma Chem is a renowned company that manufactures electrolytic chemicals.
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.
Electrochemistry,Electrolytic and Metallic Conduction,Specific Resistance or resistivity (ρ),Specific Conductance or Conductivity (κ),Equivalent Conductance (Λ), Molar Conductance (Λm),Variation of Conductance with Dilution,Debye-Hückel-Onsager Equation,Kohlransch’s Law of Independent Migration of Ions,Faraday’s Laws of Electrolysis,Electrochemical Cells,The Nernst Equation,Oxidation Number
Oxidation Number / State Method For Balancing Redox Reactions,Half-Reaction or Ion-Electron Method For Balancing Redox Reactions,Half-Reaction or Ion-Electron Method For Balancing Redox Reactions,Common Oxidising and Reducing Agents
ELECTROCHEMISTRY - I
4.1 - Metallic and Electrolytic Conductors-Faraday’s Laws-Electro plating Specific conductance and Equivalent conductance - Measurement of equivalent conductance - Variation of Equivalent Conductance and Specific Conductance with Dilution Kohlrausch Law and its applications - Ostwald’s Dilution Law and its Limitations.
Electrical and Magnetic Properties of MaterialsAbeni9
Properties of a material which determine its response to an electric field.
Materials are classified based on their electrical properties as conductors, semiconductors and insulators and newly super conductors.
Introduction to Electrochemistry
- Electrochemistry explores the interplay between electrical energy and chemical reactions, focusing on oxidation-reduction (redox) reactions and electrochemical cells.
**Oxidation and Reduction**
- Oxidation involves the loss of electrons, while reduction involves the gain of electrons, summed up by the mnemonic OIL RIG. An example reaction is Zn + Cu²⁺ → Zn²⁺ + Cu.
**Redox Reactions in Everyday Life**
- Examples include the rusting of iron, cellular respiration, and the combustion of fuels.
**Electrochemical Cells**
- Two main types are Galvanic (Voltaic) cells, which convert chemical energy into electrical energy, and Electrolytic cells, which use electrical energy to drive chemical reactions. Components include the anode (where oxidation occurs), the cathode (where reduction occurs), and an electrolyte.
**Galvanic Cells**
- A common example is the Daniell Cell, which generates electrical energy through spontaneous redox reactions.
**Electrolytic Cells**
- These cells drive non-spontaneous reactions using electrical energy, such as the electrolysis of water to produce hydrogen and oxygen gases.
**Applications of Electrochemistry**
- Includes batteries (e.g., lithium-ion, alkaline), electroplating, corrosion prevention methods like galvanization, and fuel cells that directly convert chemical energy into electrical energy.
**Electrochemistry in Nature**
- Involves biochemical processes like the electron transport chain in mitochondria and natural galvanic cells, such as those influenced by lightning in soil.
**Summary**
- Understanding redox reactions and electrochemical cells is essential. Electrochemistry has a wide range of practical applications, making it a significant field of study.
**Discussion and Q&A**
- Engage with the audience to explore real-life applications and recent advancements in electrochemistry.
This summary encapsulates the key points and themes of the presentation, providing a concise overview of the fundamental concepts and applications of electrochemistry.
2024.06.01 Introducing a competency framework for languag learning materials ...Sandy Millin
http://sandymillin.wordpress.com/iateflwebinar2024
Published classroom materials form the basis of syllabuses, drive teacher professional development, and have a potentially huge influence on learners, teachers and education systems. All teachers also create their own materials, whether a few sentences on a blackboard, a highly-structured fully-realised online course, or anything in between. Despite this, the knowledge and skills needed to create effective language learning materials are rarely part of teacher training, and are mostly learnt by trial and error.
Knowledge and skills frameworks, generally called competency frameworks, for ELT teachers, trainers and managers have existed for a few years now. However, until I created one for my MA dissertation, there wasn’t one drawing together what we need to know and do to be able to effectively produce language learning materials.
This webinar will introduce you to my framework, highlighting the key competencies I identified from my research. It will also show how anybody involved in language teaching (any language, not just English!), teacher training, managing schools or developing language learning materials can benefit from using the framework.
Synthetic Fiber Construction in lab .pptxPavel ( NSTU)
Synthetic fiber production is a fascinating and complex field that blends chemistry, engineering, and environmental science. By understanding these aspects, students can gain a comprehensive view of synthetic fiber production, its impact on society and the environment, and the potential for future innovations. Synthetic fibers play a crucial role in modern society, impacting various aspects of daily life, industry, and the environment. ynthetic fibers are integral to modern life, offering a range of benefits from cost-effectiveness and versatility to innovative applications and performance characteristics. While they pose environmental challenges, ongoing research and development aim to create more sustainable and eco-friendly alternatives. Understanding the importance of synthetic fibers helps in appreciating their role in the economy, industry, and daily life, while also emphasizing the need for sustainable practices and innovation.
The Roman Empire A Historical Colossus.pdfkaushalkr1407
The Roman Empire, a vast and enduring power, stands as one of history's most remarkable civilizations, leaving an indelible imprint on the world. It emerged from the Roman Republic, transitioning into an imperial powerhouse under the leadership of Augustus Caesar in 27 BCE. This transformation marked the beginning of an era defined by unprecedented territorial expansion, architectural marvels, and profound cultural influence.
The empire's roots lie in the city of Rome, founded, according to legend, by Romulus in 753 BCE. Over centuries, Rome evolved from a small settlement to a formidable republic, characterized by a complex political system with elected officials and checks on power. However, internal strife, class conflicts, and military ambitions paved the way for the end of the Republic. Julius Caesar’s dictatorship and subsequent assassination in 44 BCE created a power vacuum, leading to a civil war. Octavian, later Augustus, emerged victorious, heralding the Roman Empire’s birth.
Under Augustus, the empire experienced the Pax Romana, a 200-year period of relative peace and stability. Augustus reformed the military, established efficient administrative systems, and initiated grand construction projects. The empire's borders expanded, encompassing territories from Britain to Egypt and from Spain to the Euphrates. Roman legions, renowned for their discipline and engineering prowess, secured and maintained these vast territories, building roads, fortifications, and cities that facilitated control and integration.
The Roman Empire’s society was hierarchical, with a rigid class system. At the top were the patricians, wealthy elites who held significant political power. Below them were the plebeians, free citizens with limited political influence, and the vast numbers of slaves who formed the backbone of the economy. The family unit was central, governed by the paterfamilias, the male head who held absolute authority.
Culturally, the Romans were eclectic, absorbing and adapting elements from the civilizations they encountered, particularly the Greeks. Roman art, literature, and philosophy reflected this synthesis, creating a rich cultural tapestry. Latin, the Roman language, became the lingua franca of the Western world, influencing numerous modern languages.
Roman architecture and engineering achievements were monumental. They perfected the arch, vault, and dome, constructing enduring structures like the Colosseum, Pantheon, and aqueducts. These engineering marvels not only showcased Roman ingenuity but also served practical purposes, from public entertainment to water supply.
Macroeconomics- Movie Location
This will be used as part of your Personal Professional Portfolio once graded.
Objective:
Prepare a presentation or a paper using research, basic comparative analysis, data organization and application of economic information. You will make an informed assessment of an economic climate outside of the United States to accomplish an entertainment industry objective.
Welcome to TechSoup New Member Orientation and Q&A (May 2024).pdfTechSoup
In this webinar you will learn how your organization can access TechSoup's wide variety of product discount and donation programs. From hardware to software, we'll give you a tour of the tools available to help your nonprofit with productivity, collaboration, financial management, donor tracking, security, and more.
The French Revolution, which began in 1789, was a period of radical social and political upheaval in France. It marked the decline of absolute monarchies, the rise of secular and democratic republics, and the eventual rise of Napoleon Bonaparte. This revolutionary period is crucial in understanding the transition from feudalism to modernity in Europe.
For more information, visit-www.vavaclasses.com
Palestine last event orientationfvgnh .pptxRaedMohamed3
An EFL lesson about the current events in Palestine. It is intended to be for intermediate students who wish to increase their listening skills through a short lesson in power point.
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
Unit 8 - Information and Communication Technology (Paper I).pdfThiyagu K
This slides describes the basic concepts of ICT, basics of Email, Emerging Technology and Digital Initiatives in Education. This presentations aligns with the UGC Paper I syllabus.
Chapter 3 - Islamic Banking Products and Services.pptx
Electrolysis
1.
2. In chemistry, the production of
chemical changes by passing and
electric current through a solution
or molten salt (electrolyte) resulting
in the migration of ions to the
electrode: positive ions (cations) to
the negative electrode(cathode)
and negative ions (anions) to the
positive electrode (anode).
3. During electrolysis, the ions
react with the electrode, either
receiving or giving up electrons.
The resultant atoms may be
liberated as gas or deposit as a
solid on the electrode, in
amount that are proportional to
the amount of current passed.
4. If negative ions move towards
the anode they lose electrons
and become neutral, resulting
in an oxidation reaction. If
positive ion move towards the
cathode and gain electron
becoming neutral. A reduction
reaction takes place.
7. Electrolysis is used for many
purposes, including the
extraction of metals from
ores, the cleaning of
archaeological artefacts, and
the coating of materials with
thin layers of metals.
8.
9.
10. Faraday’s laws of electrolysis
Michael Faraday discovered a
quantitative relationship
between the extent of
electrolysis and the quantities
of electricity passed and put
forward two laws.
11. First law
It states that the mass of a substance
liberated at the electrode is directly
proportional to the quantity of electricity
passed through the electrolyte.
Where z: is the constant called
electrochemical equivalent
I: is the current in ampere and
t: is the time in seconds.
12. Second law
It also states that, when the same
quantity of electricity is passed
through different electrolytes the
masses of substances formed at the
electrodes are proportional to their
equivalent masses.
i.e, =
In chamistry, the production of chemical changes by passing and electric current through a solution or molten salt (electrolyte) resulting in the migration of ions to the electrode: positive ions (cations) to the negative electrode(cathode) and negative ions (anions) to the positive electrode (anode).
During electrolysis, the ions react with the electrode, either recieving or giving up electrons. The resultant atoms may be liberated as gas or deposit as a solid on the electrode. In amount that are propotional to the amount of current passed
If negative ions move towards the anode they lose electrons and become neutral, resulting in an oxidation reaction. If positive ion move towards the cathode and gain electron bocoming neutral. A reduction reaction takes place
Michael Faraday
At cathode
Electrolysis is used for many purposes, inclusing the extraction of metals from ores, the cleaning of archeological artifacts, and the coating of materials with thin layers of metals.
Faraday’s laws of electrolysis
Micheal faraday dicovered a quantitative relationship between the extent of electrlysis and the quantities of electricity passed and put forward two laws.
First law
It states that the mass of a substace liberated at the electrode is directly proportional to the quantity of electitrcity passed through the electrolyte.
Where z: is the constant called electrochemical equivalent
I: is the current in ampere and
t: is the time in seconds.
Second law
It also states that, when the same quantity of electricity is passed through different eletrolytes the masses of substances formed at the electrodes are proportional to their equivalent masses.
