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.
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.
This document provides an overview of electrochemistry. It discusses key topics like what electrochemistry is, the history and founders of electrochemistry, oxidation-reduction reactions, balancing redox equations, standard electrode potential, the Nernst equation, batteries, corrosion, electrolysis, Faraday's laws of electrolysis, and more. The document serves as a high-level introduction to many fundamental concepts in electrochemistry.
This document discusses various topics related to hydrogen as a transport fuel, batteries, and fuel cells. It provides information on:
- Different types of vehicles that use hydrogen or batteries as their fuel/power source
- Methods for producing and storing hydrogen
- How electrochemical cells like batteries and fuel cells work through redox reactions
- Characteristics and reactions of different types of batteries including lead-acid, nickel-cadmium, and lithium-ion batteries.
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.
Introduction to electrochemistry by t. haraToru Hara
This document provides an introduction to electrochemistry. It discusses how electrochemistry involves the conversion of chemical energy to electrical energy, as in primary batteries where a spontaneous reaction between zinc and copper electrodes produces a flow of electrons. It also discusses the reverse process of converting electrical energy to chemical energy, as in secondary batteries that can be recharged. Key concepts covered include oxidation, reduction, standard reduction potentials, anodes, cathodes, and how electrochemical cells work through balanced redox reactions while conserving mass and charge.
Introduction to electrochemistry by t. haraToru Hara
This document provides an introduction to electrochemistry. It discusses how electrochemistry involves the conversion of chemical energy to electrical energy, as in primary batteries where spontaneous redox reactions produce a flow of electrons. It also discusses the conversion of electrical energy to chemical energy, as in secondary batteries that can be recharged. Key concepts covered include redox reactions, oxidation and reduction half-reactions, standard reduction potentials, and how primary cells like the Daniell cell use differences in standard reduction potentials to generate electrical energy through spontaneous redox reactions.
The document discusses electrochemistry and Daniel cells. It provides details on:
- How Daniel cells work by converting chemical energy from a redox reaction of zinc and copper into electrical energy.
- 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.
Module 2_S7 and S8_Electrochemical Cells.pptxAdittyaSenGupta
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.
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.
This document provides an overview of electrochemistry. It discusses key topics like what electrochemistry is, the history and founders of electrochemistry, oxidation-reduction reactions, balancing redox equations, standard electrode potential, the Nernst equation, batteries, corrosion, electrolysis, Faraday's laws of electrolysis, and more. The document serves as a high-level introduction to many fundamental concepts in electrochemistry.
This document discusses various topics related to hydrogen as a transport fuel, batteries, and fuel cells. It provides information on:
- Different types of vehicles that use hydrogen or batteries as their fuel/power source
- Methods for producing and storing hydrogen
- How electrochemical cells like batteries and fuel cells work through redox reactions
- Characteristics and reactions of different types of batteries including lead-acid, nickel-cadmium, and lithium-ion batteries.
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.
Introduction to electrochemistry by t. haraToru Hara
This document provides an introduction to electrochemistry. It discusses how electrochemistry involves the conversion of chemical energy to electrical energy, as in primary batteries where a spontaneous reaction between zinc and copper electrodes produces a flow of electrons. It also discusses the reverse process of converting electrical energy to chemical energy, as in secondary batteries that can be recharged. Key concepts covered include oxidation, reduction, standard reduction potentials, anodes, cathodes, and how electrochemical cells work through balanced redox reactions while conserving mass and charge.
Introduction to electrochemistry by t. haraToru Hara
This document provides an introduction to electrochemistry. It discusses how electrochemistry involves the conversion of chemical energy to electrical energy, as in primary batteries where spontaneous redox reactions produce a flow of electrons. It also discusses the conversion of electrical energy to chemical energy, as in secondary batteries that can be recharged. Key concepts covered include redox reactions, oxidation and reduction half-reactions, standard reduction potentials, and how primary cells like the Daniell cell use differences in standard reduction potentials to generate electrical energy through spontaneous redox reactions.
The document discusses electrochemistry and Daniel cells. It provides details on:
- How Daniel cells work by converting chemical energy from a redox reaction of zinc and copper into electrical energy.
- 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.
Module 2_S7 and S8_Electrochemical Cells.pptxAdittyaSenGupta
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.
This document provides information on electrochemistry and electrochemical cells. It defines electrochemistry as the study of electricity production from spontaneous chemical reactions and use of electrical energy for non-spontaneous reactions. It describes different types of electrochemical cells including galvanic cells that convert chemical to electrical energy and electrolytic cells that do the opposite. Key concepts discussed include electrode potentials, standard hydrogen electrode, Nernst equation, and factors affecting cell potential. Common electrochemical devices like batteries and the corrosion process are also summarized.
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 redox reactions, electrochemistry, and electrochemical cells. It begins by defining key concepts like oxidation, reduction, oxidizing agents, and reducing agents. It then provides examples of redox reactions and discusses how electrochemical cells work. The rest of the document covers topics like cell notation, standard electrode potentials, how to determine if a redox reaction is spontaneous, the relationship between cell potential and Gibbs free energy, the effect of concentration on cell potential, corrosion, batteries, and different types of electrochemical cells like voltaic cells, electrolytic cells, and fuel cells.
This document discusses redox reactions, electrochemistry, and electrochemical cells. It begins by defining key concepts like oxidation, reduction, oxidizing agents, and reducing agents. It then provides examples of redox reactions and discusses how electrochemical cells work. The rest of the document covers topics like cell notation, standard electrode potentials, how to determine if a redox reaction is spontaneous, the relationship between cell potential and Gibbs free energy, the effect of concentration on cell potential, corrosion, batteries, and different types of electrochemical cells like voltaic cells, electrolytic cells, and fuel cells.
1. Faraday's laws of electrolysis state that the amount of substance deposited at an electrode is directly proportional to the quantity of electricity passed through the electrolyte.
2. The amount of different substances liberated by the same quantity of electricity passing through an electrolytic solution are proportional to their chemical equivalent weights.
3. Electrochemistry involves the study of corrosion, batteries, and the relationship between cell potential and Gibbs free energy.
Electrochemistry is the study of chemical reactions at the interface of an electrode and electrolyte. It deals with the interaction between electrical energy and chemical changes. Some key founders of electrochemistry include John Daniel, Michael Faraday, William Nicholson, and Johann Ritter. Electrochemistry principles are applied in batteries, corrosion prevention, and electrolysis where electrical energy is used to drive nonspontaneous redox reactions.
This document discusses electrochemistry and electrochemical cells. It defines electrochemistry as the study of chemical reactions that produce electricity or use electricity to cause 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. Examples of galvanic cells include Daniell cells and concentration cells. The document explains concepts like standard electrode potentials, the electrochemical series, and how to represent cell diagrams according to IUPAC recommendations. It also discusses the functions of salt bridges and how junction potentials can affect cell potentials.
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.
Electrochemistry involves the study of electricity produced from spontaneous chemical reactions in galvanic cells and the use of electricity to drive non-spontaneous reactions in electrolytic cells. Galvanic cells produce electricity through spontaneous redox reactions, with oxidation occurring at the anode and reduction at the cathode. Electrolytic cells use electricity to carry out non-spontaneous reactions. The potential difference between electrodes in a galvanic cell is called the cell potential, which can be calculated using standard electrode potentials and concentrations based on the Nernst equation.
3rd Lecture on Electrochemistry | Chemistry Part I | 12th StdAnsari Usama
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.
The document provides an overview of key concepts in electrochemistry including:
1) The components and operation of electrochemical cells including voltaic cells like batteries and fuel cells as well as electrolytic cells.
2) Half-reactions, electrode potentials, and using these to determine spontaneity of redox reactions.
3) Processes like corrosion, electroplating, electrolysis of water, and recharging of batteries that involve redox reactions driven by electrical energy.
This document summarizes an electrochemistry chapter that covers:
- Types of electrochemical cells including galvanic and electrolytic cells
- Reversible electrodes like metal-metal ion, gas, and metal-insoluble electrodes
- Determining standard electrode potentials and using the Nernst equation
- Examples of calculating cell potentials and writing electrode half reactions
This document summarizes an electrochemistry chapter that covers:
- Types of electrochemical cells including galvanic and electrolytic cells
- Reversible electrodes like metal-metal ion, gas, and metal-insoluble electrodes
- Determining standard electrode potentials and using the Nernst equation
- Examples of calculating cell potentials and writing electrode half reactions
ENGINEERING CHEMISTRY- Solved Model question paper,2017-18rashmi m rashmi
This document contains the solved question paper for Engineering Chemistry. It discusses several topics:
1. The derivation of the Nernst equation for single electrode potential and its relationship to Gibbs free energy.
2. Concentration cells and calculating concentrations from cell potential.
3. The construction and working of a methanol-oxygen fuel cell.
4. The construction, working, and applications of lithium-ion batteries.
5. Key battery characteristics like cell potential, capacity, and cycle life.
6. The construction and advantages of a calomel reference electrode.
Electroanalytical methods provide several advantages for quantitative analytical chemistry. They involve measuring the electrical properties of analyte solutions in electrochemical cells. Some key points:
- Electroanalytical methods allow easy automation through electrical signal measurements. They can also determine low analyte concentrations without difficulty.
- Electrochemical processes involve the transfer of electrons between substances during redox reactions. This occurs at the interface between electrodes and solutions in electrochemical cells.
- Advantages include low cost compared to spectroscopy and the ability to easily automate measurements and detect low analyte concentrations through electrical signals.
Corrosion is the deterioration of a material due to a reaction with its environment. Metals corrode through an electrochemical process where the metal oxidizes, releasing energy added during its production. Corrosion occurs via the formation of an electrochemical cell, requiring an anode, cathode, electrolyte, electrical connection, and potential difference. The thermodynamics of corrosion can predict if a reaction is possible based on its change in Gibbs free energy. Kinetically, corrosion rates can be estimated using Faraday's law relating current over time to mass lost. Common factors like environment, metal properties, and geometry can influence corrosion behavior and rates.
The document provides information about electrochemistry. It discusses oxidation-reduction reactions and how they involve the transfer of electrons between species. It explains how to assign oxidation numbers to keep track of electrons gained and lost. Balancing oxidation-reduction reactions using the half-reaction method is also covered. Finally, the document discusses voltaic cells, electrolytic cells, and applications of electrochemistry such as electroplating.
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.
This document provides information on electrochemistry and electrochemical cells. It defines electrochemistry as the study of electricity production from spontaneous chemical reactions and use of electrical energy for non-spontaneous reactions. It describes different types of electrochemical cells including galvanic cells that convert chemical to electrical energy and electrolytic cells that do the opposite. Key concepts discussed include electrode potentials, standard hydrogen electrode, Nernst equation, and factors affecting cell potential. Common electrochemical devices like batteries and the corrosion process are also summarized.
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 redox reactions, electrochemistry, and electrochemical cells. It begins by defining key concepts like oxidation, reduction, oxidizing agents, and reducing agents. It then provides examples of redox reactions and discusses how electrochemical cells work. The rest of the document covers topics like cell notation, standard electrode potentials, how to determine if a redox reaction is spontaneous, the relationship between cell potential and Gibbs free energy, the effect of concentration on cell potential, corrosion, batteries, and different types of electrochemical cells like voltaic cells, electrolytic cells, and fuel cells.
This document discusses redox reactions, electrochemistry, and electrochemical cells. It begins by defining key concepts like oxidation, reduction, oxidizing agents, and reducing agents. It then provides examples of redox reactions and discusses how electrochemical cells work. The rest of the document covers topics like cell notation, standard electrode potentials, how to determine if a redox reaction is spontaneous, the relationship between cell potential and Gibbs free energy, the effect of concentration on cell potential, corrosion, batteries, and different types of electrochemical cells like voltaic cells, electrolytic cells, and fuel cells.
1. Faraday's laws of electrolysis state that the amount of substance deposited at an electrode is directly proportional to the quantity of electricity passed through the electrolyte.
2. The amount of different substances liberated by the same quantity of electricity passing through an electrolytic solution are proportional to their chemical equivalent weights.
3. Electrochemistry involves the study of corrosion, batteries, and the relationship between cell potential and Gibbs free energy.
Electrochemistry is the study of chemical reactions at the interface of an electrode and electrolyte. It deals with the interaction between electrical energy and chemical changes. Some key founders of electrochemistry include John Daniel, Michael Faraday, William Nicholson, and Johann Ritter. Electrochemistry principles are applied in batteries, corrosion prevention, and electrolysis where electrical energy is used to drive nonspontaneous redox reactions.
This document discusses electrochemistry and electrochemical cells. It defines electrochemistry as the study of chemical reactions that produce electricity or use electricity to cause 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. Examples of galvanic cells include Daniell cells and concentration cells. The document explains concepts like standard electrode potentials, the electrochemical series, and how to represent cell diagrams according to IUPAC recommendations. It also discusses the functions of salt bridges and how junction potentials can affect cell potentials.
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.
Electrochemistry involves the study of electricity produced from spontaneous chemical reactions in galvanic cells and the use of electricity to drive non-spontaneous reactions in electrolytic cells. Galvanic cells produce electricity through spontaneous redox reactions, with oxidation occurring at the anode and reduction at the cathode. Electrolytic cells use electricity to carry out non-spontaneous reactions. The potential difference between electrodes in a galvanic cell is called the cell potential, which can be calculated using standard electrode potentials and concentrations based on the Nernst equation.
3rd Lecture on Electrochemistry | Chemistry Part I | 12th StdAnsari Usama
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.
The document provides an overview of key concepts in electrochemistry including:
1) The components and operation of electrochemical cells including voltaic cells like batteries and fuel cells as well as electrolytic cells.
2) Half-reactions, electrode potentials, and using these to determine spontaneity of redox reactions.
3) Processes like corrosion, electroplating, electrolysis of water, and recharging of batteries that involve redox reactions driven by electrical energy.
This document summarizes an electrochemistry chapter that covers:
- Types of electrochemical cells including galvanic and electrolytic cells
- Reversible electrodes like metal-metal ion, gas, and metal-insoluble electrodes
- Determining standard electrode potentials and using the Nernst equation
- Examples of calculating cell potentials and writing electrode half reactions
This document summarizes an electrochemistry chapter that covers:
- Types of electrochemical cells including galvanic and electrolytic cells
- Reversible electrodes like metal-metal ion, gas, and metal-insoluble electrodes
- Determining standard electrode potentials and using the Nernst equation
- Examples of calculating cell potentials and writing electrode half reactions
ENGINEERING CHEMISTRY- Solved Model question paper,2017-18rashmi m rashmi
This document contains the solved question paper for Engineering Chemistry. It discusses several topics:
1. The derivation of the Nernst equation for single electrode potential and its relationship to Gibbs free energy.
2. Concentration cells and calculating concentrations from cell potential.
3. The construction and working of a methanol-oxygen fuel cell.
4. The construction, working, and applications of lithium-ion batteries.
5. Key battery characteristics like cell potential, capacity, and cycle life.
6. The construction and advantages of a calomel reference electrode.
Electroanalytical methods provide several advantages for quantitative analytical chemistry. They involve measuring the electrical properties of analyte solutions in electrochemical cells. Some key points:
- Electroanalytical methods allow easy automation through electrical signal measurements. They can also determine low analyte concentrations without difficulty.
- Electrochemical processes involve the transfer of electrons between substances during redox reactions. This occurs at the interface between electrodes and solutions in electrochemical cells.
- Advantages include low cost compared to spectroscopy and the ability to easily automate measurements and detect low analyte concentrations through electrical signals.
Corrosion is the deterioration of a material due to a reaction with its environment. Metals corrode through an electrochemical process where the metal oxidizes, releasing energy added during its production. Corrosion occurs via the formation of an electrochemical cell, requiring an anode, cathode, electrolyte, electrical connection, and potential difference. The thermodynamics of corrosion can predict if a reaction is possible based on its change in Gibbs free energy. Kinetically, corrosion rates can be estimated using Faraday's law relating current over time to mass lost. Common factors like environment, metal properties, and geometry can influence corrosion behavior and rates.
The document provides information about electrochemistry. It discusses oxidation-reduction reactions and how they involve the transfer of electrons between species. It explains how to assign oxidation numbers to keep track of electrons gained and lost. Balancing oxidation-reduction reactions using the half-reaction method is also covered. Finally, the document discusses voltaic cells, electrolytic cells, and applications of electrochemistry such as electroplating.
Similar to electrochemistry-141128223112-conversion-gate02.pptx (20)
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.
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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
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
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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.
This slide is special for master students (MIBS & MIFB) in UUM. Also useful for readers who are interested in the topic of contemporary Islamic banking.
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2. What is
electrochemistry?
Electrochemistry is the study of
chemical reactions which take placeat
the interface of an electrode usually a
solid, metal or semiconductor and an
ionic conductor , theelectrolyte.
Electrochemistry deals with the
interaction between electricalenergy
and chemical change.
3. History of electrochemistry
t
English chemist john Daniel and physicist
Michael faraday both credited as founders
of electrochemistrytoday.
The first germen physicist Otto von
Guericke created the electric
generater,which produced staticelectricity
by applying friction in themachine.
The English scientist William Gilbertspen
17 years experimenting with magnetism
and toa lesserextentelectricity.
john
Daniel
Michael
faraday
4. The french chemistcharles francoisde cisternrydu fay
had discovered two types of staticelectricity.
William Nicholson and Johann Wilhelm Ritter
succeeded in decomposing water into hydrogenand
oxygen byelectrolysis.
Ritter discovered the process ofelectroplating.
William Hyde Wollaston made improvements tothe
galvaniccells.
Orsted’sdiscoveryof the magneticeffectof electrical
currents and further work on electromagnetism to
others.
5. Michael Faraday'sexperiments led him tostate his two
laws of electrochemistry and john Daniel invented
primary cells.
Paul Heroult and Charles M.Hall developedan
efficient method to obtain aluminum using
electrolysis of moltenalumina.
Nernstdeveloped the theoryof theelectromotive force
and his equation known as Nernst equation, which
related thevoltagesof a cell to its properties.
Quantumelectrochemistrywasdeveloped by Revaz
dogonadeze and hispupils.
6. Oxidation-Reduction
The term redox stands forreduction-oxidation
It refers to electrochemical processesinvolving
electron transfer to or from a molecule or iron
changing its states.
Theatom or moleculewhich loseselectrons is known
as the reducingagent.
The substancewhich accepts theelectrons iscalled the
oxidizing agent.
10. Standard electrode potential
Toallow prediction of the cellpotential,
tabulationsof standard electrode potential are available.
Tabulations are referenced to the standardhydrogen
electrode.
The standard hydrogen electrode undergoes thereaction
2 H+
+ 2 e–
→H
(aq) 2
11. Standard electrode potentialsare usually tabulated
as reduction potentials.
The reactionsare reversibleand the roleof particular
electrode in a cell depends on the relative oxi./red.
Potential of both electrodes.
The cell potential is then calculated as the sum of
reduction potential for cathode and the oxidation
potential foranode.
For example, the standard electrode potential for a
copper electrodeis:
Cell diagram
Pt(s) | H2 (1 atm) | H+
(1 M ) || Cu2 +
(1 M ) |
Cu(s)
E°cell = E°red (cathode) – E°red (anode)
12. Gibbs free energy and cell
potential
Though cell potential Cell and get electricity nfaraday
in thecell:
Forstandard cell, thisequationcan wewritten
= -nFEcell
0
= -RTlnK=-nFE0
G cell
Though produce of electric energyconverted into
electricwork,
Wmax=Welectrical= -nFEcell
13. N e r n s t e q u a t i o n
n +
| = E 0 n +
| -
E ( M M ) ( M M ) l n
B u t s o l i d M c o n c e n t r a t e c o n s t a n t
n +
| = E 0 n +
| -
E ( M M ) ( M M ) l n
E x a m p l e o f D a n i e l c e l l
2 +
| = E 0 2 +
| -
E ( C u C u ) ( C u C u ) l n
F o r c a t h o d e :
F o r a n o d e :
2 +
| = E 0 2 +
| -
E ( Z n Z n ) ( Z n Z n ) l n
2 +
| - E 2 +
|
E ( C u C u ) ( Z n Z n )
- E 0 2 +
| - l n
( Z n Z n )
C e l l P o t e n t i a l : E c e l l = :
= E 0 2 +
| - l n
( C u C u )
= E c e l l = E 0
- l n
c e l l
14. Electrical resistivity
It is an intrinsic property thatquantities how stronglya
given material opposes the flow of electrical current.
Many resistors and conductors have a uniform cross
section with a uniform flowof electriccurrentand made
of one material
The electrical resistivitydefined
15. Electrical conductivity
The reciprocal of electrical resistivity, and measuresa
material’sability toconductan electriccurrent.
It is commonly represented byσ
Conductivity is definedas
Conductivity SI units of Siemens permeter.
16. Molar conductivity
Molarconductivity is defined as theconductivityof an
electrolyte solution divided by the molar
concentration of the electrolyte, and so measures the
efficiency with which a given electrolyte conducts
electricity insolution.
From definition, the molarconductivity
17. • Twocases should bedistinguished:
Strong eletrolyte and weakelectrolyte
For strongelectrolyte
Salts, strong acids and strong bases, the molar
conductivitydependsonlyweaklyon concentration.
18. For weakelectrolyte
The molarconductivitystronglydependson
concentration.
The more dilute a solution, the greater its molar
conductivity, due to increased ionicdissociation.
Forweak electrolyteobeys Oswald'sdilulation law.
19. Kohlrausch’s law of independent
migration of ions
High accuracy in dilutesolutions, molarconductivity
is composed of individual contributions ofions.
Limiting conductivity of anions and cations are
additive, theconductivityof a solutionof a salt is equal
to the sum of conductivity contributions from the
cation and anion
Λ0
m
=v+Λ0
+
+v-Λ0
-
20. Battery
Many types of battery have been commercializedand
represent an important practical application of
electrochemistry.
Early wet cells powered the first telegraph and
telephonesystems, and were the sourceof current for
electroplating.
The zinc-manganese dioxidedry cell was the first
portable, non-spill able battery type thatmade
flashlights and otherportabledevices practical.
21. The mercury battery using zinc and mercuric oxude
provided higher levelsof powerand capacity than the
original dry cell forearlyelectronicdevices.
Lead-acid battery was secondarybattery.
The electrochemical reaction that produced current
was reversible, allowing electrical energy and chemical
energy to be interchanged asneeded.
Lead-acid cellscontinue to be widelyused in
automobiles.
22. The lithium battery, which does not use water in the
electrolyte, provides improved performance overother
types.
Rechargeable lithium ion battery is an essential partof
many mobiledevices.
23. Corrosion
Corrosion is the term applied tosteel rustcaused byan
electrochemical process.
Corrosion of iron in the form of reddish rust, black
tarnish on silver, red orgreen may beappearon copper
and its alloys, such asbrass.
24. Prevention of corrosion
Coating
Metalscan becoated with paintorother less
conductive metals.
This prevents the metal surface from being exposed to
electrolytes.
Scratchesexposing the metal substratewill result in
corrosion.
25. • Sacrificial anodes
The method commonly used to protect a structural
metal is toattach a metal which is moreanodic than
the metal to beprotected.
This forces the structural metal to be catholic thus
spared corrosion. it is calledsacrificial.
Zinc bars areattached tovarious locationson steel
ship hulls torender the ship hull catholic.
Other metal used magnesium.
26. Electrolysis
The spontaneous redox
reactions of a conventional
battery produce electricity
through the differentchemical
potentials of the cathode and
anode in theelectrolyte.
Electrolysis requires an
external source of electrical
energy to include a chemical
reaction , and this process
takes place in acompartment
called an electrolyticcell.
27. Electrolysis of molten sodium
chlorine
This process can yield large amounts of metallic
sodium and gaseous chlorine, and widelyused on
mineral dressing and metallurgy industries.
When molten, the salt sodium chloride can be
electrolyzed to yield metallic sodium andgaseous
chlorine.
This process takes place in a special cell named
DowR
nea
’sct
cio
en
ls
lt
.hattake place at Down's cell are the following
Anode (oxidation): 2 Cl–
→ Cl2(g) + 2 e–
Cathode (reduction): 2 Na+
+ 2 e–
→ 2 Na
(l) (l)
Overall reaction: 2 Na+
+ 2 Cl–
→ 2 Na + Cl
(l) (l) 2(g)
28. Quantitative electrolysis and
Faraday’s law
Quantitativeaspectsof electrolysiswereoriginally
developed by Michel faraday.
Faraday is alsocredited to havecoined the terms
electrolyte.
Electrolysisamong manyothers whilestudying
analysis of electrochemicalreactions.
Faraday advocateof the lawof conservationof energy.
29. First law
The mass of products yielded on the electrodes was
proportional to the the value of current supplied to the cell,
the length of time the current existed, and the molar mass
of the substance analyzed.
The amount of substance deposited on each electrode of an
electrolytic cell is directly proportional to the quantity of
electricity passed through thecell.
m=
30. Second law
Theamountsof bodieswhich areequivalent toeach
other in the ordinary chemical action have equal
quantities of of electricity naturally associated with
them.
Thequantitiesof different elementsdeposited bya
given amount of electricity are in the ratio of the
chemical equivalentweights
32. Branch of electrochemistry
Photoelectrochemistry
It is subfield of studywithin physical chemistry.
The interest in thisdomain is high in thecontextof
development of renewable energy conversion and
storage technology.
Theeffects of luminousradiation on the propertiesof
electrodes and on electrochemical reactions are the
subject of photoelectrochemistry
33. Semiconductor’selectrochemistry
Semiconductor material has a band gap and generates a
pair of electron and hole per absorbed photon if the
energy of the photon is higher than the band gap of the
semiconductor.
This property of semiconductor materials has been
successfullyused toconverted solarenergy intoelectrical
energy by photovoltaicdevices.
Semiconductor-electrolyte interface
When a semiconductorcomes intocontactwith a liquid,
to maintain electrostaticequillibrium
There will be a charge transfer between the
semiconductor and liquid phase,if formal redoxpotential
of redox species lies inside semiconductorband gap.
34. At thermodynamic eqilibrium, the fermi level of
semiconductorand the formal redox potential of redox
species and between interfacesemiconductor.
This introduce n-type semiconductor andp-type
semiconductor.
This semiconductorused as photovoltaicdevicesimilar to
solid state p-n junctiondevices.
Both n and p typesemiconductorcan used as photovoltaic
devices to convert solar energy into electrical energy and
are called photoelectricalcells
35. Boielectrochemistry
It is branch of electrochemistry and biophysical
chemistryconcerned with topics likecell electron-
proton transport, cell membrane potentials and
electrode reactions of redoenzymes.
Bioelectrochemistry isa science at the many junctions
of sciences.
36. Nanoelectrochemistry
Nanoelectrochemistry is a branch ofelectrochemistry
that investigates the electrical and electrochemical
propertiesof materialsat the nanometersize regime.
Nanoelectrochemistry plays significant role in the
fabricationof varioussensors, and devices fordetecting
molecules atvery law concentrations.
37. The term electrochemical nanostructuring can be used
to mean differentthings.
This term is employed to refer to generation at will of
nanostructure on electrode surface, involving a given
positioning with a certainprecision
The term nanostructure is used to describe the
generation of nanometric patternswith moveor less
narrow size distribution and a periodic or random
ordering on thesurface.
Butwithoutcontrol on the spatial locationof the
nanostructure.
38. Application of electrochemistry
There arevariousextremely importantelectrochemical
processes in both nature andindustry.
The coating of objects with metals or metal oxides
through electrodeposition and thedetectionof alcohol in
drunken drivers through the redox reactionof ethanol.
Diabetes blood sugar meters measure theamountof
glucose in the blood through its redox potential.
39. The generation of chemical energy through
photosynthesis in inherently an electrochemicalprocess.
Productionof metals likealuminiumand titanium from
theirores.
For Photoelectrochemistry
Artificial photosynthesis
Regenerative cell or Dye-sensitizedcell
Photo electrochemical splitting ofwater
40. For Boielectrochemistry
Someof different experimental techniques thatcan be
used to study bioelectrochemicalproblems.
Ampermetic of biosensors
Biofuel cells
Bioelectrosynthesis