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oxidationreduction (redox) reactions, electrons are transferred from one species (the reductant) to another (the oxidant).
This transfer of electrons provides a means for converting chemical energy to electrical energy or vice versa.
The study of the relationship between electricity and chemical reactions is called electrochemistry.
In this App , we describe electrochemical reactions in more depth and explore some of their applications.
We start by describing how they can be used to generate an electrical potential, or voltage; and discuss factors that affect the magnitude of the potential.
We then explore the relationships among the electrical potential, the change in free energy, and the equilibrium constant for a redox reaction, which are all measures of the thermodynamic driving force for a reaction.
Finally, we examine two kinds of applications of electrochemical principles: (1) those in which a spontaneous reaction is used to provide electricity and (2) those in which electrical energy is used to drive a thermodynamically nonspontaneous reaction.
By the end of this App , you will understand why different kinds of batteries are used in cars, flashlights, cameras, and portable computers; how rechargeable batteries operate; and why corrosion occurs and how to slowif not preventit.
You will also discover how metal objects can be plated with silver or chromium for protection; how silver polish removes tarnish; and how to calculate the amount of electricity needed to produce aluminum, chlorine, copper, and sodium on an industrial scale.
Electrochemistry is the study of chemical processes that cause electrons to move.
This movement of electrons is called electricity, which can be generated by movements of electrons from one element to another in a reaction known as an oxidation-reduction ("redox") reaction.
Electrochemistry is the branch of physical chemistry concerned with the relationship between electrical potential difference, as a measurable and quantitative phenomenon, and identifiable chemical change, with the potential difference as an outcome of a particular chemical change, or vice versa.
These reactions involve electrons moving via an electronically-conducting phase (typically an external electrical circuit, but not necessarily, as in electroless plating) between electrodes separated by an ionically conducting and electronically insulating electrolyte (or ionic species in a solution).
When a chemical reaction is driven by an electrical potential difference, as in electrolysis, or if a potential difference results from a chemical reaction as in a battery or fuel cell, it is called an electrochemical reaction.
Unlike in other chemical reactions, in electrochemical reactions electrons are not transferred directly between atoms, ions, or molecules, but via the aforementioned electronically-conducting circuit.
This phenomenon is what distinguishes an electrochemical reaction from a conventional chemical reaction.
App Electrochemistry Include :
Oxidation States and Redox Reactions
Balanced Oxidation-Reduction Equations
Voltaic Cells
Cell Potential Under Standard Conditions
Gibbs Energy and Redox Reactions
Cell Potential Under Nonstandard Conditions
Batteries and Fuel Cells
Corrosion
Electrolysis
Electrochemistry (Exercises)
lead monoxide
litharge
fatty acid oxidation
beta oxidation of stearic acid
oxidation of fat
Eto chemistry
titanium 4 oxide
ruthenium tetroxide
nitric oxide
nickel oxide
carbon di oxide
hydrogen per oxide
oxidation
biological electrochemistry
electrochemical
electrochemical series
corrosion control
cathodic corrosion protection
electrolysis by Alison
hydrogen forklift batteries
This transfer of electrons provides a means for converting chemical energy to electrical energy or vice versa.
The study of the relationship between electricity and chemical reactions is called electrochemistry.
In this App , we describe electrochemical reactions in more depth and explore some of their applications.
We start by describing how they can be used to generate an electrical potential, or voltage; and discuss factors that affect the magnitude of the potential.
We then explore the relationships among the electrical potential, the change in free energy, and the equilibrium constant for a redox reaction, which are all measures of the thermodynamic driving force for a reaction.
Finally, we examine two kinds of applications of electrochemical principles: (1) those in which a spontaneous reaction is used to provide electricity and (2) those in which electrical energy is used to drive a thermodynamically nonspontaneous reaction.
By the end of this App , you will understand why different kinds of batteries are used in cars, flashlights, cameras, and portable computers; how rechargeable batteries operate; and why corrosion occurs and how to slowif not preventit.
You will also discover how metal objects can be plated with silver or chromium for protection; how silver polish removes tarnish; and how to calculate the amount of electricity needed to produce aluminum, chlorine, copper, and sodium on an industrial scale.
Electrochemistry is the study of chemical processes that cause electrons to move.
This movement of electrons is called electricity, which can be generated by movements of electrons from one element to another in a reaction known as an oxidation-reduction ("redox") reaction.
Electrochemistry is the branch of physical chemistry concerned with the relationship between electrical potential difference, as a measurable and quantitative phenomenon, and identifiable chemical change, with the potential difference as an outcome of a particular chemical change, or vice versa.
These reactions involve electrons moving via an electronically-conducting phase (typically an external electrical circuit, but not necessarily, as in electroless plating) between electrodes separated by an ionically conducting and electronically insulating electrolyte (or ionic species in a solution).
When a chemical reaction is driven by an electrical potential difference, as in electrolysis, or if a potential difference results from a chemical reaction as in a battery or fuel cell, it is called an electrochemical reaction.
Unlike in other chemical reactions, in electrochemical reactions electrons are not transferred directly between atoms, ions, or molecules, but via the aforementioned electronically-conducting circuit.
This phenomenon is what distinguishes an electrochemical reaction from a conventional chemical reaction.
App Electrochemistry Include :
Oxidation States and Redox Reactions
Balanced Oxidation-Reduction Equations
Voltaic Cells
Cell Potential Under Standard Conditions
Gibbs Energy and Redox Reactions
Cell Potential Under Nonstandard Conditions
Batteries and Fuel Cells
Corrosion
Electrolysis
Electrochemistry (Exercises)
lead monoxide
litharge
fatty acid oxidation
beta oxidation of stearic acid
oxidation of fat
Eto chemistry
titanium 4 oxide
ruthenium tetroxide
nitric oxide
nickel oxide
carbon di oxide
hydrogen per oxide
oxidation
biological electrochemistry
electrochemical
electrochemical series
corrosion control
cathodic corrosion protection
electrolysis by Alison
hydrogen forklift batteries
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