Electrochemistry

The course starts with the general introduction of electrochemistry. It further discusses oxidation state and oxidation reduction reaction or redox reactions in detail which involves balancing of redox reactions. The course then introduced voltaic cells which is followed by standard electrode potentials, strengths of oxidizing and reducing agents. The course also discussed the criteria of spontaneity like whether the redox reaction is spontaneous or not. It further discusses cell potential under nonstandard conditions, free energy and equilibrium constant which is followed by cell potential and concentration. The course is concluded with the discussion on stoichiometry of electrolysis.

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215 lectures

Educators

UO

Course Curriculum

18 videos

16 videos

16 videos

27 videos

Chemical Equilibrium

34 videos

Acids and Bases

37 videos

Aqueous Equilibria

18 videos

18 videos

Electrochemistry

18 videos

Nuclear Chemistry

13 videos

Electrochemistry Lectures

Electrochemistry

Electrochemistry - Intro

In chemistry, electrochemistry is a branch of physical chemistry that studies chemical reactions involving electrical energy, either directly or indirectly. The name derives from the Greek words for amber (electron) and chemistry (chemeia). Electrochemistry deals with the electron transfer reactions that take place at the interface of two electrodes in contact with an electrolyte. The study of these reactions is associated with the study of electrolysis. The process of electrolysis is used to generate a potential difference (voltage) between two electrodes, which is used to drive an electrical current through the electrolytic solution.

Umut Ozuguzel

UO

Electrochemistry

Balancing Redox Equations - Overview

In chemistry, a redox reaction is a chemical reaction in which the oxidation states of the atoms of the participating elements are changed. Any such reaction involves both a reduction process and a complementary oxidation process, two key concepts involved with electron transfer processes. A redox reaction may be written with either an oxidation sign or a reduction sign.

Umut Ozuguzel

UO

Electrochemistry

Balancing Redox Equations - Example 1

In chemistry, a redox reaction is a chemical reaction in which the oxidation states of the atoms of the participating elements are changed. Any such reaction involves both a reduction process and a complementary oxidation process, two key concepts involved with electron transfer processes. A redox reaction may be written with either an oxidation sign or a reduction sign.

Umut Ozuguzel

UO

Electrochemistry

Balancing Redox Equations - Example 2

In chemistry, a redox reaction is a chemical reaction in which the oxidation states of the atoms of the participating elements are changed. Any such reaction involves both a reduction process and a complementary oxidation process, two key concepts involved with electron transfer processes. A redox reaction may be written with either an oxidation sign or a reduction sign.

Umut Ozuguzel

UO

Electrochemistry

Balancing Redox Equations - Example 3

In chemistry, a redox reaction is a chemical reaction in which the oxidation states of the atoms of the participating elements are changed. Any such reaction involves both a reduction process and a complementary oxidation process, two key concepts involved with electron transfer processes. A redox reaction may be written with either an oxidation sign or a reduction sign.

Umut Ozuguzel

UO

Electrochemistry

Balancing Redox Equations - Example 4

In chemistry, a redox reaction is a chemical reaction in which the oxidation states of the atoms of the participating elements are changed. Any such reaction involves both a reduction process and a complementary oxidation process, two key concepts involved with electron transfer processes. A redox reaction may be written with either an oxidation sign or a reduction sign.

Umut Ozuguzel

UO

Electrochemistry

Standard Electrode Potentials - Overview

In chemistry, a standard electrode potential is the reference electrode potential for a half-cell reaction when the reaction involves a standard hydrogen electrode (SHE) and the standard reduction potential (E°) of the half-cell is known. The potential of the SHE is 0 V and the potential of the reduction reaction is the same as the E° of the reaction. The standard electrode potential is the potential difference between the SHE and the reduction reaction.

Umut Ozuguzel

UO

Electrochemistry

Standard Electrode Potentials - Example 1

In chemistry, a standard electrode potential is the reference electrode potential for a half-cell reaction when the reaction involves a standard hydrogen electrode (SHE) and the standard reduction potential (E°) of the half-cell is known. The potential of the SHE is 0 V and the potential of the reduction reaction is the same as the E° of the reaction. The standard electrode potential is the potential difference between the SHE and the reduction reaction.

Umut Ozuguzel

UO

Electrochemistry

Standard Electrode Potentials - Example 2

In chemistry, a standard electrode potential is the reference electrode potential for a half-cell reaction when the reaction involves a standard hydrogen electrode (SHE) and the standard reduction potential (E°) of the half-cell is known. The potential of the SHE is 0 V and the potential of the reduction reaction is the same as the E° of the reaction. The standard electrode potential is the potential difference between the SHE and the reduction reaction.

Umut Ozuguzel

UO

Electrochemistry

Predicting Spontaneousity - Overview

In physics, spontaneity is the tendency of a physical process to occur without intervention by any external force. The concept is distinct from that of thermodynamic free energy, which is a function of the state of a system.

Umut Ozuguzel

UO

Electrochemistry

Cell Potential Free Energy And Equilibrium Constant- Overview

The equilibrium constant (more precisely, the equilibrium constant for a chemical reaction) is the constant that describes the tendency of a chemical reaction to go to completion, that is, to reach equilibrium. The equilibrium constant is the ratio of products to reactants at equilibrium.

Umut Ozuguzel

UO

Electrochemistry

Cell Potential Free Energy And Equilibrium Constant - Example 1

In chemistry, the Gibbs free energy (G) is a thermodynamic potential that measures the "available" energy in a system. It is the maximum amount of non-enthalpy work that can be performed at constant temperature and pressure. It is named after the American scientist Josiah Willard Gibbs. The Gibbs free energy is a thermodynamic potential that measures the "available" energy in a system. It is the maximum amount of non-enthalpy work that can be performed at constant temperature and pressure. It is named after the American scientist Josiah Willard Gibbs.

Umut Ozuguzel

UO

Electrochemistry

Cell Potential Free Energy And Equilibrium Constant - Example 2

In chemistry, the Gibbs free energy (G) is a thermodynamic potential that measures the "available" energy in a system. It is the maximum amount of non-enthalpy work that can be performed at constant temperature and pressure. It is named after the American scientist Josiah Willard Gibbs. The Gibbs free energy is a thermodynamic potential that measures the "available" energy in a system. It is the maximum amount of non-enthalpy work that can be performed at constant temperature and pressure. It is named after the American scientist Josiah Willard Gibbs.

Umut Ozuguzel

UO

Electrochemistry

Cell Potential And Concentration - Overview

In biology, potential difference is a difference in electric potential between two points, measured relative to a common reference point.

Umut Ozuguzel

UO

Electrochemistry

Cell Potential And Concentration - Example 1

In biology, potential difference is a difference in electric potential between two points, measured relative to a common reference point.

Umut Ozuguzel

UO

Electrochemistry

Cell Potential And Concentration - Example 2

In biology, potential difference is a difference in electric potential between two points, measured relative to a common reference point.

Umut Ozuguzel

UO

Electrochemistry

Stoichiometry Of Electrolysis - Overview

In chemistry, a stoichiometric quantity is a chemical quantity that is expressed as the ratio of a small number of entities to another small number of entities. In a chemical reaction, reactants are used up to the point where they are completely converted to products. The mass of a reactant used is a mass in grams, the volume of a reactant used is a volume in liters, and the mole of a reactant used is the number of moles. The mole is the amount of a substance that contains the same number of entities as there are atoms in 12 grams of carbon-12.

Umut Ozuguzel

UO

Electrochemistry

Stoichiometry Of Electrolysis - Example 1

In chemistry, a stoichiometric quantity is a chemical quantity that is expressed as the ratio of a small number of entities to another small number of entities. In a chemical reaction, reactants are used up to the point where they are completely converted to products. The mass of a reactant used is a mass in grams, the volume of a reactant used is a volume in liters, and the mole of a reactant used is the number of moles. The mole is the amount of a substance that contains the same number of entities as there are atoms in 12 grams of carbon-12.

Umut Ozuguzel

UO