Chemical Equilibrium

The course starts with the introduction of equilibrium which is followed by describing solid-liquid equilibrium, liquid-vapor equilibrium and solid-vapor equilibrium. It then goes on to explain the law of chemical equilibrium and equilibrium constant which is followed by predicting the direction and extent of a reaction. The course also discusses how to express equilibrium constant in terms of pressure. The heterogeneous equilibria is also discussed which is followed by the method to calculate the equilibrium concentration. The course further discusses the relationship between equilibrium constant, reaction quotient and Gibbs energy. The course concludes by discussing Le Chatelier’s principle and the factors affecting equilibrium in detail.

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215 lectures

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Chemical Equilibrium

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Acids and Bases

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Aqueous Equilibria

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Electrochemistry

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Nuclear Chemistry

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Chemical Equilibrium Lectures

Chemical Equilibrium

Concept Of Equilibrium - Overview

In thermodynamics, a state of thermodynamic equilibrium is a state in which a system is in thermal equilibrium with its surroundings. A system in thermodynamic equilibrium is in thermal equilibrium, mechanical equilibrium, electrical equilibrium, and chemical equilibrium. A system is in equilibrium when it is in thermal equilibrium with its surroundings.

Umut Ozuguzel

UO

Chemical Equilibrium

Chemical Equilibrium - Intro

In chemistry, chemical equilibrium (also known as dynamic equilibrium) is a state of chemical stability in which the concentrations of the chemical substances do not change in the course of time due to their reaction with each other in a closed system. Chemical equilibrium is an example of dynamic equilibrium, a thermodynamic concept.

Umut Ozuguzel

UO

Chemical Equilibrium

Equilibrium Constant - Overview

In chemistry, the equilibrium constant, also called the equilibrium coefficient, is the constant of a chemical reaction that is a function of the concentrations of the chemical species involved in the reaction and their partial pressures, and that is used to predict the equilibrium concentrations of the products and reactants in the reaction at a given temperature. The equilibrium constant is usually denoted by the symbol K. The equilibrium constant is commonly defined as the ratio of the partial pressure of products to the partial pressure of reactants at equilibrium. The equilibrium constant is a generalization of the equilibrium expression for a single reaction, which is the ratio of the concentrations of products to that of the reactants.

Umut Ozuguzel

UO

Chemical Equilibrium

Equilibrium Constant - Example 1

In chemistry, the equilibrium constant, also called the equilibrium coefficient, is the constant of a chemical reaction that is a function of the concentrations of the chemical species involved in the reaction and their partial pressures, and that is used to predict the equilibrium concentrations of the products and reactants in the reaction at a given temperature. The equilibrium constant is usually denoted by the symbol K. The equilibrium constant is commonly defined as the ratio of the partial pressure of products to the partial pressure of reactants at equilibrium. The equilibrium constant is a generalization of the equilibrium expression for a single reaction, which is the ratio of the concentrations of products to that of the reactants.

Umut Ozuguzel

UO

Chemical Equilibrium

Equilibrium Constant - Example 2

In chemistry, the equilibrium constant, also called the equilibrium coefficient, is the constant of a chemical reaction that is a function of the concentrations of the chemical species involved in the reaction and their partial pressures, and that is used to predict the equilibrium concentrations of the products and reactants in the reaction at a given temperature. The equilibrium constant is usually denoted by the symbol K. The equilibrium constant is commonly defined as the ratio of the partial pressure of products to the partial pressure of reactants at equilibrium. The equilibrium constant is a generalization of the equilibrium expression for a single reaction, which is the ratio of the concentrations of products to that of the reactants.

Umut Ozuguzel

UO

Chemical Equilibrium

Equilibrium Constant - Example 3

In chemistry, the equilibrium constant, also called the equilibrium coefficient, is the constant of a chemical reaction that is a function of the concentrations of the chemical species involved in the reaction and their partial pressures, and that is used to predict the equilibrium concentrations of the products and reactants in the reaction at a given temperature. The equilibrium constant is usually denoted by the symbol K. The equilibrium constant is commonly defined as the ratio of the partial pressure of products to the partial pressure of reactants at equilibrium. The equilibrium constant is a generalization of the equilibrium expression for a single reaction, which is the ratio of the concentrations of products to that of the reactants.

Umut Ozuguzel

UO

Chemical Equilibrium

Equilibrium Constant - Example 4

In chemistry, the equilibrium constant, also called the equilibrium coefficient, is the constant of a chemical reaction that is a function of the concentrations of the chemical species involved in the reaction and their partial pressures, and that is used to predict the equilibrium concentrations of the products and reactants in the reaction at a given temperature. The equilibrium constant is usually denoted by the symbol K. The equilibrium constant is commonly defined as the ratio of the partial pressure of products to the partial pressure of reactants at equilibrium. The equilibrium constant is a generalization of the equilibrium expression for a single reaction, which is the ratio of the concentrations of products to that of the reactants.

Umut Ozuguzel

UO

Chemical Equilibrium

Expressing Equilibrium Constant In Terms Of Pressure - Overview

In chemistry, a reaction is said to be at equilibrium when the concentrations of the reactants and products do not change with the passing of time. At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction. The forward and backward reactions are said to be in chemical equilibrium when the rates of the forward and backward reactions are equal.

Umut Ozuguzel

UO

Chemical Equilibrium

Expressing Equilibrium Constant In Terms Of Pressure - Example 1

In chemistry, a reaction is said to be at equilibrium when the concentrations of the reactants and products do not change with the passing of time. At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction. The forward and backward reactions are said to be in chemical equilibrium when the rates of the forward and backward reactions are equal.

Umut Ozuguzel

UO

Chemical Equilibrium

Expressing Equilibrium Constant In Terms Of Pressure - Example 2

In chemistry, a reaction is said to be at equilibrium when the concentrations of the reactants and products do not change with the passing of time. At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction. The forward and backward reactions are said to be in chemical equilibrium when the rates of the forward and backward reactions are equal.

Umut Ozuguzel

UO

Chemical Equilibrium

Expressing Equilibrium Constant In Terms Of Pressure - Example 3

In chemistry, a reaction is said to be at equilibrium when the concentrations of the reactants and products do not change with the passing of time. At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction. The forward and backward reactions are said to be in chemical equilibrium when the rates of the forward and backward reactions are equal.

Umut Ozuguzel

UO

Chemical Equilibrium

Expressing Equilibrium Constant In Terms Of Pressure - Example 4

In chemistry, a reaction is said to be at equilibrium when the concentrations of the reactants and products do not change with the passing of time. At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction. The forward and backward reactions are said to be in chemical equilibrium when the rates of the forward and backward reactions are equal.

Umut Ozuguzel

UO

Chemical Equilibrium

Heterogeneous Equilibria - Overview

In thermodynamics, a heterogeneous equilibrium is an equilibrium state that involves a phase change of the system. In such an equilibrium, the system is not in thermal equilibrium with its surroundings; that is, the system is at a temperature different from that of the surroundings.

Umut Ozuguzel

UO

Chemical Equilibrium

Heterogeneous Equilibria - Example 1

In thermodynamics, a heterogeneous equilibrium is an equilibrium state that involves a phase change of the system. In such an equilibrium, the system is not in thermal equilibrium with its surroundings; that is, the system is at a temperature different from that of the surroundings.

Umut Ozuguzel

UO

Chemical Equilibrium

Calculating The Equibrium Constant - Overview

The equilibrium constant is a quantitative measure of the tendency of a chemical reaction to move towards chemical equilibrium. It is the constant for a reaction in which the reactants and products are in chemical equilibrium with each other.

Umut Ozuguzel

UO

Chemical Equilibrium

Calculating The Equilibrium Constant - Example 1

The equilibrium constant, also known as the constant of proportionality, is the constant of proportionality in the equilibrium expression. The equilibrium constant is the equilibrium constant for a chemical reaction, which is the quotient of the concentrations of products over the concentrations of reactants. The equilibrium constant is a special case of the equilibrium constant for a chemical reaction, which is the quotient of the concentrations of products over the concentrations of reactants. The equilibrium constant is a special case of the equilibrium constant for a chemical reaction, which is the quotient of the concentrations of products over the concentrations of reactants. The equilibrium constant is a special case of the equilibrium constant for a chemical reaction, which is the quotient of the concentrations of products over the concentrations of reactants.

Umut Ozuguzel

UO

Chemical Equilibrium

Calculating The Equilibrium Constant - Example 2

The equilibrium constant, also known as the constant of proportionality, is the constant of proportionality in the equilibrium expression. The equilibrium constant is the equilibrium constant for a chemical reaction, which is the quotient of the concentrations of products over the concentrations of reactants. The equilibrium constant is a special case of the equilibrium constant for a chemical reaction, which is the quotient of the concentrations of products over the concentrations of reactants. The equilibrium constant is a special case of the equilibrium constant for a chemical reaction, which is the quotient of the concentrations of products over the concentrations of reactants. The equilibrium constant is a special case of the equilibrium constant for a chemical reaction, which is the quotient of the concentrations of products over the concentrations of reactants.

Umut Ozuguzel

UO

Chemical Equilibrium

Reaction Quotient - Overview

In organic chemistry, the reaction quotient or reaction-rate quotient is an equilibrium constant expression that relates the concentrations of reactants and products to the equilibrium constant for the reaction. It is usually denoted by the symbol Q, and is equal to the equilibrium constant for the reaction divided by the product of the concentrations of the reactants.

Umut Ozuguzel

UO

Chemical Equilibrium

Reaction Quotient - Example 1

In organic chemistry, the reaction quotient or reaction-rate quotient is an equilibrium constant expression that relates the concentrations of reactants and products to the equilibrium constant for the reaction. It is usually denoted by the symbol Q, and is equal to the equilibrium constant for the reaction divided by the product of the concentrations of the reactants.

Umut Ozuguzel

UO

Chemical Equilibrium

Reaction Quotient - Example 2

In organic chemistry, the reaction quotient or reaction-rate quotient is an equilibrium constant expression that relates the concentrations of reactants and products to the equilibrium constant for the reaction. It is usually denoted by the symbol Q, and is equal to the equilibrium constant for the reaction divided by the product of the concentrations of the reactants.

Umut Ozuguzel

UO

Chemical Equilibrium

Reaction Quotient - Example 3

In organic chemistry, the reaction quotient or reaction-rate quotient is an equilibrium constant expression that relates the concentrations of reactants and products to the equilibrium constant for the reaction. It is usually denoted by the symbol Q, and is equal to the equilibrium constant for the reaction divided by the product of the concentrations of the reactants.

Umut Ozuguzel

UO

Chemical Equilibrium

Finding Equilibrium Concentrations - Overview

In chemistry, chemical equilibrium is an equivalence of opposing chemical reactions, in which the forward and backward reactions proceed at the same rate. The chemical equilibrium of a system can be disturbed by changes such as the addition of a catalyst or by the separation of the mixture into its components. At equilibrium, the concentrations of products and reactants no longer change with time (they are said to be "constant"); the system is said to be "in chemical equilibrium". Chemical equilibrium is an example of dynamic equilibrium, in which the concentrations of the reactants and products do not change with time.

Umut Ozuguzel

UO

Chemical Equilibrium

Finding Equilibrium Concentrations - Example 1

In chemistry, chemical equilibrium is an equivalence of opposing chemical reactions, in which the forward and backward reactions proceed at the same rate. The chemical equilibrium of a system can be disturbed by changes such as the addition of a catalyst or by the separation of the mixture into its components. At equilibrium, the concentrations of products and reactants no longer change with time (they are said to be "constant"); the system is said to be "in chemical equilibrium". Chemical equilibrium is an example of dynamic equilibrium, in which the concentrations of the reactants and products do not change with time.

Umut Ozuguzel

UO

Chemical Equilibrium

Finding Equilibrium Concentrations - Example 2

In chemistry, chemical equilibrium is an equivalence of opposing chemical reactions, in which the forward and backward reactions proceed at the same rate. The chemical equilibrium of a system can be disturbed by changes such as the addition of a catalyst or by the separation of the mixture into its components. At equilibrium, the concentrations of products and reactants no longer change with time (they are said to be "constant"); the system is said to be "in chemical equilibrium". Chemical equilibrium is an example of dynamic equilibrium, in which the concentrations of the reactants and products do not change with time.

Umut Ozuguzel

UO

Chemical Equilibrium

Finding Equilibrium Concentrations - Example 3

In chemistry, chemical equilibrium is an equivalence of opposing chemical reactions, in which the forward and backward reactions proceed at the same rate. The chemical equilibrium of a system can be disturbed by changes such as the addition of a catalyst or by the separation of the mixture into its components. At equilibrium, the concentrations of products and reactants no longer change with time (they are said to be "constant"); the system is said to be "in chemical equilibrium". Chemical equilibrium is an example of dynamic equilibrium, in which the concentrations of the reactants and products do not change with time.

Umut Ozuguzel

UO

Chemical Equilibrium

Finding Equilibrium Concentrations - Example 4

In chemistry, chemical equilibrium is an equivalence of opposing chemical reactions, in which the forward and backward reactions proceed at the same rate. The chemical equilibrium of a system can be disturbed by changes such as the addition of a catalyst or by the separation of the mixture into its components. At equilibrium, the concentrations of products and reactants no longer change with time (they are said to be "constant"); the system is said to be "in chemical equilibrium". Chemical equilibrium is an example of dynamic equilibrium, in which the concentrations of the reactants and products do not change with time.

Umut Ozuguzel

UO

Chemical Equilibrium

Simplifying Approximations - Overview

In mathematics, an approximation is a calculation that is a close representation of the value of the desired result. The value may be an exact value or an upper or lower bound to the true value. Approximations are often used in physics and engineering, and also in mathematics.

Umut Ozuguzel

UO

Chemical Equilibrium

Simplifying Approximations - Example 1

In mathematics, an approximation is a calculation that is a close representation of the value of the desired result. The value may be an exact value or an upper or lower bound to the true value. Approximations are often used in physics and engineering, and also in mathematics.

Umut Ozuguzel

UO

Chemical Equilibrium

Simplifying Approximations - Example 2

In mathematics, an approximation is a calculation that is a close representation of the value of the desired result. The value may be an exact value or an upper or lower bound to the true value. Approximations are often used in physics and engineering, and also in mathematics.

Umut Ozuguzel

UO

Chemical Equilibrium

Le Chateliers Principle - Overview

The Le Châtelier's principle states that if a dynamic system at equilibrium experiences a change in concentration of one of its reactants, the equilibrium shifts in the direction that tends to diminish that change. This is a general principle of all dynamic systems at equilibrium, including chemical systems. The principle is named after the French chemist Henry Louis Le Châtelier (1850–1936), who expressed it in 1887.

Umut Ozuguzel

UO

Chemical Equilibrium

Le Chateliers Principle - Example 1

The Le Châtelier's principle states that if a dynamic system at equilibrium experiences a change in concentration of one of its reactants, the equilibrium shifts in the direction that tends to diminish that change. This is a general principle of all dynamic systems at equilibrium, including chemical systems. The principle is named after the French chemist Henry Louis Le Châtelier (1850–1936), who expressed it in 1887.

Umut Ozuguzel

UO

Chemical Equilibrium

Le Chateliers Principle - Example 2

The Le Châtelier's principle states that if a dynamic system at equilibrium experiences a change in concentration of one of its reactants, the equilibrium shifts in the direction that tends to diminish that change. This is a general principle of all dynamic systems at equilibrium, including chemical systems. The principle is named after the French chemist Henry Louis Le Châtelier (1850–1936), who expressed it in 1887.

Umut Ozuguzel

UO

Chemical Equilibrium

Le Chateliers Principle - Example 3

The Le Châtelier's principle states that if a dynamic system at equilibrium experiences a change in concentration of one of its reactants, the equilibrium shifts in the direction that tends to diminish that change. This is a general principle of all dynamic systems at equilibrium, including chemical systems. The principle is named after the French chemist Henry Louis Le Châtelier (1850–1936), who expressed it in 1887.

Umut Ozuguzel

UO

Chemical Equilibrium

Le Chateliers Principle - Example 4

The Le Châtelier's principle states that if a dynamic system at equilibrium experiences a change in concentration of one of its reactants, the equilibrium shifts in the direction that tends to diminish that change. This is a general principle of all dynamic systems at equilibrium, including chemical systems. The principle is named after the French chemist Henry Louis Le Châtelier (1850–1936), who expressed it in 1887.

Umut Ozuguzel

UO