1. Static vs Dynamic Equilibrium: Static equilibrium refers to a state where all forces and torques are balanced, and the system is at rest. Dynamic equilibrium, on the other hand, refers to a state where the forward and reverse processes occur at the same rate, and the quantities such as pressure, temperature, and concentration of reactants and products remain unchanged over time.

2. Reversible vs Irreversible Reactions: Reversible reactions are those where the reactants form products, which subsequently react together to give the reactants back. This can be represented as A ⇌ B. Irreversible reactions are those where the reactants form products, and the reaction cannot go back, i.e., A → B.

3. Characteristics of Equilibrium State: At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction. The concentrations of reactants and products remain constant. The state of equilibrium is dynamic, not static. It is unaffected by the presence of a catalyst.

4. Equilibria Involving Physical Changes: Physical equilibria refer to the equilibrium systems where physical states can change, such as the melting of ice or the evaporation of water. The characteristics of these equilibria include the fact that they occur at a specific temperature for a given substance (e.g., boiling point, melting point) and that they involve a change in the physical state.

5. Homogeneous vs Heterogeneous Equilibrium: Homogeneous equilibrium refers to the equilibrium that involves reactants and products in the same phase. In contrast, heterogeneous equilibrium involves reactants and products in different phases.

6. Law of Mass Action: This law states that the rate of a chemical reaction is directly proportional to the product of the molar concentrations of the reactants, each raised to the power equal to its stoichiometric coefficient in the balanced chemical equation.

7. Application of the Law of Equilibrium: The law of equilibrium can be applied to write the expression of the equilibrium constant for different types of chemical reactions. For a homogeneous reaction, the equilibrium constant expression includes the concentrations of all reactants and products. For a heterogeneous reaction, the equilibrium constant expression includes only those substances that are in the gaseous phase or in solution.

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1. Static vs Dynamic Equilibrium: Static equilibrium refers to a state where all forces and torques are balanced, and the system is at rest. Dynamic equilibrium, on the other hand, refers to a state where the forward and reverse processes occur at the same rate, and the quantities such as pressure, temperature, and concentration of reactants and products remain unchanged over time.

2. Reversible vs Irreversible Reactions: Reversible reactions are those where the reactants form products, which subsequently react together to give the reactants back. This can be represented as A ⇌ B. Irreversible reactions are those where the reactants form products, and the reaction cannot go back, i.e., A → B.

3. Characteristics of Equilibrium State: At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction. The concentrations of reactants and products remain constant. The state of equilibrium is dynamic, not static. It is unaffected by the presence of a catalyst.

4. Equilibria Involving Physical Changes: Physical equilibria refer to the equilibrium systems where physical states can change, such as the melting of ice or the evaporation of water. The characteristics of these equilibria include the fact that they occur at a specific temperature for a given substance (e.g., boiling point, melting point) and that they involve a change in the physical state.

5. Homogeneous vs Heterogeneous Equilibrium: Homogeneous equilibrium refers to the equilibrium that involves reactants and products in the same phase. In contrast, heterogeneous equilibrium involves reactants and products in different phases.

6. Law of Mass Action: This law states that the rate of a chemical reaction is directly proportional to the product of the molar concentrations of the reactants, each raised to the power equal to its stoichiometric coefficient in the balanced chemical equation.

7. Application of the Law of Equilibrium: The law of equilibrium can be applied to write the expression of the equilibrium constant for different types of chemical reactions. For a homogeneous reaction, the equilibrium constant expression includes the concentrations of all reactants and products. For a heterogeneous reaction, the equilibrium constant expression includes only those substances that are in the gaseous phase or in solution.

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1. Static vs Dynamic Equilibrium: Static equilibrium refers to a state where all forces and torques are balanced, and the system is at rest. Dynamic equilibrium, on the other hand, refers to a state where the forward and reverse processes occur at the same rate, and the quantities such as pressure, temperature, and concentration of reactants and products remain unchanged over time.

2. Reversible vs Irreversible Reactions: Reversible reactions are those where the reactants form products, which subsequently react together to give the reactants back. This can be represented as A ⇌ B. Irreversible reactions are those where the reactants form products, and the reaction cannot go back, i.e., A → B.

3. Characteristics of Equilibrium State: At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction. The concentrations of reactants and products remain constant. The state of equilibrium is dynamic, not static. It is unaffected by the presence of a catalyst.

4. Equilibria Involving Physical Changes: Physical equilibria refer to the equilibrium systems where physical states can change, such as the melting of ice or the evaporation of water. The characteristics of these equilibria include the fact that they occur at a specific temperature for a given substance (e.g., boiling point, melting point) and that they involve a change in the physical state.

5. Homogeneous vs Heterogeneous Equilibrium: Homogeneous equilibrium refers to the equilibrium that involves reactants and products in the same phase. In contrast, heterogeneous equilibrium involves reactants and products in different phases.

6. Law of Mass Action: This law states that the rate of a chemical reaction is directly proportional to the product of the molar concentrations of the reactants, each raised to the power equal to its stoichiometric coefficient in the balanced chemical equation.

7. Application of the Law of Equilibrium: The law of equilibrium can be applied to write the expression of the equilibrium constant for different types of chemical reactions. For a homogeneous reaction, the equilibrium constant expression includes the concentrations of all reactants and products. For a heterogeneous reaction, the equilibrium constant expression includes only those substances that are in the gaseous phase or in solution.

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