Dynamic Equilibrium

Dynamic Equilibrium

Introduction:

• Dynamic equilibrium is a concept in chemistry that describes the balance between two opposing reactions occurring simultaneously within a closed system.
• To fully understand dynamic equilibrium, we can break it down into two key components: "Dynamic" and "Equilibrium".

Dynamic

• The term "dynamic" implies that the forward and reverse reactions of a chemical process are continuously happening.
• In dynamic equilibrium, these reactions never cease; they occur simultaneously.

Equilibrium

• "Equilibrium" refers to a specific point in a chemical reaction where the rate of the forward reaction is equal to the rate of the reverse reaction.
• When this balance is achieved, the reaction is said to have reached equilibrium.

Characteristics of Dynamic Equilibrium

• At equilibrium, the concentrations of both reactants and products remain constant.
• It's important to note that the concentrations of reactants and products may not necessarily be equal; their values depend on the specific reaction and conditions.
• The reaction mixture at equilibrium contains both reactants and products, and the reactions continue without any overall change in the concentrations.

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Dynamic Equilibrium

Example: Iron (III) Ions with Thiocyanate Ions

• Consider the reaction between iron (III) ions (Fe³⁺) and thiocyanate ions (CNS⁻).
• Fe³⁺(aq) + CNS⁻(aq) ⇌ FeCNS²⁺(aq)
• In this example, pale yellow iron (III) ions react with colourless thiocyanate ions.
• At equilibrium, the concentrations of Fe³⁺, CNS⁻, and FeCNS²⁺ remain constant, maintaining a dynamic balance between the forward and reverse reactions.

Conclusion: