Understanding Chemical Equilibrium

This page explores the fundamental concepts of chemical equilibrium in closed systems. The content explains how reversible reactions reach a balance point when conditions remain unchanged.

Definition: Dynamic equilibrium occurs when the rate of forward reaction equals the rate of reverse reaction in a closed system, resulting in constant concentrations of reactants and products.

Vocabulary: A closed system is an environment where reactants and products cannot escape, allowing for true equilibrium to be established.

Example: The concentration versus time graph demonstrates how reactant concentrations decrease while product concentrations increase until reaching equilibrium, where both remain constant.

Highlight: At equilibrium, the reaction has not stopped - rather, it continues in both directions at equal rates, maintaining constant concentrations.