Definition: Le Chatelier's Principle states that when a system at equilibrium experiences a change, it will adjust to counteract that change.

Example: In a reaction A+B⇌C+D, adding more reactants (A or B) causes the equilibrium to shift right, while adding more products (C or D) causes it to shift left.

Highlight: Equilibrium shifts are described directionally - "to the right" indicates favoring product formation, while "to the left" indicates favoring reactant formation.

Vocabulary: An equilibrium shift refers to the system's response to changes in concentration, adjusting the relative amounts of reactants and products.

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.