Chemical Equilibrium Lecture Notes

A series of flashcards focused on the vocabulary and key concepts related to chemical equilibrium as covered in the lecture.

Dynamic Equilibrium

A condition where the forward and reverse reactions occur at equal rates, leading to constant concentrations of reactants and products.

Equilibrium Constant (K)

A constant that measures the relative amounts of products and reactants present at equilibrium, specific to a reaction at a given temperature.

Reaction Quotient (Q)

A measure of the relative amounts of products and reactants present at any given time during a reaction.

Homogeneous Equilibrium

An equilibrium system where all reactants and products are in the same phase (gas, liquid, etc.).

Heterogeneous Equilibrium

An equilibrium system where reactants and products exist in different phases.

Le Châtelier’s Principle

The principle stating that if a dynamic equilibrium is disturbed, the system will respond to counteract the disturbance and restore equilibrium.

Reversible Reaction

A reaction that can proceed in both forward and reverse directions.

K >> 1

Indicates that at equilibrium, there are significantly more products than reactants.

K << 1

Indicates that at equilibrium, there are significantly more reactants than products.

Changes in Concentration

Altering the concentration of reactants or products will shift the equilibrium to the side that opposes the change.

Catalysts and Equilibrium

A catalyst speeds up the rate of both the forward and reverse reactions without affecting the position of the equilibrium.

Kc vs Kp

Kc is the equilibrium constant based on concentrations (molarity), while Kp is based on partial pressures.

Temperature and Equilibrium Constant

Changing the temperature will alter the value of the equilibrium constant (K) for a reaction.

Volume Change on Gas Phase Reactions

Changes in volume affect gas-phase reactions; shifting toward the side with fewer gas molecules reduces pressure.

ICE Table

A table used to calculate the concentrations of reactants and products at equilibrium (Initial, Change, Equilibrium).

Equilibrium Expression

An equation that relates the concentrations of products and reactants at equilibrium in terms of K.

Kc Expression

The ratio of products to reactants, each raised to the power of their coefficients in a balanced equation.