General Chemistry Lecture 1 - Key Concepts

Flashcards covering key concepts from the first lecture on General Chemistry, focusing on chemical equilibrium and related principles.

Chemical Equilibrium

A dynamic process in which concentrations of reactants and products remain constant over time.

Equilibrium Constant (K)

A unitless value of the ratio of concentration (or partial pressure) terms at a specific temperature.

Dynamic Balance

A state in which the forward and reverse reactions occur at the same rate, maintaining constant concentrations.

Law of Mass Action

The ratio of concentrations or partial pressures of products to reactants at equilibrium has a characteristic value at a given temperature.

Le Châtelier’s Principle

If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.

Heterogeneous Equilibria

Equilibria involving reactants and products that are in different phases (e.g., solid, liquid, gas).

Equilibrium Expression

A mathematical expression that relates the concentrations or partial pressures of the reactants and products at equilibrium.

Reaction Quotient (Q)

A ratio used to determine the direction of a reaction at any point in time, compared to the equilibrium constant.

Chemical Kinetics

The study of the rates of chemical reactions and the factors affecting them.

Acid-Base Equilibria

The balance between the dissociation of acids and bases in solution.