Equilibrium & Acid Reactions

These flashcards cover essential concepts and terminology related to equilibrium and acid reactions as discussed in the lecture.

Equilibrium

The state of equal and opposing rates of reactions in a closed system where concentrations of reactants and products remain constant.

Dynamic Equilibrium

A state of balance in which reactants are converted to products and vice versa at equal and constant rates.

Static Equilibrium

A state in which there is no exchange between reactants and products, with no forward or reverse reactions occurring.

Collision Theory

A theory stating that in order for a reaction to occur, molecules must collide with sufficient energy and correct orientation.

Gibbs Free Energy (ΔG)

A thermodynamic quantity that indicates whether a reaction can occur spontaneously; ΔG = 0 indicates equilibrium.

Enthalpy

The measure of energy change in a system due to bond breaking and forming, with exothermic reactions releasing energy (ΔH < 0) and endothermic reactions absorbing energy (ΔH > 0).

Entropy (ΔS)

The measure of disorder or randomness in a system, where high entropy (chaotic) is when moving from solids to gases.

Le Chatelier’s Principle

A principle stating that if a system at equilibrium is disturbed, the system will shift to minimize the disturbance and re-establish equilibrium.

Equilibrium Constant (Keq)

A constant that describes the ratio of the concentrations of products to reactants at equilibrium for a reversible reaction.

Rice Table

A table used to calculate the concentrations of reactants and products at equilibrium, showing Initial concentration, Change in concentration, and Equilibrium concentration.

Reaction Quotient (Q)

The ratio of product concentrations to reactant concentrations at any point in a reaction, used to predict the direction of a reaction shift relative to Keq.