Page 2: Reaction Properties and Equilibrium Characteristics

This page focuses on the practical applications and interpretations of equilibrium constants and reaction quotients in determining reaction behavior.

Definition: A reaction is considered total when the constante d'équilibre k valeur exceeds 10⁴

Highlight: The relationship between quotient de réaction et k determines reaction direction:

• When Qr < K, reaction proceeds in forward direction
• When Qr > K, reaction proceeds in reverse direction
• When Qr = K, system is at equilibrium

Example: For acid-base equilibria, the concentration of H₃O⁺ can be calculated using the formula [H₃O⁺] = c·τ, where c is initial concentration and τ is the reaction progress variable

Vocabulary: τ (tau) represents the extent of reaction progress, measured as a fraction of initial concentration

Page 1: Understanding Reaction Quotients and Equilibrium Constants

This page introduces the fundamental concepts of reaction quotients and equilibrium constants in chemical systems. For a general reaction aA + bB ⟶ cC + dD, the reaction quotient is expressed using concentrations of products and reactants.

Definition: The quotient de réaction initial formule is defined as Qr = [C][D]/[A]ᵃ[B]ᵇ

Highlight: The equilibrium constant K equals the reaction quotient at equilibrium (K = Qr equilibrium)

Example: For acid-base reactions, K can be related to Ka and pKa through the formula K = 10⁻ᵖᴷᵃ

Vocabulary: Ka represents the acid dissociation constant, while pKa is its negative logarithm

The page also details special properties where solvents (typically water) and solid substances don't affect the reaction quotient calculations.