Kinetics, Equilibrium, and Thermodynamics Review

Flashcards covering kinetics, equilibrium, and thermodynamics concepts.

Activation Energy (Ea)

The minimum energy required for a reaction to occur; the energy barrier from reactants to products.

Arrhenius Equation

k = Ae^(-Ea/RT); Relates the rate constant (k) to temperature.

Frequency Factor (A)

In the Arrhenius equation, includes collision frequency and other factors influencing reaction rate.

Exponential Factor (e^(-Ea/RT))

The fraction of molecules with enough energy to overcome the activation barrier.

Reaction Coordinate Diagram

Illustrates the energy changes during a reaction from reactants to products, including the transition state.

Transition State

The highest energy point on the reaction coordinate diagram; an intermediate state between reactants and products.

Rate-Limiting Step

The slowest step in a reaction mechanism, reflected by a large activation energy on the reaction coordinate diagram.

Exergonic Reaction

A reaction with a negative change in Gibbs Free Energy (ΔG), favoring product formation (K > 1).

Endergonic Reaction

A reaction with a positive change in Gibbs Free Energy (ΔG), favoring reactant formation (K < 1).

van't Hoff Equation

ln(K) = -ΔH/RT + ΔS/R; Relates the equilibrium constant (K) to temperature and enthalpy change (ΔH).