Key Concepts
- Rate of Reaction: The change in concentration of a reactant or product per unit time.
- Rate Law: An equation that relates the rate of a reaction to the concentrations of the reactants.
- Order of Reaction: The sum of the exponents of the concentration terms in the rate law.
- Rate Constant (k): A proportionality constant that relates the rate of a reaction to the concentrations of the reactants.
- Molecularity: The number of molecules or ions involved in an elementary reaction.
- Half-Life: The time required for the concentration of a reactant to decrease to half its initial value.
- Activation Energy (Ea): The minimum energy required for a reaction to occur.
- Arrhenius Equation: Relates the rate constant to the activation energy and temperature.
- Catalyst: A substance that increases the rate of a reaction without being consumed.
- Enzyme Kinetics: The study of the rates of enzyme-catalyzed reactions.
Formulas
- Rate Law: Rate = k[A]^m[B]^n
- Arrhenius Equation: k = Ae^(-Ea/RT)
- Half-Life for a First-Order Reaction: t1/2 = 0.693/k
Factors Affecting Reaction Rate
- Concentration of Reactants: Higher concentration, faster rate.
- Temperature: Higher temperature, faster rate.
- Surface Area: Greater surface area, faster rate (for heterogeneous reactions).
- Catalyst: Presence of a catalyst, faster rate.
- Pressure: For gaseous reactions, higher pressure, faster rate.
Integrated Rate Laws
- Zero-Order: [A] = [A]₀ - kt
- First-Order: ln[A] = ln[A]₀ - kt
- Second-Order: 1/[A] = 1/[A]₀ + kt
Reaction Mechanisms
- Elementary Reactions: Reactions that occur in a single step.
- Rate-Determining Step: The slowest step in a reaction mechanism.
- Intermediate: A species that is formed and consumed during a reaction.
Additional Topics
- Collision Theory: A theory that explains reaction rates based on the collisions between molecules.
- Transition State Theory: A theory that explains reaction rates based on the formation of a high-energy intermediate.
- Enzyme Kinetics: Michaelis-Menten equation, Lineweaver-Burk plot.
Note: This is a brief overview. For a more in-depth understanding, refer to your textbook or consult with your teacher.
