R2.2
How Fast? The Rate of Chemical Change
Collision theory, factors affecting rate, and rate equations.
R2.2.1 Collision Theory & Rate
What makes reactions go faster?
→R2.2.2 Factors Affecting Rate
Temperature, concentration, catalysts, surface area.
→R2.2.3 Measuring Rate
Experimental methods and rate-time graphs.
→R2.2.4 Rate Equations & Arrhenius (HL)
Rate = k[A]ᵐ[B]ⁿ and the Arrhenius equation.
→R2.2.5 Catalysts
Energy profiles, Maxwell-Boltzmann, and how catalysts work.
→HL EXTENSION
R2.2.6 Rate Expressions
The rate law, the rate constant k, and its units.
→R2.2.7 Reaction Orders
Zero, first, and second order effects on rate.
→R2.2.8 Determining Orders
Method of initial rates from experimental data.
→R2.2.9 [A]-Time Graphs
Concentration-time curves for each order.
→R2.2.10 Rate-[A] Graphs
Rate-concentration plots and common mistakes.
→R2.2.11 Half-Life
Constant half-life for first-order reactions.
→R2.2.12 Arrhenius Equation
k = Ae^(-Ea/RT), Arrhenius plots, finding Ea.
→R2.2.13 Reaction Mechanisms
RDS, molecularity, and relating mechanisms to rate laws.
→Flashcards
Review key definitions and concepts with interactive flashcards.