Kinetics
Eleven topics on how fast reactions go and why. Reaction rates and the rate laws found from experiment, how concentration changes over time, the collision model and energy profiles behind a reaction, the step-by-step mechanisms that set the rate law, and how a catalyst speeds things up.
Topics
Equations For every problem in this unit
Rate
the change in concentration per unit time (a slope)
Rate law
rate = k[A]m[B]n (orders from experiment, not coefficients)
Integrated laws
zero: [A] linear; first: ln[A] linear; second: 1/[A] linear
Elementary step
a single molecular event; molecularity gives its rate law
Mechanism
elementary steps that sum to the overall reaction
Rate-determining step
the slowest step controls the rate; derive the rate law from it, eliminating any intermediates
Activation energy
Ea: the barrier from reactants to the transition state
Successful collision
enough energy (≥ Ea) AND the correct orientation
Catalyst
lowers Ea via a new path; does not change ΔH or equilibrium
Unit 1 tools
Challenge bank
60 open-ended problems.
Read the question, work it out, then flip the card to compare your reasoning to the worked solution. Mark each card so you can return to the ones that still bite.
Question
Tap card to reveal explanation
Worked solution
Tap card to return to question
Nothing here yet.
Switch to All, work through some cards, and tag them as Got it or Revisit.
Cumulative assessment
Test the unit.
Twenty mixed items pulled from across all 11 topics. Identifies which misconceptions still bite when you cannot see which topic the question came from.
20questions
11topics
16codes covered