PHYSICAClass 12 Chemistry simulations · Chemical Kinetics
Order of reaction and half-life
Compare how the concentration of a reactant falls for zero-, first- and second-order reactions.
What to notice
Only for a first-order reaction is the half-life independent of the starting concentration.
Key relation
zero: [A] = [A]₀ − kt ; first: [A] = [A]₀e^(−kt), t½ = 0.693/k ; second: 1/[A] = 1/[A]₀ + kt
Try this
Double [A]₀ for each order and see what happens to t½.
What you can change
- Order: 0 to 2
- Rate constant k: 0.01 to 0.5
- [A]₀: 0.2 to 2 M
- Time: 0 to 60 s
More in Chemical Kinetics
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