chemistry / Reactions / free
Kinetics
Measure how quickly a reaction changes and what controls its pace.
Follow the cause1 / 3
Concentrations set encounter rates. Particles must meet, orient, and have enough energy for a productive event.
rate over timerate law · k 0.0355 s⁻¹
Focus the idea
order1
rate constant0.0355 s⁻¹
half-life19.5 s
temperature45 °C · 318 K
Order 1: t½ = ln2/k = 19.5 s with [A]₀ = 1 M. A first-order half-life is independent of starting concentration.
The curve is the ideal integrated rate law for A → products, with k = 0.010 (in the order's units) at 25 °C and Eₐ = 50 kJ/mol. A measured rate law must be inferred from data; stoichiometric coefficients do not automatically become reaction orders.
04 / PRACTICE
0 / 3 checkedMake the chemistry yours.
Answer from the model, then use the explanation to connect the particle picture to the chemical rule.
CHECK 1 / 3