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Chemical kinetics quantifies reaction rates: reaction rate = k[A]^m[B]^n, where k depends on temperature (Arrhenius).
Trinn-for-trinn guide
- 1Input initial concentrations, rate constant, order
- 2Calculate reaction progress over time
- 3Show concentration vs. time plots
Løste eksempler
Inndata
First-order reaction: ln[A] = ln[A₀] - kt
Resultat
Concentration decreases exponentially; half-life constant
Inndata
Second-order: 1/[A] = 1/[A₀] + kt
Resultat
Concentration decreases slowly at low values
Vanlige feil å unngå
- ✕Confusing reaction order with stoichiometry
- ✕Using wrong integrated rate law
Ofte stilte spørsmål
How do you determine reaction order?
Experimental data fitting or testing integrated rate laws.
Why temperature affects k so dramatically?
Exponential Arrhenius dependence: k = A·e^(-Ea/RT).
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