Rate equations

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Sara

Cards (10)

  • Rate =Rate\ = K [A]m[B]n\ K\ \left[A\right]^m\left[B\right]^n

    K=rate constant
    m and n = order of the reactions
  • m + n = overall order of the reaction
  • Zero order

    As concentration changes, rate doesn’t change
  • First order

    If concentration doubles, rate will double.
    Rate is directly proportional to concentration
  • Second order

    If concentration doubles, rate will increase by a factor of 4.
    Rate is proportional to concentration squared
  • Rate concentration graphs
  • Concentration time graph
  • Rate determining step

    • slowest step
    • Overall rate is determined by the slowest step
  • Arrhenius equation

    K =K\ = Ae−EaRT\ Ae\frac{-Ea}{RT}
    K = rate constant
    A = Arrhenius constant, Pre exponential factor
    Ea = activation energy (j)
    R = Gas constant
    T = temperature (k)
  • ln⁡K =\ln K\ = ln⁡A − EaRT\ \ln A\ -\ \frac{Ea}{RT}