Can anyone tell me how I can convert a rate constant derived from first order kinetics (units are $\mathrm{h^{-1}}$) into an actual rate (turnovers/h)?

The scenario is that I know my rate constant for a molecule degrading in solution and it is $0.012\ \mathrm{h^{-1}}$. I know that I have $10^{14}$ catalyst molecules in the solution. How can I translate that into a number of molecules converted per catalyst per hour?

  • 1
    $\begingroup$ What approaches have you considered so far? $\endgroup$
    – Curt F.
    Mar 10 '15 at 2:50
  • $\begingroup$ Okay, I think I have it. The key is to recognize that the rate constant in units of hr^-1 was for the entire solution, and I can just multiply the rate by the number of molecules that I start with and divide by the molecules of catalyst. Factor label method to the rescue! $\endgroup$
    – Coherent
    Mar 10 '15 at 4:34

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