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ln[A] = ln[A] 0 - kt

0.88 M. ln. The reaction 2A B is first order in A, with a rate constant of 2.8 x 10 -2 s -1 at 80 0 C. How long will it take for the concentration in A to decrease from 0.88 M to 0.14 M ?. 0.14 M. =. 2.8 x 10 -2 s -1. ln. ln[A] 0 – ln[A]. =. k. k. [A] 0. [A].

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ln[A] = ln[A] 0 - kt

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  1. 0.88 M ln The reaction 2A B is first order in A, with a rate constant of 2.8 x 10-2 s-1 at 800C. How long will it take for the concentration in A to decrease from 0.88 M to 0.14 M ? 0.14 M = 2.8 x 10-2 s-1 ln ln[A]0 – ln[A] = k k [A]0 [A] [A]0 = 0.88 M ln[A] = ln[A]0 - kt [A] = 0.14 M kt = ln[A]0 – ln[A] = 66 s t =

  2. What is the half life of N2O5 , if it decomposes with a rate constant of 5.7 x 10-4 s-1? = t½ ln2 0.693 = k 5.7 x 10-4 s-1 = 1216 s = 20 minutos But.. How do we know the decomposition is first order? Because of the units of k: (s-1)

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