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The rate constant for a certain reaction is k = 5.90x10-3 s1 If the initial reactant concentration was 0.250 M, what will the
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Answer #1

we have:

[A]o = 0.25 M

t = 4.00 min = 4*60 s = 240.0 s

k = 5.9*10^-3 s-1

use integrated rate law for 1st order reaction

ln[A] = ln[A]o - k*t

ln[A] = ln(0.25) - 5.9*10^-3*2.4*10^2

ln[A] = -1.386 - 5.9*10^-3*2.4*10^2

ln[A] = -2.802

[A] = e^(-2.802)

[A] = 6.067*10^-2 M

Answer: 6.07*10^-2 M

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