a)
we have:
[A]o = 0.125 M
[A] = 1.52*10^-3 M
k = 0.385 h-1
use integrated rate law for 1st order reaction
ln[A] = ln[A]o - k*t
ln(1.52*10^-3) = ln(0.125) - 0.385*t
-6.489 = -2.079 - 0.385*t
0.385*t = 4.41
t = 11.45 h
Answer: 11.5 h
b)
we have:
[A]o = 0.125 M
t = 3.0 h
k = 0.385 h-1
use integrated rate law for 1st order reaction
ln[A] = ln[A]o - k*t
ln[A] = ln(0.125) - 0.385*3
ln[A] = -2.079 - 0.385*3
ln[A] = -3.234
[A] = e^(-3.234)
[A] = 3.938*10^-2 M
Answer: 3.94*10^-2 M
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