Given:
Half life = 4.5 days
use relation between rate constant and half life of 1st order reaction
k = (ln 2) / k
= 0.693/(half life)
= 0.693/(4.5)
= 0.154 days-1
we have:
[A]o = 49 mg
t = 54.0 days
k = 0.154 days-1
use integrated rate law for 1st order reaction
ln[A] = ln[A]o - k*t
ln[A] = ln(49) - 0.154*54
ln[A] = 3.892 - 0.154*54
ln[A] = -4.424
[A] = e^(-4.424)
[A] = 1.198*10^-2 mg
Answer: 1.2*10^-2 mg
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