a)
This is 1st order reaction.
So, rate law is:
Rate = k [C3H6]
2)
we have:
[C3H6]o = 0.100 M
t = 20 min = 20*60 s = 1200 s
k = 6.7*10^-4 s-1
use integrated rate law for 1st order reaction
ln[C3H6] = ln[C3H6]o - k*t
ln[C3H6] = ln(0.1) - 6.7*10^-4*1.2*10^3
ln[C3H6] = -2.303 - 6.7*10^-4*1.2*10^3
ln[C3H6] = -3.107
[C3H6] = e^(-3.107)
[C3H6] = 4.475*10^-2 M
Answer: 4.5*10^-2 M
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