we have:
[N2O5]o = 0.300 M
t = 10.0 min = 600 s
k = 5.96*10^-4 s-1
By seeing the unit of K, we can say that this is 1st order reaction.
use integrated rate law for 1st order reaction
ln[N2O5] = ln[N2O5]o - k*t
ln[N2O5] = ln(0.3) - 5.96*10^-4*6*10^2
ln[N2O5] = -1.204 - 5.96*10^-4*6*10^2
ln[N2O5] = -1.562
[N2O5] = e^(-1.562)
[N2O5] = 0.2098 M
Answer: 0.210 M
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