1. Tardigrade
  2. Question
  3. Chemistry
  4. Gaseous N2O5 decomposes according to the following equation: N2O5(g)→2NO2(g)+(1/2)O2(g) The experimental rate law is-Δ[N2O5]/Δ t=k[N2O5] At a certain temperature the rate constant is k = 5.0 × 10-4 sec-1. In how seconds will the concentration of N2O5 decrease to one-tenth of its initial value?

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Q. Gaseous $N_2O_5$ decomposes according to the following equation:
$N_{2}O_{5}\left(g\right)\to2NO_{2}\left(g\right)+\frac{1}{2}O_{2}\left(g\right)$
The experimental rate law is$-\Delta\left[N_{2}O_{5}\right]/\Delta t=k\left[N_{2}O_{5}\right]$
At a certain temperature the rate constant is $k = 5.0 \times 10^{-4} sec^{-1}$. In how seconds will the concentration of $N_2O_5$ decrease to one-tenth of its initial value?

Chemical Kinetics

Solution:

$t=\frac{2.303}{5\times10^{-4}} log\frac{A_{0}}{A_{0}/10}=4.6\times10^{3}sec$