Chemistry - Chemical Kinetics Question with Solution | TestHub

The unit of the rate constant (${\mathrm{s}}^{-1}$) indicates that the reaction is of the first order.

The rate law for the first-order reaction is given by:

$\text{Rate}=k[{\mathrm{N}}_2{\mathrm{O}}_5]$

Given:

$\text{Rate}=1.02\times 10^{-4}\mathrm{mol}{\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$

$k=3.4\times 10^{-5}{\mathrm{s}}^{-1}$

Substituting the given values into the rate law:

$1.02\times 10^{-4}=3.4\times 10^{-5}\times [{\mathrm{N}}_2{\mathrm{O}}_5]$

$[{\mathrm{N}}_2{\mathrm{O}}_5]=\frac{1.02\times 10^{-4}}{3.4\times 10^{-5}}$

$[{\mathrm{N}}_2{\mathrm{O}}_5]=\frac{10.2\times 10^{-5}}{3.4\times 10^{-5}}=3.0\mathrm{mol}{\mathrm{L}}^{-1}$

Answer: $3.0\mathrm{mol}{\mathrm{L}}^{-1}$