Chemistry - Chemical Kinetics Question with Solution | TestHub

From the unit of the rate constant (${\text{s}}^{-1}$), we can determine that the given reaction is a first-order reaction.

For a first-order reaction, the rate law is expressed as:
$\text{Rate}=k[{\text{N}}_2{\text{O}}_5]$

Given values are:
$\text{Rate}=2.4\times 10^{-5}{\text{ mole L}}^{-1}{\text{s}}^{-1}$
$k=3.0\times 10^{-5}{\text{ s}}^{-1}$

Substituting these values into the rate equation:
$2.4\times 10^{-5}=3.0\times 10^{-5}\times [{\text{N}}_2{\text{O}}_5]$

Solving for the concentration of ${\text{N}}_2{\text{O}}_5$:
$[{\text{N}}_2{\text{O}}_5]=\frac{2.4\times 10^{-5}}{3.0\times 10^{-5}}$

$[{\text{N}}_2{\text{O}}_5]=\frac{2.4}{3.0}$

$[{\text{N}}_2{\text{O}}_5]=0.8{\text{ mol L}}^{-1}$

Answer: $0.8$