Question

The rate constant for the reaction
$2N_2{O}_5\to 4N{O}_2+O_2$
is $3.0\times {10}^{-5}{\text{sec}}^{-1}$. If the rate is $2.4\times {10}^{-5}mol{L}^{-1}{\text{sec}}^{-1}$, then the concentration of $N_2{O}_5(inmole{L}^{-1}$) is

• A. $1.4$
• B. $1.2$
• C. $0.004$
• D. $0.8$

Answer 1

The correct option is D $0.8$

$\text{Rate constant (k)}=3\times {10}^{-5}{\text{sec}}^{-1}$
$\text{Rate of reaction}=2.40\times {10}^{-5}mole{\text{L}}^{-1}{\text{sec}}^{-1}$
$\text{Rate of reaction}=k\times [Molarconc.of{N}_2{O}_5]$
$\left[N_2{O}_5\right]=\frac{2.40\times {10}^{-5}}{3\times {10}^{-5}}=0.8mol{L}^{-1}$