Question

For a reaction $2N_2{O}_5\to 4N{O}_2+O_2$;
Initial concentration of $N_2{O}_5$ is $7.2$ mol $L^{-1}$ and after $20$ minutes $\left[N{O}_2\right]=2.4$ mol $L^{-1}$, then what will be rate of decomposition of $N_2{O}_5$ in mol $L^{-1}$ $mi{n}^{-1}$

• A. $0.06$
• B. $0.03$
• C. $1.3$
• D. $2.4$

Answer 1

The correct option is A $0.06$

The given reaction is :-

$2N_2{O}_5\to 4{NO}_2+O_2$

Initial conc. of $N_2{O}_5=7.2M$

After 20min. , conc. of ${NO}_2=2.4M$

Initial conc. of ${NO}_2=2.4M$

Now, Rate $=\frac{-d\left[N_2{O}_5\right]\times 1}{dt}\times \frac{1}{2}=\frac{1}{4}\times \frac{d\left[{NO}_2\right]}{dt}$

$\Rightarrow Rate=\frac{1}{4}\times \frac{2.4}{4}=\frac{0.3}{2}=0.15$

Now, $\frac{-d\left[N_2{O}_5\right]}{dt}\times \frac{1}{2}=0.15$

$\Rightarrow \frac{-d\left[N_2{O}_5\right]}{dt}=0.3$