Question

$2 \mathrm{~N}_2 \mathrm{O}_5(\mathrm{~g}) \rightarrow 4 \mathrm{NO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g})$

What is the ratio of the rate of decomposition of $N_{2}O_{5}$ to rate of formation of $O_{2}$ ?

• A. $1 : 2$
• B. $2 : 1$
• C. $1 : 4$
• D. $4 : 1$

Answer 1

Answer: (B)

As per unique value of reaction rate:

$- \frac{1}{2} \frac{\text{d}}{\text{dt}} \left[\text{N}_{2} \text{O}_{5}\right] = \frac{1}{1} \frac{\text{d}}{\text{dt}} \left[\text{O}_{2}\right]$

$\therefore \frac{\frac{\text{d}}{\text{dt}} \left[\text{N}_{2} \text{O}_{5}\right]}{\frac{\text{d}}{\text{dt}} \left[\text{O}_{2}\right]} = \text{2 : 1}$ ​