Question

Consider the reaction $2 N _{2} O _{4} \rightleftharpoons 4 NO _{2}$ and given that $\frac{-d\left[ N _{2} O _{4}\right]}{dt}=k$ and $\frac{d\left[ NO _{2}\right]}{d t}=k^{\prime}$, then

• A. $2 k^{\prime}=k$
• B. $ k^{\prime}=2 k$
• C. $k^{\prime}=k$
• D. none of these

Answer 1

Answer: (B)

$ 2 N _{2} O _{4} \rightleftharpoons 4 NO _{2}$

Rate $=-\frac{1}{2} \frac{d\left[ N _{2} O _{4}\right]}{dt}=+\frac{1}{4} \frac{d\left[ NO _{2}\right]}{d t}$

$\frac{1}{2} k=\frac{1}{4} k^{\prime}$

$ \Rightarrow k^{\prime}=2 k$