Question

For the reaction, $2N_{2}O_{5} \to 4NO_{2} + O_{2}$, the rate of reaction can be expressed in terms of time and concentration by the expression:

• A. Rate $= -\frac{d\left[N_{2}O_{5}\right]}{dt}=-\frac{1}{4}\frac{d\left[NO_{2}\right]}{dt}=\frac{1}{2}\frac{d\left[O_{2}\right]}{dt}$
• B. Rate $= -\frac{1}{2} \frac{d\left[N_{2}O_{5}\right]}{dt}=\frac{1}{4}\frac{d\left[NO_{2}\right]}{dt}=\frac{d\left[O_{2}\right]}{dt}$
• C. Rate $= -\frac{1}{4} \frac{d\left[N_{2}O_{5}\right]}{dt}=\frac{1}{2}\frac{d\left[NO_{2}\right]}{dt}=\frac{d\left[O_{2}\right]}{dt}$
• D. Rate $= -\frac{1}{2} \frac{d\left[N_{2}O_{5}\right]}{dt}=\frac{1}{2}\frac{d\left[NO_{2}\right]}{dt}=\frac{1}{2} \frac{d\left[O_{2}\right]}{dt}$

Answer 1

Answer: (B)

Correct answer is (b) Rate $= -\frac{1}{2} \frac{d\left[N_{2}O_{5}\right]}{dt}=\frac{1}{4}\frac{d\left[NO_{2}\right]}{dt}=\frac{d\left[O_{2}\right]}{dt}$