Question

Consider the reaction, $2N_{2}O_{5} \to 4NO_{2} + O_{2}$ In the reaction $NO_{2}$ is being formed at the rate of $0.0125\, mol \, L^{-1} s^{-1}$. What is the rate of reaction at this time?

• A. $0.0018 \, mol \, L^{-1} s^{-1}$
• B. $0.0031 \, mol \, L^{-1} s^{-1}$
• C. $0.0041 \, mol \, L^{-1} s^{-1}$
• D. $0.050\, mol \, L^{-1} s^{-1}$

Answer 1

Answer: (B)

Rate $=\frac{1}{4} \frac{d[NO_{2}]}{dt}$
$=\frac{1}{4}\times0.0125$
$=0.0031 \,mol \,L^{-1}s^{-1}$