Duration: 4:14

1 views

0

Reaction between \( \mathrm{NO} \) and \( \mathrm{O}_{2} \) to form \( \mathrm{NO}_{2} \) is \( 2 \mathrm{NO}+\mathrm{O}_{2} \longrightarrow 2 \mathrm{NO}_{2} \) follows the following mechanism
\[
\begin{array}{ll}
\mathrm{NO}+\mathrm{NO} \underset{\mathrm{k}-1}{\stackrel{\mathrm{k}_{1}}{\rightleftharpoons}} \mathrm{N}_{2} \mathrm{O}_{2} & \text { (in rapid equilibrium) } \\
\mathrm{N}_{2} \mathrm{O}_{2}+\mathrm{O}_{2} \stackrel{\mathrm{k}_{2}}{\longrightarrow} 2 \mathrm{NO}_{2} & \text { (slow) }
\end{array}
\]
\( \mathrm{P} \)
W
Show that the rate of reaction is given by
\[
-\frac{1}{2}\left(\frac{\mathrm{d}\left[\mathrm{NO}_{2}\right]}{\mathrm{dt}}\right)=\mathrm{K}[\mathrm{NO}]^{2}\left[\mathrm{O}_{2}\right]
\]
📲PW App Link - https://bit.ly/YTAI_PWAP
🌐PW Website - https://www.pw.live