Question

Nitric Oxide reacts with Oxygen to produce Nitrogen Dioxide as follows :
$\sf 2NO + O_2 \longrightarrow 2NO_2$

The mechanism of the reaction is :
$\sf NO + O_2 \leftrightharpoons NO_3 \ (Fast)$
The rate constant here is K

$\sf NO_3 + NO \longrightarrow 2NO_2 \ (Slow)$
The rate constant is $\sf K_1$

Write the rate law for the above reaction. ​

Answer 1

EXPLANATION.

Rate law is only calculate for slow

reaction.

Rate law

$\implies{ \frac{ k_{3} k_{1}}{ k_{2} } } (no)( o_{2})(no)$

Keff

=> [ No] = 2

=> [O2 ] = 1

=> [No]²[O2]¹

order of reaction = 2 + 1 = 3

Note = see the image attachment

for full solution.

Answer 2

☆SOLUTION :- REFER TO THE ATTACHMENT

HOPE IT HELPS :)