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Chemical Kinetics — Chemistry STD 12 Science — Question

Gujarat BoardEnglish MediumSTD 12 ScienceChemistryChemical Kinetics3 Marks
Question
Nitric oxide, NO, reacts with oxygen to produce nitrogen dioxide.
$\text{2NO(g)+O}_2(\text{g)}\rightarrow\text{2NO}_2\text{(g)}$
The rate law for this reaction is:
$\text{Rate = k}[\text{NO]}^2[\text{O]}_2$
Propose a machanism for the reaction.
✓

Answer

The probable proposed mechanism may be, $\text{NO+O}_2\rightarrow \text{NO}_3 \text{ (fast)}\ \dots\text{Step I}\\ $ $\text{NO}_3+ \text{NO }\rightarrow\text{NO}_2+\text{NO}_2 \text{ (slow)}\ \dots\text{Step II}{}$Since slowest reaction is the rate determining step, therefore
$\text{Rate = k}_1[\text{NO}_3]\text{ [NO]}$ $\text{k}=\frac{\text{|NO}_3|}{|\text{NO| |O}_2|}$ $[\text{NO}_3]=\text{k[NO] [O}_2]$ $\text{Rate = k}_1\text{K[NO] [O}_2]\text{ [NO]}=\text{k[NO]}^2[\text{O}_2]$, where $K =k_1.K$

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