For the reaction,
${NO}_{2} (g) + CO (g) ⟶ NO (g) + {CO}_{2} (g)$
at temperatures below $500 K$ , the rate law is rate $= k {[{NO}_{2}]}^{2}$ Which mechanism is consistent with this information?
Mechanism 1 :
${NO}_{2} + {NO}_{2} ⟶ {NO}_{3} + NO (slow)$
$CO + {NO}_{3} ⟶ {CO}_{2} + {NO}_{2} (f a s t)$
Mechanism 2 :
${NO}_{2} + {NO}_{2} ⟶ {NO}_{3} + NO (fast)$
$CO + {NO}_{3} ⟶ {CO}_{2} + {NO}_{2} (s l o w)$

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Neither 1 nor 2

2 only

Either 1 or 2

1 only

answer is A.

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Detailed Solution

$r = K {[{NO}_{2}]}^{2}$

rate determining step is slower step

$\frac{Mech - 1}{{NO}_{2} + {NO}_{2}} - {NO}_{3} + NO (Sl ow)$

$V = k [{NO}_{2}] [{No}_{2}]$

$V = k {[{NO}_{2}]}^{2}$

Mech - 2

$CO + {NO}_{3} \to {CO}_{2} + {NO}_{2}$

$V = K [\begin{array}{ll} CO \end{array}] [{NO}_{3}]$

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