Which of the following is an example of a fractional order reaction?

N H_{4} N O_{2} \to N_{2} + 2 H_{2} O

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N O + O_{3} \to N O_{2} + O_{2}

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2 N O + B r_{2} \to 2 N O B r

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C H_{3} C H O \to C H_{4} + C O

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Solution

The correct option is D $C H_{3} C H O \to C H_{4} + C O$
where $∙ C H_{3}$ is methyl radical.
In the steady state, the rates of formation and destruction of methyl radicals are equal, so that
$\frac{d [∙ C H_{3}]}{d t} = k_{i} [C H_{3} C H O] - k_{t} [∙ C H_{3}]^{2} = 0$
$[∙ C H_{3}] \propto [C H_{3} C H O]^{1 / 2}$
$\frac{d [C H_{4}]}{d t} = k_{p} [∙ C H_{3}] [C H_{3} C H O] \propto [C H_{3} C H O]^{3 / 2}$
Hence the order of the reaction is 3/2.
Option D is correct.

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Similar questions

The reaction :

2 N O + B r_{2} \to 2 N O B r

obeys the following mechanism:

N O + B r_{2} ⇌ N O B r_{2}

------- (Fast)

N O B r_{2} + N O \to 2 N O B r

-------- (Slow)

The order of the reaction is:

Calculate the total number of molecules that will possess fractional bond order among the following molecules
$O_{2}^{2 +}, N_{2}^{2 +}, O_{2}^{+}, N O, C O, C O^{+}, O_{2}^{-}, N O^{2 +}, C N^{-}, N O^{2 -}, N_{2}^{-}$

Q. The reaction

2 N O + B r_{2} \to 2 N O B r

, is supposed to follow the following mechanism
(i)

N O + B r_{2} ⇌ N O B r_{2}

(ii)

N O B r_{2} + N O s l o w \to 2 N O B r

The rate law expression is:

Q. For the reaction

2 NO + {Br}_{2} \to 2 NOBr

the following mechanism has been given:

NO + {Br}_{2} ⇌ {NOBr}_{2}

{NOBr}_{2} + NO \to 2 NOBr (slow)

Hence, the rate law is :

Q. For the reaction

2 NO + {Br}_{2} \to 2 NOBr

the following mechanism has been given:

NO + {Br}_{2} ⇌ {NOBr}_{2}

{NOBr}_{2} + NO \to 2 NOBr (slow)

Hence, the rate law is :

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