The mechanism of the reaction 2NO-O2- 2NO2 is- NO-NOk1k-1-N2O2 fast - N2O2-O2 k 2 -2NO 2 slowThe rate constant of the reaction is-

The correct option is D k_2[ k_1/k_ 1 ] r = k_2[N_2O_2 ] [O_2 ] ....(i) k_1/k_ 1 = [N_2O_2 ]/[NO ]^2 or [N_2O_2 ] = k_1/k_ 1[NO ]^2 from eq. (i) ...

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Byju's Answer

Standard XII

Chemistry

Zinc II Sulphate

The mechanism...

Question

The mechanism of the reaction $2 N O + O_{2} \to 2 N O_{2}$ is:
$N O + N O_{1} N_{2} O_{2} (f a s t); N_{2} O_{2} + O_{2}_{2} 2 N O_{2} (s l o w)$
The rate constant of the reaction is:

k_{2}

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k_{2} k_{1} (k_{- 1})

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k_{2} k_{1}

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k_{2} (\begin{matrix} \frac{k_{1}}{k_{- 1}} \end{matrix})

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Solution

The correct option is D $k_{2} (\begin{matrix} \frac{k_{1}}{k_{- 1}} \end{matrix})$
$r = k_{2} [N_{2} O_{2}] [O_{2}]$ ....(i)
$\frac{k_{1}}{k_{- 1}} = \frac{[N_{2} O_{2}]}{{[N O]}^{2}} o r [N_{2} O_{2}] = \frac{k_{1}}{k_{- 1}} {[N O]}^{2} f r o m e q .$ (i)
$r = k_{2} \frac{k_{1}}{k_{- 1}} = {[N O]}^{2} [O_{2}]$
compair $r = k {[N O]}^{2} [O_{2}]$
$k = k_{2} \frac{k_{1}}{k_{- 1}}$

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Similar questions

Q. The mechanism of the reaction

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

is:

N O + N O_{1} N_{2} O_{2}

(fast) ------ 1

N_{2} O_{2} + O_{2}_{2} 2 N O_{2}

(slow) -----2

The rate constant of the reaction is:

Q. The mechanism of the reaction :

2 N O + O_{2} ⟶ 2 N O_{2}

is,

N O + N O_{1} K_{- 1} N_{2} O_{2} (f a s t)

;

N_{2} O_{2} + O_{2} k_{2} - \to 2 N O_{2} (s l o w)

The rate constant of the reaction is :

Q. What is the relation between the equilibrium constants

K

K_{1}

and

K_{2}

for the following reactions?

N_{2} + 2 O_{2} ⇋ 2 N O_{2}, K

N_{2} + O_{2} ⇋ 2 N O, K_{1}

2 N O + O_{2} ⇋ 2 N O_{2}, K_{2}

Q. Reaction between NO and

O_{2}

to form

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

follows the following mechanism:

First step :

N O + N O ⇌ N_{2} O_{2}

(in rapid equilibrium)

Here,

K_{1}

is the rate constant for forward reaction while

K_{- 1}

is the rate constant for backward reaction.

Second step :

N_{2} O_{2} + O_{2}_{2} 2 N O_{2}

(slow)

Determine the rate of reaction.

Q. Assertion :Observed rate constant of the given reaction given below decreases with temperature.

N O + N O_{f} K_{b} N_{2} O_{2}

N_{2} O_{2} + O_{2} K \to s l o w 2 N O_{2}

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

Reason:

K_{c}

of the reaction being exothermic and decrease in

K_{c}

overweigh increase in K with increase in temperature.

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The mechanism of the reaction 2NO+O2→2NO2 is:NO+NOk1⇌k−1N2O2(fast);N2O2+O2k2⟶2NO2(slow)The rate constant of the reaction is:

The correct option is D k2(k1k−1)r=k2[N2O2][O2]....(i)k1k−1=[N2O2][NO]2or[N2O2]=k1k−1[NO]2fromeq.(i)r=k2k1k−1=[NO]2[O2]compair r=k[NO]2[O2]k=k2k1k−1

The mechanism of the reaction $2 N O + O_{2} \to 2 N O_{2}$ is:
$N O + N O_{1} N_{2} O_{2} (f a s t); N_{2} O_{2} + O_{2}_{2} 2 N O_{2} (s l o w)$
The rate constant of the reaction is: