The following mechanism has been proposed for the reaction of NO with Br 2 to form NOBr NO - g - Br -2- g - rightleftharpoons NOBr -2 g NOBr-2 g - NO - g rightarrow -2 - NOBr - g If the second step is the rate determining step- the order of the reaction with respect to NO g isA- 1B- 0C- 2D- 3

The correct option is C 2Rate = k [NOBr_2]NO—–(I) But NOBr_2 is in equilibrium K_eq = [NOBr_2]/[NO][Br_2] From (I) & (II) Rate = K. K_eq[NO][Br_2][NO] Rate ...

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Byju's Answer

Standard XII

Chemistry

Rate of Reaction

The following...

Question

The following mechanism has been proposed for the reaction of NO with $B r_{2}$ to form NOBr
$N O_{(g)} + B r_{2_{(g)}} ⇌ N O B r_{2 (g)} N O B r_{2 (g)} + N O_{(g)} \to 2 N O B r_{(g)}$
If the second step is the rate determining step, the order of the reaction with respect to $N O_{(g)}$ is

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Solution

The correct option is C 2
$R a t e = k [N O B r_{2}] N O - - - - - (I)$
But $N O B r_{2}$ is in equilibrium
$K_{e q} = \frac{[N O B r_{2}]}{[N O] [B r_{2}]}$
From $(I) & (I I)$
Rate $= K . K_{e q} [N O] [B r_{2}] [N O]$
Rate $= K^{1} [N O]^{2} [B r_{2}] (w h e r e k^{1} = K . K_{e q})$

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Similar questions

Q. The following mechanism has been proposed for the reaction of

N O

with

B r_{2}

to form

N O B r

{N O}_{(g)} + {B r}_{2 (g)} f a s t ⇌ {N O B r}_{2 (g)}

N O {B r}_{2 (g)} + {N O}_{(g)} s l o w ⇌ 2 {N O B r}_{(g)} .

If the second step is the rate determining step, the order of the reaction with respect to

{N O}_{(g)}

is:

Q. The following mechanism has been proposed for the reaction of

N O

with

B r_{2}

to from

N O B r

{N O}_{(g)} + {B r}_{2} (g) f a s t ⇌ {N O B r}_{2 (g)}

N O {B r}_{2 (g)} + {N O}_{(g)} s l o w ⇌ {2 N O B r}_{(g)}

If the seconds step is the rate determining step,the order of the reaction is:

Q. A two-step mechanism has been suggested for the reaction of nitric oxide and bromine:

N O (g) + B r_{2} (g) k_{1} - \to N O B r_{2} (g)

N O B r_{2} (g) + N O (g) k_{2} - \to 2 N O B r (g)

Observed rate law is, rate =

k [N O]^{2} [B r_{2}]

: Hence, rate determining step is

Q. The following mechanism has been proposed for the reaction of NO with

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to form NOBr :

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)

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The following mechanism has been proposed for the reaction of NO with Br2 to form NOBr NO(g)+Br2(g)⇌NOBr2(g)NOBr2(g)+NO(g)→2 NOBr(g) If the second step is the rate determining step, the order of the reaction with respect to NO(g) is

The correct option is C 2Rate=k[NOBr2]NO−−−−−(I) But NOBr2 is in equilibrium Keq=[NOBr2][NO][Br2] From (I)&(II) Rate =K.Keq[NO][Br2][NO] Rate =K1[NO]2[Br2](where k1=K.Keq)

The following mechanism has been proposed for the reaction of NO with $B r_{2}$ to form NOBr
$N O_{(g)} + B r_{2_{(g)}} ⇌ N O B r_{2 (g)} N O B r_{2 (g)} + N O_{(g)} \to 2 N O B r_{(g)}$
If the second step is the rate determining step, the order of the reaction with respect to $N O_{(g)}$ is

The correct option is C 2
$R a t e = k [N O B r_{2}] N O - - - - - (I)$
But $N O B r_{2}$ is in equilibrium
$K_{e q} = \frac{[N O B r_{2}]}{[N O] [B r_{2}]}$
From $(I) & (I I)$
Rate $= K . K_{e q} [N O] [B r_{2}] [N O]$
Rate $= K^{1} [N O]^{2} [B r_{2}] (w h e r e k^{1} = K . K_{e q})$