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Heat of Formation

A two-step me...

Question

A two-step mechanism has been suggested for the reaction of nitric oxide and bromine.
$N O (g) + B r_{2} (g) K_{1} - \to N O B r_{2} (g)$
$N O B r_{2} (g) + N O (g) K_{2} - \to 2 N O B r (g)$
The observed rate law is, rate $= k [N O]^{2} [B r_{2}]$ . Hence, the rate-determining step is :

A

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

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B

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

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C

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

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D

none of these

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Solution

The correct option is B $N O B r_{2} (g) + N O (g) \to 2 N O B r (g)$
$N O (g) + B r_{2} (g)_{1} N O B r_{2} (g)$ .....(i)
$N O B r_{2} (g) + N O (g) k_{2} - -- \to R D S 2 N O B r_{2} (g)$ .....(ii)
Rate = $k_{2}$ $[N O B r_{2}] [N O]$
Since, $N O B r_{2}$ is the reactive intermediate, so its constant ratio is dertermined from step (i).
$k_{1} o r k_{e q} = \frac{[N O B r_{2}]}{[N O] [B r_{2}]}$
or $[N O B r_{2}] = k_{1} [N O] [B r_{2}]$
Substitute the $[N O B r_{2}]$ in step (iii),
$∴$ Rate = $k_{1} k_{2} [N O]^{2} [B r_{2}] = K [N O]^{2} [B r_{2}]$

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Similar questions

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

N O

B r_{2}

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)}

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

N O

B r_{2}

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. Write the rate law for
- Reaction is second order in

N O (g)

and first order in

B r_{2} (g)

Q. The following data were obtained for the reaction

N O_{(g)} + B r_{2 (g)} \to 2 N O B r_{(g)}

Expt initial conc initial rate

Expt	Initial conc	Initial rate:
[NO]	$[B r_{2}]$	mol L $^{- 1}$ min $^{- 1}$
0.1	0.1	$1.3 \times 10^{- 6}$
0.2	0.1	$5.2 \times 10^{- 6}$
0.3	0.3	$1.56 \times 10^{- 5}$

The order of the reaction is:

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