A two-step mechanism has been suggested for the reaction of nitric oxide and bromine- NO g - Br 2 g k 1- NOBr 2 g NOBr 2 g - NO g k 2- 2 NOBr g Observed rate law is- rate - k - NO -2- Br 2- Hence- rate determining step is A- NO g - Br 2 g - NOBr 2 g B- NOBr 2 g - NO g - 2 NOBr g C- 2 NO g - Br 2 g - 2 NOBr g D- None of these

The correct option is B NOBr_2(g) + NO(g) → 2NOBr(g)Second step will be the rate determining step ...

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A two-step me...

Question

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

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

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

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

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Similar questions

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)

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

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)} .

{N O}_{(g)}

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)}

N O (g)

B r_{2} (g)

B r_{2}

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)}

N O_{(g)}

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