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Order of Reaction

The following...

Question

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:

1

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0

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3

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2

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Solution

The correct option is B $2$
Given, the rate determining step,

Rate = $k [N O B r_{2}] [N O]$ _______1
$K_{e q} = \frac{[N O B r_{2}]}{[N O] [B r_{2}]}$
$∴ [N O B r_{2}] = K_{e q} [N O [B r_{2}]$
substitute this value in equation 1, we get,

Rate $\propto [N O]^{2} [B r_{2}]^{1}$

The order of reaction with respect to $N O$ is $= 2$

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Similar questions

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)}

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)}

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 (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}]

B r_{2}

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