For the reaction; $H_{2} (g) + I_{2} (g) ⟶ 2 HI (g),$ the rate law is
$Rate = k [H_{2}] [I_{2}]$
Which of the mechanisms given is consistent with this rate law?
I II
$\begin{array}{ll} I_{2} ⇌ I + I (fast) \\ H_{2} + I + I ⟶ 2 HI (slow) \end{array}$ $\begin{array}{ll} I_{y} ⟶ I + I (slow) \\ H_{2} + I + I ⟶ 2 HI (fast) \end{array}$

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Either I or II

II only

Neither I nor II

I only

answer is A.

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Detailed Solution

The reactions,

$\begin{array}{l} I_{2} ⇌ 2 I (fast) \\ H_{2} + I + I ⟶ 2 HI (slow) \end{array}$

This mechanisms is consistent with this rate law. Here, only I is correct.

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I	II
$\begin{array}{ll} I_{2} ⇌ I + I (fast) \\ H_{2} + I + I ⟶ 2 HI (slow) \end{array}$	$\begin{array}{ll} I_{y} ⟶ I + I (slow) \\ H_{2} + I + I ⟶ 2 HI (fast) \end{array}$