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Question

The reaction at hydrogen and iodine monochloride is represented by the equation is
$$H_{2} (g) + 2ICl (g) \rightarrow 2HCl (g) + I_{2} (g)$$
This reaction is first order in $$H_{2}(g)$$ and also first - order in ICI(g). which of these proposed mechanism can be consistent with the given information about this reaction ?
Mechanism I : $$H_{2} (g) + 2ICl (g) \rightarrow 2HCl (g) + I_{2} (g)$$
Mechanism II : $$H_{2} (g) + ICl (g) \overset{slow}{\rightarrow} HCl (g) + HI (g)$$
$$HI (g) + ICl (g) \overset{fast}{\rightarrow} HCl (g) + I_{2} (g)$$ :


A
I only
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B
II only
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C
Both I and II
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D
Neither I nor II
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Solution

The correct option is B II only
According to question the given reaction is first order in $$H_2(g)$$ and also first order in $$ICl(g)$$ so, the slowest (rate determining) step in the reaction should involve $$H_2(g)$$ & $$ICl(g)$$ one mole each.
The mechanism $$II$$ is seeming consistent with the conditions stated as:-
$$H_2(g)+ICl(g)\longrightarrow HCl(g)+HI(g)$$    (slow)
   $$Rate=K[H_2][ICl]$$
& $$HI(g)+ICl(g)\longrightarrow HCl(g)+I_2(g)$$   (fast)

Chemistry

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