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

Solution

## The correct option is B II onlyAccording 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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