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Question

The following reaction has a second-order rate law:
$$H_{2}(g) + 2ICl(g) \rightarrow I_{2}(g) + 2HCl(g)   $$
Rate $$= k[H_{2}][ICl]$$
Devise a possible reaction mechanism.


Solution

Possible reaction mechanism:
$$H_2+ICl\longrightarrow HCl+HI\dots slow(RDS)$$
$$HI+ICl\longrightarrow HCl+I_2\dots fast$$
Hence, $$Rate=K[H_2][ICl]$$ from rate determining step(rds).

Chemistry
NCERT
Standard XII

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