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Iodine monochloride reacts with hydrogen according to the equation :
$2 ICl (g) + H_{2} (g) \to I_{2} (g) + 2 HCl (g)$
The rate data below have been obtained.
[ICI], M $[H_{2}]$ , M Initial Rate, $M . s^{- 1}$
0.10 0.10 0.030
0.20 0.10 0.060
0.10 0.050 0.015
What is the rate law for the reaction?

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$Rate = k [ICl] [H_{2}]$

$Rate = k {[ICl]}^{2} [H_{2}]$

$Rate = k [ICl] {[H_{2}]}^{1 / 2}$

$Rate = k {[ICl]}^{2} {[H_{2}]}^{1 / 2}$

answer is A.

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Detailed Solution

$aA + bB ⟶ products$

$2 ICl (g) + H_{2} (g) \to I_{2} (g) + 2 HCl (g)$

$Rate = k [A]^{m} [B]^{n}$

$Rate = k [ICl] [H_{2}]$

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