The following mechanism has been proposed for the gas phase reaction of H2 with ICl: H2 (g) + ICl(g) ---> HI (g) + HCl (g) HI (g) + ICl(g) ---> I2 (g) + HCl(g)   If the first step is slow and the second one is fast, which rate law do you expect to be observed for the overall reaction? Group of answer choices A.) r = k[H2][ICl]2   B.) r = k[HI][ICl]   C.) r = k[H2]   D.) r = k[H2][ICl]

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