Chemistry question, please help

Question

QUESTION 3

3.1 The following mechanism has been proposed for the gas – phase reaction of hydrogen (H2) and iodine monochloride (ICl):

H₂(g) + ICl(g) → HI(g) + HCl(g)

HI(g) + ICl(g) → I₂(g) + HCl(g)

3.1.1 Write the balanced chemical equation for the overall reaction.

3.1.2 Identify any intermediate/s in the mechanism.

3.1.3 Write the rate law for each elementary step in the reaction mechanism.

3.1.4 If the first step is slow and the second step is fast, write the rate law you would expect to be observed for the overall reaction.

Answer 1

H₂(g) + ICl(g) → HI(g) + HCl(g)

HI(g) + ICl(g) → I₂(g) + HCl(g)

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H2(g) + 2ICI(g) ==> 2HCl(g) + I2(g) ... balanced equation for the overall reaction

The intermediate is HI(g)

The rate law for each elementary step is:

Rate = k[H₂][ICI]

Rate = k[HI][ICI]

Rate law for overall reaction assuming first step is slow:

Rate = k[H₂][ICI]