[hellwraiz]

These are the steps for a reaction.

CH3COCH3 + H+  CH3C(OH)CH3                 fast
CH3C(OH)CH3 → CH3C(OH)=CH2 + H+           slow
CH3C(OH)=CH2 + I2 → CH3COCH2I + HI      fast

My question is, why is the rate equation rate = k[CH3C(OH)CH3][H+] and not rate = k[CH3C(OH)CH3][H+][CH3C(OH)=CH2]

These equations are from a past paper and they did not show me the states of the molecules

[sjb]

What are your understandings of the speeds of the reactions?

[Orcio_87]

My question is, why is the rate equation rate = k[CH3C(OH)CH3][H+] and not rate = k[CH3C(OH)CH3][H+][CH3C(OH)=CH2]

This would mean that reaction is somehow second order to acetone.

Why does reaction speed does not depend on concentration of iodine - I don't know.

[hellwraiz]

What are your understandings of the speeds of the reactions?

My understanding is that because the second reaction is slow, it is the rate determining step, so all the chemicals that are in that step are in the rate equation.

[sjb]

My understanding is that because the second reaction is slow, it is the rate determining step, so all the chemicals that are in that step are in the rate equation.

So why is the rate not just k[enol]?

[hellwraiz]

So why is the rate not just k[enol]?

That is kinda my question. In the pastpaper it is stated that the rate is k[CH3COCH3][H+] and I don't know why.

[sjb]

Are enols stable?