Question

A possible mechanism for the overal eaction is CIO- (aq) + I-(aq) ---> + IO-(aq) 1)...

A possible mechanism for the overal eaction is

CIO- (aq) + I-(aq) ---> + IO-(aq)

1) CIO-(aq) + H20(l) ---K1--> <--K-1--- HCIO (aq) + OH- (aq) FAST

2) I- (aq) + HCIO (aq) ---K2--> HIO (aq) + CI- (aq) SLOW

3) OH-(aq) + HIO (aq)---->H2O(l) + IO- (aq) FAST

Provide the rate law for formaion of OI- based on this mechanism. Express the rate constant in terms of K1, K-1, K2, and K3.

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Answer #1

Ans:

We know that the Rate of reaction is depends upon the Slow step.

Therefore, Rate of reaction will determined on the basis of Second step.

I- (aq) + HCIO (aq) ---K2--> HIO (aq) + CI- (aq) ----SLOW

Hence, Rate law is, R = K2 [I-][HClO] i.e. It is a second order reaction.

Rate Constant,

1) CIO-(aq) + H20(l) ---K1--> <--K-1--- HCIO (aq) + OH- (aq) FAST

R = K1[ClO-]= K-1[HClO]------ As H2O and OH- are in excess, rate will be independent of them.

2) I- (aq) + HCIO (aq) ---K2--> HIO (aq) + CI- (aq) SLOW

R = K2 [I-][HClO]

3) OH-(aq) + HIO (aq)---->H2O(l) + IO- (aq) FAST

R = K3 [HIO]------------- As OH- is in excess.

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