Consider the following mechanism. (1) ClO(aq) + H2O(l) equilibrium reaction arro

Question

Consider the following mechanism. (1) ClO(aq) + H2O(l) equilibrium reaction arrow HClO(aq) + OH (aq) [fast] (2) I (aq) + HClO(aq) HIO(aq) + Cl (aq) [slow] (3) OH (aq) + HIO(aq) H2O(l) + IO(aq) [fast] (a) What is the overall equation? (Use the lowest possible coefficients. Include states-of-matter under SATP conditions in your answer. (b) Identify the intermediate(s), if any. (Separate substances in a list with a comma. Omit states-of-matter in your answer.) (c) What are the molecularity and the rate law for each step? (Rate equations take the general form 'rate = k . [A] . [B]'.) (d) Is the mechanism consistent with the actual rate law: rate = k[ClO][I ]?

Explanation / Answer

ClO(aq) + H2O(l) ----------> HClO(aq) + OH (aq) (fast)

I (aq) + HClO(aq) HIO(aq) + Cl (aq) (slow)

OH (aq) + HIO(aq) H2O(l) + IO(aq) (fast)

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ClO- (aq) + I- (aq) ----------> IO- (aq) + Cl- (aq)

HIO (aq) and HClO (aq) are intermediate since the reaction is slow.

Only two molecules are involving in slow step and hence molecularity = 2

rate law = k [I-] [HClO] from slow step step of raction. because we donot find rate of a reaction in their fast steps. we can know from their slow steps.

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