Question

Consider the following mechanism. (1) ClO−(aq) + H2O(l) equilibrium reaction arrow HClO(aq) + OH −(aq) [fast]...

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 −]?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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)

---------------------------------------------------------------------

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.

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
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.
The reaction 2 H2O2 --> 2 H2O + O2 follows the mechanism: Step 1: H2O2 (aq)...
The reaction 2 H2O2 --> 2 H2O + O2 follows the mechanism: Step 1: H2O2 (aq) + I-(aq) --> H2O(l) + IO-(aq) SLOW    Step 2: IO-(aq) + H2O2(aq) --> H2O(l) + O2(g) + I-(aq) FAST What is the molecularity overall? A. termolecular B. bimolecular C. cannot be determined D. unimolecular
The following mechanism has been suggested for the reaction: H2O2+2H+2I--->I2+H2O H2O2+I--->HOI+OH (SLOW) OH+H--->H2O (FAST) HOI+H+I--->I2+H2O (FAST)...
The following mechanism has been suggested for the reaction: H2O2+2H+2I--->I2+H2O H2O2+I--->HOI+OH (SLOW) OH+H--->H2O (FAST) HOI+H+I--->I2+H2O (FAST) Identify the molecularity of the rate determining step. please explain why.
Determine the rate law that is consistent with the following mechanism: Step 1: OCl− + H2O...
Determine the rate law that is consistent with the following mechanism: Step 1: OCl− + H2O ⇄ HOCl + OH− (fast) Step 2: I− + HOCl  HOI + Cl− (slow) A) Rate = k[OCl−][H2O] B) Rate = k[I−][HOCl] C) Rate = k[OCl−][H2O][I−] D) Rate = k[OCl−][H2O]/[I−] E) Rate = k[OCl−][H2O]/[OH−] F) Rate = k[OCl−][H2O][I−]/[OH−]
The mechanism for the reaction 2 H2O2(aq) à 2 H2O(l) + O2(g) in the presence of...
The mechanism for the reaction 2 H2O2(aq) à 2 H2O(l) + O2(g) in the presence of I–(aq) is proposed to be: Step 1: H2O2(aq) + I–(aq) à H2O(l) + OI–(aq)                                   (slow) Step 2: H2O2(aq) + OI–(aq) à H2O(l) + O2(g) + I–(aq)                       (fast) What is the rate law for the overall reaction?             a. Rate = k[H2O2]2             b. Rate = k[H2O2][I–]             c. Rate = k[H2O2]2[I–]/[H2O]             d. Rate = k[H2O2][OI–]             e. Rate = k[H2O2]
Consider the reaction: 2 NH3 (aq) + OCl-(aq) -> N2H4(aq) + H2)(I) + Cl-(aq) This three-step...
Consider the reaction: 2 NH3 (aq) + OCl-(aq) -> N2H4(aq) + H2)(I) + Cl-(aq) This three-step mechanism is proposed: Nh3(aq) + OCl-(aq) --><-- NH2Cl(aq) + Cl-(aq) Fast NH2Cl(aq) + NH3(aq) --> N2H5+(aq) + Cl-(aq) Slow N2H5+ (aq) + OH-(aq) --> N2H4 (aq) + H2O(l) Fast A. Show that the mechanism sums to the overall reaction. B. What is the rate law predicted by the mechanism? The answer is wrong in the textbook solutions, so I can't check my work and...
Nitramide, NO2NH2, decomposes slowely in aqueous slution according to the following reaction: NO2NH2 (aq) ---> N2O...
Nitramide, NO2NH2, decomposes slowely in aqueous slution according to the following reaction: NO2NH2 (aq) ---> N2O (g) + H2O the reaction follows the rate law: Rate= k(NO2NH2)/(H3O+) *Omit H2O from the rate law that you determine from the Mechanisms* (a) Which of the following mechanisms is the most appropriate for the interpretation of this rate law? Justify your answer. Mechamism 1 NO2NH2 ---> N2O + H2O  rate constant = k1 Mechanism 2 NO2NH2 + H3O+ <---> NO2NH3+ + H2O Fast rate...
The rate law for the reaction H+(aq) + OH−(aq) ---> H2O(l) is Rate = k[H+ ][OH−...
The rate law for the reaction H+(aq) + OH−(aq) ---> H2O(l) is Rate = k[H+ ][OH− ], with
 k = 1.3 x 10^11 mol-1 L s-1 at 25 deg C. In an experiment, 0.500 L of 0.020 mol L-1 KOH(aq) is rapidly mixed with an equal volume of 0.020 mol L-1 HBr(aq). Calculate the time, in seconds, required for [H+ ] to decrease to 1.0x 10^-7 mol L-1.

The iodide-catalyzed decomposition of hydrogen peroxide is thought to proceed by a four-step mechanism: H2O2(aq) +...
The iodide-catalyzed decomposition of hydrogen peroxide is thought to proceed by a four-step mechanism: H2O2(aq) + I-(aq) --> HOI(aq) + OH-(aq) (slow) HOI(aq) + OH-(aq) --> H2O(l) + OI-(aq) OI-(aq) + H2O2(aq) --> HOOI(aq) + OH-(aq) HOOI(aq) + OH-(aq) --> H2O(l) + O2(g) + I-(aq) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. oRate = k [H2O2]2 oRate = k [I-] [H2O2] oRate = k [H2O2] [H2O2] oRate...
The reaction 2 ClO2(aq) + 2 OH-(aq) ClO3-(aq) + ClO3-(aq) + H2O(l) was studied at a...
The reaction 2 ClO2(aq) + 2 OH-(aq) ClO3-(aq) + ClO3-(aq) + H2O(l) was studied at a certain temperature with the following results: Experiment [ClO2(aq)] (M) [OH-(aq)] (M) Rate (M/s) 1 0.0494 0.0494 0.0450 2 0.0494 0.0988 0.0899 3 0.0988 0.0494 0.180 4 0.0988 0.0988 0.360 (a) What is the rate law for this reaction? Rate = k [ClO2(aq)] [OH-(aq)] Rate = k [ClO2(aq)]2 [OH-(aq)] Rate = k [ClO2(aq)] [OH-(aq)]2 Rate = k [ClO2(aq)]2 [OH-(aq)]2 Rate = k [ClO2(aq)] [OH-(aq)]3 Rate...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT