Question

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.

Homework Answers

Answer #1

reaction is

H2O2+2H+2I--->I2+H2O

Mechanism is

H2O2    +    I-   --->    HOI   +   OH (SLOW)

OH+H--->H2O (FAST)

HOI+H+I--->I2+H2O (FAST)

molecularity of the reaction is nothing but a number of molecules or ions that participate in the slow step because slow step is the rate determining step

here rate determining step

H2O2    +    I-   --->    HOI   +   OH-

no of molecules participated here is 2

molecularity is 2

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Consider the following proposed mechanisms for Reaction (1): Mechanism A (one step): H2O2 + 2I- +...
Consider the following proposed mechanisms for Reaction (1): Mechanism A (one step): H2O2 + 2I- + 2H3O+ à I2 + 4H2O Reaction (1) Mechanism B (three steps) H2O2 + I- à OH- + HOI (slow) H3O+ + OH- ßà 2H2O (fast) HOI + H3O+ + I- à I2 + H2O (fast) a) Show that when you sum the three elementary steps, the net result of Mechanism B is Reaction (1): b) What would be the expected rate law for mechanism...
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 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 mechanism of a reaction is shown below.             a) What is the overall reaction? b)...
The mechanism of a reaction is shown below.             a) What is the overall reaction? b) Which compounds are intermediates? c) Predict the rate law based on this mechanism. d) What is the overall order of the reaction?             HOOH + I¯      HOI + OH¯        (slow)             HOI + I¯    I2   +   OH¯                 (fast)             2OH¯   +   2H3O+ 4 H2O             (fast)
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...
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]
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 following three step mechanism has been proposed for this reaction: Step 1: A + B...
The following three step mechanism has been proposed for this reaction: Step 1: A + B <--> G fast Step 2: A + G --> E + D slow Step 3: E + 2C --> 2D + F fast Determine the rate law predicted by the mechanism. Identify any intermediates shown. The experiemental rate law was determined to be Rate = [A]2[B]. Is this mechanism valid?
Consider the following two-step mechanism for a reaction: NO2(g)+Cl2(g)→ClNO2(g)+Cl(g)Slow NO2(g)+Cl(g)→ClNO2(g)Fast Part A What is the overall...
Consider the following two-step mechanism for a reaction: NO2(g)+Cl2(g)→ClNO2(g)+Cl(g)Slow NO2(g)+Cl(g)→ClNO2(g)Fast Part A What is the overall reaction? Express your answer as a chemical equation. Identify all of the phases in your answer. Part B Identify the intermediates in the mechanism Part C What is the predicted rate law?
The following mechanism has been proposed for the gas-phase reaction of chloroform (CHCl3) and chlorine. Cl2...
The following mechanism has been proposed for the gas-phase reaction of chloroform (CHCl3) and chlorine. Cl2 ? 2Cl (fast, reversible) Cl + CHCl3 ? HCl + CCl3 (slow) Cl + CCl3 ? CCl4 (fast) What rate law does this mechanism predict? (Choose from the list below and enter your answers in alphabetical order, e.g. ABC ). A)k G) [HCl]1/2 M) [Cl]2 B) [HCl] H) [Cl2]1/2 N) [CHCl3]2 C) [Cl2] I) [Cl]1/2 O) [CCl3]2 D) [Cl] J) [CHCl3]1/2 P) [HCl]2 E)...