For the reaction H2O2 + 2H+ + 2I – ® I2 + 2H2O the following mechanism has been suggested.
Identify the rate law for the reaction and explain why |
For the reaction H2O2 + 2H+ + 2I – ® I2 + 2H2O the following mechanism...
II. Show your work in detail (step by step). You must show your work. The following mechanism has been suggested for the reaction: H2O2 + 2H+ + 2I – ® I2 + 2H2O H2O2 + I – ® HOI + OH – Slow OH – + H+ ® H2O Fast HOI + H+ + I – ® I2 + H2O Fast Identify all intermediates included in this mechanism.
8. The rate law for the reaction H2O2 + 2H+212 + 2H2O is rate-k[H202][1]. The following mechanism has been suggested. H2O2+1 - HOI + OH - slow OH + H H20 fast HỘI + H+ + + I2 + H2O fast Identify all intermediates included in this mechanism. A) H and I D) Honly B) H and HOI E) H20 and OH C) HOI and OH 9. Which of the following statements is false? A) A catalyst increases the rate...
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...
4. (22 pts) Consider the following exothermic reaction: H2O2 +2t + 2H' → 12 + 2H20 Consider the following mechanism for this reaction H,02 + r-* Hol + OH' Hol + r- 12 + он. 20H 2H2 H20 slow fast fast a) What species are intermediates in the above mechanism? Any catalysts? b) Sketch an energy versus reaction progress plot for the three step mechanism and clearly label the rate determining step in your diagram. c) What rate law would...
14-99. The mechanism for the reaction 2H,0, (aq) ® 2H,00) +0,) in the presence of I (aq) is proposed to be: Step 1: H,02(aq) + I (aq) ® H,0(0) + Ol (aq) Step 2: H,0, (aq) + 01 (aq) ® H,00) + 0,(g) + 1 (aq) (slow) (fast) What is the molecularity of the rate-determining step? Select one: a. zero molecular b. unimolecular c. bimolecular d. termolecular e. More information is needed to answer this question.
i. For the reaction: 2H202→ 2H2O+O2 a proposed mechanism is: H2O2 + H3O2+ → H2O + H30+ +02 (a) The intermediate in the proposed mechanism is The catalyst is (b) Apply the steady state approximation to this mechanism to deduce the rate law in terms of d[O2]/dt. (15 pts)
H2O2 + 3 I- + 2 H+ → I3- + 2 H2O Step 1. H2O2 + H+ → H3O2+ Step 2. H3O2+ + I- → H2O + HOI Step 3. HOI + I- → OH- + I2 Step 4. OH- + H+ → H2O Step 5. I2 + I- → I3- How many of the following statements are correct based on the information given? 1. I3- is a product of this reaction 2. I2 is a reactant in this reaction...
The reaction mechanism that has been proposed for the decomposition of H2O2 by iodide ion is: H2O2 + I- → H2O + IO- (slow) H2O2 + IO- → H2O + O2 + I- (fast) Which one of the following statements is true? Select one: a. The reaction is second order with respect to I-. b. I- is an intermediate. c. The reaction is first order with respect to I-. d. IO- is a catalyst. e. The reaction is zero order...
5. Iodide is oxidized by hydrogen peroxide according to the following mechanism: H 2 O 2 + I- → H 2 O + OI- (slow) H+ + OI- → HOI (fast) HOI + H+ + I- → I2 + H2O (fast) (a) What is the overall reaction? (b) What is the molecularity of each step? (c) Write the rate equation for the rate-determining step. (d) What are the intermediates in this reaction? (If none, write “none.”)
What is the rate law for the one-step mechanism shown below, and why? Explain how you got to your conclusion H2O2 + 2I- + 2H+ --> I2 + 2H20