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.
Intermediate of a reaction are those which is formed in the reaction but consumed during the process and does not appear in the final reaction ,
intermediate formed in this reaction is HOI and OH-
II. Show your work in detail (step by step). You must show your work. The following...
For the reaction H2O2 + 2H+ + 2I – ® I2 + 2H2O the following mechanism has been suggested. H2O2 + I – ® HOI + OH – slow OH – + H+ ® H2O fast HOI + H+ + I – ® I2 + H2O fast Identify the rate law for the reaction and explain why
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...
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...
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.”)
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...
#13 Interpreting Mechanisms 1. Consider the following mechanism: Step 1 Br2 2Br fast Step 2 Br + H2 H2Br fast Step 3 H2Br + Br 2HBr slow a. What is the overall equation? b. Identify the intermediate(s) if any. c. What is the molecularity and the rate law for each step including any reversible steps? d. What is the predicted rate law expression for this reaction. Be sure to only list reactants from the overall equation and...
Please answer each part with work shown. Thank you.
6. The following three mechanisms have been proposed for a particular reaction. Mechanism II Mechanism III Mechanisml H2 +NO-H2O+N (slow) N +NON2+0 (fast) O+H2-> H2O (fast) 2 NO-N202 (fast equilibrium) H2-N202-H20+ N3O (slow) H2+N20-H2O+N2 (fast) H2 + 2 NO- H2O+N2O (slow) N20+ H2N2+ H2O (fast) a) What is the overall reaction that each proposed mechanism supports? b) Calculate the ΔΗ'm for the overall reaction. c) For each mechanism, draw an energy...
Student Name: Instructor Name: EXP #4: POST-LAB 1. A proposed mechanism for the iodine clock reaction is shown below: Iodine Clock Reaction Mechanism: 1 HSoS0+HIO2 ki-2.95 x 10-1M-'s-1 2-2.0 x 1010 AM-2s-1 ka 1.0 x 105 M-'s-1 ka-3.0 x 105 M-3s-1 HIO2+I +H+2HOI HIO2+ HOI IO +I + 2H+ IO I+2H HIO2 + HOI HOI+I+H I2+H20 ks 3.0 x 1012M-2s-1 I+ H20 HOI+ I +H ke -2.2s-1 I2+HSO+H20+21 +SO- +3H+ -1.0 x 100 M-1-1 where the values of k are...
can you solve and show work if possible
Question 5 9 pts For the following mechanism: Step 1: 2A -----> B (fast) Step 2: B + C -----> 2D (slow) a) What is the predicted rate law (not using intermediates)? [Select] b) What is the overall reaction? (Select] c) How would adding a catalyst affect this reaction? (Select]
2 H2O2(aq) + 2 H2O(l) + O2(g) 5. Hydrogen peroxide decomposes according to the equation above. a. An aqueous solution of H2O, that is 6.00 percent H,O, by mass has a density of 1.03 g ml. Calculate each of the following. (i) The original number of moles of H2O, in a 125 ml sample of the 6.00 percent H2O2 solution (ii) The number of moles of O,(g) that are produced when all of the H2O2 in the 125 mL sample...