The following mechanism has been proposed for the conversion of tert-butyl bromide to tert-butyl alcohol in aqueous solution: step 1 slow: (CH3)3CB → (CH3)3C+ + Br step 2 fast: (CH3)3C+ + OH" → (CH3)3COH (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]™[B]"... , where '1' is understood (so don't write it) for m, n etc.) Rate =

The following mechanism has been proposed for the conversion of tert-butyl bromide to tert-butyl alcohol in aqueous solution: step 1 slow: (CH3)3CB → (CH3)3C+ + Br step 2 fast: (CH3)3C+ + OH" → (CH3)3COH (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]™[B]"... , where '1' is understood (so don't write it) for m, n etc.) Rate =

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 25QRT

See similar textbooks

Similar questions

I monitor the reaction of Compound B with a large excess of NaOH at 298 K, and get the following results for its absorbance over time: Time (seconds) Absorbance (no units) 0 0.4555 10 0.3857 20 0.3178 30 0.2457 40 0.2011 50 0.1798 60 0.1304 On the basis of these numbers and a spreadsheet program, answer the following question: What is the most-likely order of Compound B in its reaction with NaOH? a. 0 b. 4 c. 1 d. 3 e. 2
The following mechanism has been proposed for the conversion of tert-butyl bromide to tert-butyl alcohol in aqueous solution: step 1 : (CH3)3CBr (CH3)3C+ + Br- step 2 : (CH3)3C+ + OH- (CH3)3COH(a) Identify the molecularity of each step in the mechanism.step 1 _________ (unimolecularbimoleculartermolecular) step 2 _________ (unimolecularbimoleculartermolecular) (b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leave it blank._______+________>________+_________(c) Identify any intemediates in this mechanism. Intermediate: Enter formula. ________ If none, leave box blank: fill in the blanks
The rate law for the reaction of phenolphthalein with NaOH was determined to be Rate = k[P2−][OH−]. What are the units on the value of the rate constant, k?
The bromination of aceton is acid –catalyzed. CH3COCH3 + Br2 + H+ ---------> CH3COCH2Br + 2H+ + Br- The rate of disappearance of bromine was measured for several different concentrations of acetone, bromine, and H+ ion at a certain temperature. A B C [ CH3COCH3] [Br2] [ H+] Rate of disapperance [ Br2] 0.30 0.050 0.050 5.7 x 10 -5 0.30 0.10 0.050 5.7 x 10 –5 0.30 0.050 0.10 1.2 x 10 -4 0.40 0.050 0.20 3.1 x 10 -4 Write the rate law. Find the rate constant. Determine the half-life of the reaction if the [A]o = 0.50M ; [B]o = 0.40 M; [C]o = 0.6 M. ( Half-life is based on over all order of the reacaction)
The first-order rate constant, k1, for the decomposition of ampicillin at pH 5.8 and 35?C is k1 = 2 × 10-7 sec-1. The solubility of ampicillin is 1.1 g/100 mL. If it is desired to prepare a suspension of the drug containing 2.5 g/100 mL, calculate the zero-order rate constant, k0, and the shelf-life, that is, the time in days required for the drug to decompose to 90% of its original concentration (at 35?C) in solution. Note: 100 mL = 1 deciliter = 1 dL.
2A -> A2 (Fast) A2 + B= A2B (slow) predict the rate law from the following two step mechanism
A woman is admitted to hospital after a drug overdose. The drug's half life is 7.2 hours. A toxic plasma concentration of 264 milligrams/ml is recorded. After 72 hours, what would you expect the plasma concentration in microg/ml of the drug to be? (You may assume that the distribution is complete and that the elimination is described by a first-order process.) Answer to 1 dp. microg/ml
An irreversible unimolecular reaction (A -> B) has a rate constant (k) equal to 0.46 s-1. What is the half-time (t1/2)? If at time “zero” the concentration of A is 28 mM, what is the concentration at 1.5 seconds? At 2.17 seconds? Specify your units. t1/2 = [A] at t1/2 = [A] = at t = 2.17 s
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
Distinguish between the differential rate law and the integrated rate law. Which of these is often called just the rate law? What is k in a rate law, and what are orders in a rate law? Explain.
Calculate the time (min)required for a first-order reaction A -> Product to be 64.9% completed, knowing that the half lifetime t 1/2 is 206 min
Consider the following mechanism: Just C (1) ClO−(aq) + H2O(l) ⇌ 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? Select the single best answer. ClO−(aq) + I−(aq) ⇌ IO−(aq) + Cl−(aq) (b) Identify the intermediate(s), if any. Select the single best answer. HClO, OH−, HIO (c) What are the molecularity and the rate law for each step? Select the single best answers. (1): unimolecular bimolecular termolecular rate = k1([HClO][OH−])/([HClO][OH−]) k1[ClO−][H2O] k1[HClO][OH−] (2): unimolecular bimolecular termolecular rate = k2[I−][HClO] k2([HIO][Cl−])/([I−][HClO]) k2[HIO][Cl−] (3): unimolecular bimolecular termolecular rate =…