The following mechanism has been proposed for the conversion of tert-butyl bromide to tert-butyl alcohol in aqueous solution: step 1 slow: (CH3)3CBr (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 blar + + (2) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (3) 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)3CBr (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 blar + + (2) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (3) 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 & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions

Section: Chapter Questions

Problem 86IL: The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common...

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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
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1. The following data were collected from the alkaline hydrolysis reaction of t-butylbromide to t-butyl alcohol as: (CH3)3CBr à alkaline hydrolysis à (CH3)3COH a. At concentration 0.5 M the rate was 0.005 (mol/L.s) b. At concentration 1.5 M the rate was 0.015 (mol/L.s) If you know that: Rate2 / Rate1 = ([A2] / [A1])m Find out the followings: a. The reaction order b. The reaction constant c. The half-life of the reaction.
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.
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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)
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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 =…
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.