Step 1) 2) 3) 4) 5) 6) CI-CI hv CH₂ + Cl CH3 + CI-CI ci + CH3 CH3 + CH3 ci + ci 2 CI* of the mechanism steps shown is the rate-determining step for the chlorination of methane. CH3 + HCI CH3Cl + Ci CH3CI CH3CH3 CI-CI

Step 1) 2) 3) 4) 5) 6) CI-CI hv CH₂ + Cl CH3 + CI-CI ci + CH3 CH3 + CH3 ci + ci 2 CI* of the mechanism steps shown is the rate-determining step for the chlorination of methane. CH3 + HCI CH3Cl + Ci CH3CI CH3CH3 CI-CI

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter13: Substitution

Section: Chapter Questions

Problem 43CTQ

See similar textbooks

Similar questions

a) Sketch the energy diagram for the conversion of tertiary butyl bromide to methyl t-butyl ether. Note that this is a two step reaction with the t-butyl cation as an intermediate. Assume that this is overall an exothermic reaction. Show the location of both transition states and the intermediate. The first step has the higher energy of activation and is the rate determining step. (CH3)3C-Br ------> (CH3)3C+ + Br- (CH3)3C+ + H3CO- ------> (CH3)3C-O-CH3 (b)Draw the curved arrow mechanism and the transition state when the tertiary butyl carbocation reacts with the methoxide ion to give an ether. (CH3)3C+ + H3CO- ------> (CH3)3C-O-CH3
2- Write step-by-step mechanism for the following reaction: Cul R1 но .*...... ....... ........
For the gas phase isomerization of isopropenyl allyl ether, CH2=C(CH3)-O-CH2CH=CH2-->CH3COCH2CH2CH=CH2 the rate constant at 405 K is 2.60x10^-5 s^-1 and the rate constant at 440. K is 4.75x10^-4 s^-1. The activation energy for the gas phase isomerization of isopropenyl allyl ether is ________ kJ.
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)
Complete all steps
Acetic anhydride reacts with water in the following manner: CH3C(O)-O-C(O)CH3 + H2O = 2CH3CO2 If this reaction is carried out in an inert solvent with low concentrations of both acetic anhydride and water, it follows the rate law rate = k [CH3C(O)-O-C(O)CH3] [H2O] with a rate constant of 0.0035 s-1. However, if low concentrations of acetic anhydride are placed in pure water, it follows the rate law rate = K [CH3C(O)-O-C(O)CH3] where K = 0.1944 s-1. Explain why this is happening.
what is the rate at which Br- (aq) disppears in reaction below if the rate of disappearence of BrO3- (aq) is 0.022 M/s
Rate data were collected for the following reaction at a particular temperature. (C2H5)2(NH)2 + 12 = (C2H5)2N2 + 2HI Expt Initial [(C2H5)2(NH)2], Initial [12], mol/L Reaction Rate, Ms-1 mol/L 1 0.10 0.10 0.0090 2 0.20 0.10 0.036 3 0.10 0.20 0.018 0.10 0.30 0.027 Write the overall rate law expression and determine the order of reaction of (a) (C₂H5)2(NH)2, (b) 12, (c) overall order of reaction, and (d) the rate constant.
The decomposition of di-2-methylpropan-2-yl peroxide produces propanone and ethane: (CH3)3COOC(CH3)3 → 2CH3COCH3 + C₂H6 and is described by the generally accepted mechanism: (CH3)3COOC(CH3)3 → 2 (CH3)3CO (CH3)3CO → CH3COCH3 + CH3* CH3 + CH3 →→ C₂H6 k₁ k₂ k3 1. Identify the intermediates. 2. Explain why this is NOT a chain reaction. 3. Confirm using the steady state approximation that the production of ethane is first order even though it takes place in a number of steps.
VI. The rate of the reaction (CH3)3CCI + NaSCH2CH3 → (CH3)2C=CH2 + CH3CH2SH + NaCl is first-order in (CH3)3CCI and first-order in NaSCH₂CH3. Please draw the rate- limiting step of the reaction, using curved arrows to show the flow of electrons. If any lone pairs are involved in a reaction, their involvement must be explicitly shown. ( 20
Below is the equation for a nucleophilic substitution reaction and some experimental data. CH3CH2Br + CH3COO- ⇌ CH3CH2CO2CH3 + Br- ΔH=-75 kJ/mol Rate = k [CH3CH2Br][CH3COO-] Which reaction energy profile would be the best representative of the data provided?
A mechanism that has been proposed for the conversion of 2-methylpropene to tert-butyl alcohol in acidic aqueous solution is: step 1 slow: (CH3)2C=CH2 + H+ --------> (CH3)3C+ step 2 fast: (CH3)3C+ + H2O ---------> (CH3)3COH + H+ (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]m[B]n... , where '1' is understood (so don't write it) for m, n etc.) Rate = _______________