3A. Below are GC results from the two reactions described in the experiment. In each reaction, an alcohol (n-butanol or t-butanol) is reacted with a 1:1 molar ratio of chloride and bromide and the ratio of products is analyzed to determine the rate law and reaction mechanism by which the reaction proceeds. Use the GC results below to determine what mechanism reaction 1 and reaction 2 proceed by and write a brief analysis of why you came to this conclusion. What alcohol is the starting material for each reaction? What is the rate law for each reaction? (It is important that you look up the boiling points of the four products of these two reactions to determine which is the chloro and which is the bromo product in each GC chromatogram. Assume that the peaks are eluted from the GC in order of boiling point.) Intensity (PA) Intensity (PA) 500000 400000 300000 200000 100000 0 -100000 250000 200000 150000 100000 50000 0 -50000 0.5 1 2 1 1 2 Reaction 1 Peak Number Retention Time (min) Peak Area %) 3.899 4.912 Reaction 1 1.5 3 Time (min) 1 2 Reaction 2 4 2.5 2 Time (min) 3 32.358 67.642 3.5 Reaction 2 Peak Number Retention Time (min) Peak Area %) 2.231 51.126 3.428 48.874 5 4 6 4.5

3A. Below are GC results from the two reactions described in the experiment. In each reaction, an alcohol (n-butanol or t-butanol) is reacted with a 1:1 molar ratio of chloride and bromide and the ratio of products is analyzed to determine the rate law and reaction mechanism by which the reaction proceeds. Use the GC results below to determine what mechanism reaction 1 and reaction 2 proceed by and write a brief analysis of why you came to this conclusion. What alcohol is the starting material for each reaction? What is the rate law for each reaction? (It is important that you look up the boiling points of the four products of these two reactions to determine which is the chloro and which is the bromo product in each GC chromatogram. Assume that the peaks are eluted from the GC in order of boiling point.) Intensity (PA) Intensity (PA) 500000 400000 300000 200000 100000 0 -100000 250000 200000 150000 100000 50000 0 -50000 0.5 1 2 1 1 2 Reaction 1 Peak Number Retention Time (min) Peak Area %) 3.899 4.912 Reaction 1 1.5 3 Time (min) 1 2 Reaction 2 4 2.5 2 Time (min) 3 32.358 67.642 3.5 Reaction 2 Peak Number Retention Time (min) Peak Area %) 2.231 51.126 3.428 48.874 5 4 6 4.5

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter16: Reaction Rates

Section16.3: Reaction Rate Laws

Problem 25SSC

See similar textbooks

Similar questions

The kinetic isotope effect for the reaction between 4-methoxyphenylethyl bromide and sodium hydroxide in aqueous solution was determined as kí/kĎ = 6.4, at room temperature. Write a reaction mechanism that is consistent with this experimental observation and explain your choice. (D)H H(D) Br OH H₂O H(D) + H₂O (HOD) + Br¯
For the following reaction, if O2 is used up at a rate of 5.02Mhr, what is the rate of consumption of CH3OH+2CH3OH+3O2→2CO2+4H2O using three significant figures.
If needed for this question. 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);C* + Br step 2 fast: (CH3)3C* + OH" → (CH3);COH (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 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]m[B]"... , where 'l' 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 blank. + + (2) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: Rate = (3) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]m [B]¹..., where '1' is understood (so don't write it) for m, n etc.)
ΚΗ Consider the following reaction which has the observed kinetic isotope effect = 1.5. kD CY2 CY2 P -P....pt + + Cy2 Cy2 A) Draw a mechanism for this reaction and identify the type of reaction which is occurring.
In a typical laboratory setting, a reaction is carried out in a ventilated hood with air circulation provided by outside air. A student noticed that a reaction that gave a high yield of a product in winter gave a low yield of that same product in the summer, eventhough his technique did not change and the reagents and co centrations used were identical. What is a plausible explanation for the different yield?
Complete the following reaction: H3N:BF3 + BCl3 Write down and explain the possible reaction mechanism with the rate law for this SE1 reaction.
(3) Evaluate the following uses of catalysis in terms of the goals of green chemistry (it is up to you if you want to refer to the 12 Principles or just the more general goals proposed by Dr. Lipke). Identify benefits as well as possible downsides. 2 a. A catalytic process that uses O, to oxidize an organic substrate dissolved in hexanes as a solvent, replacing a previous process that required the use of pyridine-N-oxide as an oxidant. b. A catalytic process that allows organic plant matter to be broken down into small organic molecules that can be used to produce fuels and fine chemicals that would otherwise be made from petroleum. c. A catalytic process that uses a mercury salt to catalyze the oxidation of methane to a methanol derivative, circumventing 2 a more traditional route using H, and CO to produce methanol as an intermediate.
The photochemical chlorination of trichloromethane (chloroform, CHCl3) in the gas to give CCl4 has been found to follow the rate law d[CCl4]/dt = kr[Cl2]1/2Ia1/2. Devise a mechanism that leads to this rate law when the chlorine pressure is high.
centropy (randomness) 10. Arrange the following reactions in order of increasing AS value. 1. H₂(g) + F2(g) → 2HF(g) зд 2. NH4NO3(s) → N₂O(g) + 2H₂O() 19, 12, 15 3. (NH4)2Cr2O7(s) →→→ Cr2O3(s) + 4H₂O(l) + N₂(g) 1,1g, 25
a) The liquid phase reaction of tert-butyl alcohol (A) and hydrochloric acid (B) carried out isothermally in a flow system to form tert-butyl chloride (C) and water (D). The reaction was carried out under an excess of tert-butyl alcohol (CH3)3COH + HCI = (CH3)3CCI + H2O
What is the rate law expression for the reaction in sodium hydroxide and ethyl acetate? Trial NaOH CH3COOC2H5 Initial Condcutivity of NaOH Solution (uS/cm) Initial Rate (uS/cm)/s) 1 21 ml 2.1ml 1285 24.72 2 21 ml 2.1ml 2399 50.32 3 21 ml 2.1ml 1262 23.72