Be sure to answer all parts.The bromination of acetone is acid-catalyzed:H*CH,COCH, + Br;CH,COCH,Br +H + BrcatalystThe rate of disappearance of bromine was measured for several different concentrations of acetone,bromine, and H ions at a certain temperature:Rate ofICH,COCH, Brz(M)Disappearanceof Br (M/s)(M)(M)(1) 0.6500.0650 0.0650 5.91 x 105(2) 0.6500.130 0.0650 5.91 x 10 5(3) 0.6500.0650 0.130 1.18 x 10(4) 0.8650.0650 0.260 3.14 x 10(5) 0.8650.0650 0.0650 7.86 x 105(a) What is the rate law for the reaction?O rate-k[CH,COCH,(Br3l(H']rate=k[CH,COCH,lIBr2|[H*)O rate=k[CH,COCH,J[BrH"]O rate-k{CH3COCH,J[Br2|[H?rate=k(CH,COCH,l[Br,l[H (a) What is the rate law for the reaction?O rate=k[CH,COCHJ [Br3l*[H*]O rate=k[CH,COCH,J [Brzl[H]O rate=k[CH,COCH;][Br2l(H")O rate=k[CH;COCH3][Br2|(H')?O rate=k[CH,COCH,][Br2][H"]okrate=k[CH,COCH3][Br2]rate=k[CH,COCH,|[H)itO rate=k[Br2][H]ncesO rate=k[CH;COCH3]rate=k[Br2]rate=k[H"](b) Determine the rate constant using the data from experiment (1). Report your answer to 3significant figures.k =O O

Answered: Image /qna-images/answer/c384e7d6-d573-456b-a930-14f9180c3413.jpg

The bromination of acetone is acid-catalyzed: CH,COCH, + Br, CH,COCH,Br+ H + Br catalyst The rate of disappearance of bromine was measured for several different concentrations of acetone, bromine, and H ions at a certain temperature: Rate of ICH,COCH, Br2 Disappearance of Br3(M/s) (M) (M) (M) (1) 0.650 0.0650 0.0650 5.91 x 105 (2) 0.650 0.130 0.0650 5.91 x 105 (3) 0.650 0.0650 0.130 1.18 x 104 (4) 0.865 0.0650 0.260 3.14 x 104 (5) 0.865 0.0650 0.0650 7.86 x 10 5 (a) What is the rate law for the reaction? rate-k[CH,COCH,'IBrH") O rate-k(CH,COCH,J'IBr2|[H') O rate-k[CH,COCH,|[Brl'IH') rate-k[CH,COCH,[Br|[H12 O rate-k[CH,COCH,[Br,l|H'1

The bromination of acetone is acid-catalyzed: CH,COCH, + Br, CH,COCH,Br+ H + Br catalyst The rate of disappearance of bromine was measured for several different concentrations of acetone, bromine, and H ions at a certain temperature: Rate of ICH,COCH, Br2 Disappearance of Br3(M/s) (M) (M) (M) (1) 0.650 0.0650 0.0650 5.91 x 105 (2) 0.650 0.130 0.0650 5.91 x 105 (3) 0.650 0.0650 0.130 1.18 x 104 (4) 0.865 0.0650 0.260 3.14 x 104 (5) 0.865 0.0650 0.0650 7.86 x 10 5 (a) What is the rate law for the reaction? rate-k[CH,COCH,'IBrH") O rate-k(CH,COCH,J'IBr2|[H') O rate-k[CH,COCH,|[Brl'IH') rate-k[CH,COCH,[Br|[H12 O rate-k[CH,COCH,[Br,l|H'1

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 11QRT

See similar textbooks

Similar questions

Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
11.41 For a drug to be effective in treating an illness, its levels in the bloodstream must be maintained for a period of time. One way to measure the level of a drug in the body is to measure its rate of appearance in the urine. The rate of excretion of penicillin is first order, with a half-life of about 30 min. If a person receives an injection of 25 mg of penicillin at t = 0, how much penicillin remains in the body after 3 hours?
In the nuclear industry, chlorine trifluoride is used to prepare uranium hexafluoride, a volatile compound of uranium used in the separation of uranium isotopes. Chlorine trifluoride is prepared by the reaction CI2(g)+3F2(g)2CIF3(g). Write the equation that relates the rate expressions for this reaction in terms of the disappearance of Cl2 and F2 and the formation of CIF3.
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.
For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
Nitroglycerine is an extremely sensitive explosive. In a series of carefully controlled experiments, samples of the explosive were heated to 160 C and their first-order decomposition studied. Determine the average rate constants for each experiment using the following data: Initial [C3H5N3O9] (M) 4.88 3.52 2.29 1.81 5.33 4.05 2.95 1.72 t (s) 300 300 300 300 180 180 180 180 %Decomposed 52.0 52.9 53.2 53.9 34.6 35.9 36.0 35.4
Describe how graphical methods can be used to determine the order of a reaction and its rate constant from a series of data that includes the concentration of A at varying times.
In the PhET Reactions under Options. (a) Leave the Initial Temperature at the default setting. Observe the reaction. Is the rate of reaction fast or slow? (b) Click Pause" and then Reset All, and then enter 15 molecules of A and 10 molecules of BC once again. Select Show Bonds" under Options. This time, increase the initial temperature until, on the graph, the total average energy line is completely above the potential energy curve. Describe what happens to the reaction.
For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.
What is the difference between average rate, initial rate, and instantaneous rate?
11.64 HBr is oxidized in the following reaction: 4 HBr(g) + O2(g) —• 2 H2O(g) + 2 Br,(g) A proposed mechanism is HBr + O2 -* HOOBr (slow) HOOBr + HBr — 2 HOBr (fast) HOBr + HBr — H2O + Bn (fast) Show that this mechanism can account for the correct stoichiometry. Identify all intermediates in this mechanism. What is the molecularity of each elementary’ step? Write the rate expression for each elementary' step. Identify the rate-determining step.