4. The decomposition of acetaldehyde (CH3CHO) to methane and carbon monoxide is an example of a free radical chain reaction. The overall reaction is believed to occur through the following sequence of steps: k1 CH3CHO + CHз * +CНО * k2 CH3CНО + CH3 * CH4 + CH3CО * k3 CH3CO * - CO + CH3 * k4 CH3 * +CH3 * → C2H6 Free radical species are indicated by the * symbol. In this case, the free radical CHO * that is generated in the first reaction is kinetically insignificant and thus you can ignore this d[CH,] « ([CH,CнO])3/2 holds. substance. According to the experimental observation, Using the steady state approximation, derive the 3/2 order relation of this reaction and find the rate constant K in ICH, = K([CH3CHO])³/2. NOTE: The final reaction is a second order reaction. dlCaHel = -2k4[CH3 +]? dt dt dt

4. The decomposition of acetaldehyde (CH3CHO) to methane and carbon monoxide is an example of a free radical chain reaction. The overall reaction is believed to occur through the following sequence of steps: k1 CH3CHO + CHз * +CНО * k2 CH3CНО + CH3 * CH4 + CH3CО * k3 CH3CO * - CO + CH3 * k4 CH3 * +CH3 * → C2H6 Free radical species are indicated by the * symbol. In this case, the free radical CHO * that is generated in the first reaction is kinetically insignificant and thus you can ignore this d[CH,] « ([CH,CнO])3/2 holds. substance. According to the experimental observation, Using the steady state approximation, derive the 3/2 order relation of this reaction and find the rate constant K in ICH, = K([CH3CHO])³/2. NOTE: The final reaction is a second order reaction. dlCaHel = -2k4[CH3 +]? dt dt dt

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Q2: Nitramide decomposes in water according to the chemical equation, kobs N₂O + H₂O 0,N-NH, The observed rate law is the following, The proposed mechanism is: O,N-NH, = 1² +11 d[N₂0] dt = kobs [0,N – NH2] [H+] O,N-NH + H* N₂O O,N-NH H* + OH H₂O Fast Is the reaction mechanism consistent with the observed rate law? If so, what is the relationship between kobs and the rate constants of the individual steps? Fast Equilibrium + он Slow
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A kinetic study yielded the following reaction rate data: The reaction mechanism is Experiment Number Initial Concentrations [HO] Initial Rate of Disappearance of R-Br and Formation of R-OH [R-Br] 0.50 0.50 0.25 0.25 1.00 0.50 2 0.50 0.25 0.25 SN2 SN1 O No reaction will occur E1 E2 curfor the following reaction
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