The gas-phase decomposition of acetaldehyde can be represented by the overall chemical equation CH,CНO — СН, + СО It is thought to occur through the sequence of reactions CH-CHO — СH, + CHO CHs + CH:CHO — CHн: + CH:CHно CH-CHO — СО + CH, CH; + CH3 → CH;CH; Show that this reaction mechanism corresponds to a chain reaction, and identify the initiation, propagation, and ter- mination steps.

The gas-phase decomposition of acetaldehyde can be represented by the overall chemical equation CH,CНO — СН, + СО It is thought to occur through the sequence of reactions CH-CHO — СH, + CHO CHs + CH:CHO — CHн: + CH:CHно CH-CHO — СО + CH, CH; + CH3 → CH;CH; Show that this reaction mechanism corresponds to a chain reaction, and identify the initiation, propagation, and ter- mination steps.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.49PAE: The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by...

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List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.
The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.
The conversion of high molecular weight olefins into saturated hydrocarbons makes use ofH 2 and is a heterogeneous process catalyzed by nickel. Draw and describe the mechanismaccording to the LH mechanism.
Suppose that, in the absence of a catalyst, a certain biochemicalreaction occurs x times per second at normal bodytemperature (37 °C). In order to be physiologically useful,the reaction needs to occur 5000 times faster than when itis uncatalyzed. By how many kJ>mol must an enzyme lowerthe activation energy of the reaction to make it useful?
Calculate the magnitude of the diffusion-controlled rate constant at 320 K for the recombination of two atoms in water, for which η = 0.89 cP. Assuming the concentration of the reacting species is 1.5 mmol dm−3 initially, how long does it take for the concentration of the atoms to fall to half that value? Assume the reaction is elementary.
The ha lf-l ife of pyruvic acid in the presence of an aminotransferaseenzyme (which converts it to alanine) was found to be 221 s. How long will it take for the concentration of pyruvic acid to fal l to 1/ 64 of its in it ial va lue in th is first-order reaction?
Suggest a plausible mechanism for this reaction that is consistent with the rate law.
Q1.Differentiate between homogenous and heterogeneous catalysis with suitable examples Q2. What are the basic rules use for the nomenclature of co-ordination compounds?
The equilibrium constant for the binding of a drug molecule to a protein was measured as 200. In a separate experiment, the rate constant for the binding process, which is second order overall, was found to be 1.5 × 108 dm3 mol–1 s–1. What is the rate constant for the first-order dissociation of the drug molecule from the protein–drug complex?
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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.
It has been found that in acid solution (greater than 1M H3O+) the rate expression rate for the reaction of H2O2 with I- is of the form : rate= k2[H2O2][I-][H3O+], where k2 = .25L2*mol-2*s-1 at 25C. Therefore, the rate law over the whole range of acidity from very acid solutions to a neatural solution is given be a two-term rate expression: rate = k1[H2O2][I-] + K2[H2O][I-][H3O+] Where K1 has the value of .0115L*mol-1*s-1 at 25C. Compare the relative magnitudes of these two terms under the conditions employed in your rate measurements for mixture 1. ( you should find what that the second term makes a negligible contribution to the reaction rate at H3O+ smaller than 3 x 10 -4) mixture 1 concentrations H2O2 = 5.3 x10-5 I- = 8.3 x 10 -6 H3O = 10-5