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Consider the following reaction mechanism for the addition of HCl to propene in the gas hase. The overall reaction is just HCl + CH;CH=CH2 → CH;CH2CH3, but the experimentally bserved rate law is more complicated than that stoichiometry would suggest. 2 HCI (HCI)2 kz HCl + CH3CH = CH2 2 complex k-2 (НC)2 + compleх + сн,CHCICH, Here (HCl)2 is an HCl dimer and “complex" represents some intermediate species of

Consider the following reaction mechanism for the addition of HCl to propene in the gas hase. The overall reaction is just HCl + CH;CH=CH2 → CH;CH2CH3, but the experimentally bserved rate law is more complicated than that stoichiometry would suggest. 2 HCI (HCI)2 kz HCl + CH3CH = CH2 2 complex k-2 (НC)2 + compleх + сн,CHCICH, Here (HCl)2 is an HCl dimer and “complex" represents some intermediate species of

Chemistry: The Molecular Science
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
Section11.7: Reaction Mechanisms
Problem 11.12E
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Consider the following reaction mechanism for the addition of HCl to propene in the gas phase. The overall reaction is just HCI + CH3CH=CH2 → CH;CH2CH3, but the experimentally observed rate law is more complicated than that stoichiometry would suggest. 2 HCl 2 (HCI), k_1 k2 HCI + CH3CH = CH, 2 complex k_2 (HCI)2 + complex → CH3CHCICH3 (Here (HCl)2 is an HCl dimer and “complex" represents some intermediate species of unknown structure.) Assume that the third step is rate determining, and that the first two steps both remain in equilibrium throughout the reaction. d[CH;CHCICH3] Please write Derive an expression for the rate of formation of CH3CHCICH,' dt your final expression in the boxes. HINT: Be sure to use the equilibrium assumption, and not the steady state approximation. Your final rate law should NOT include the concentrations of any intermediates.
Transcribed Image Text:Consider the following reaction mechanism for the addition of HCl to propene in the gas phase. The overall reaction is just HCI + CH3CH=CH2 → CH;CH2CH3, but the experimentally observed rate law is more complicated than that stoichiometry would suggest. 2 HCl 2 (HCI), k_1 k2 HCI + CH3CH = CH, 2 complex k_2 (HCI)2 + complex → CH3CHCICH3 (Here (HCl)2 is an HCl dimer and “complex" represents some intermediate species of unknown structure.) Assume that the third step is rate determining, and that the first two steps both remain in equilibrium throughout the reaction. d[CH;CHCICH3] Please write Derive an expression for the rate of formation of CH3CHCICH,' dt your final expression in the boxes. HINT: Be sure to use the equilibrium assumption, and not the steady state approximation. Your final rate law should NOT include the concentrations of any intermediates.
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