The mechanism for the reaction between 2-chloroethanol , CH2CICH2OH, and hydroxide ions in aqueous solution to form ethylene oxide, (CH2CH2)O, is thought to consist of two steps(1) CH2CICH2OH + OH-= CH2CICH2O- + H2O fast(2) CH2CICH2O- = (CH2CH2)O + CI- slowShow that, for this mechanism, the rate of formation of ethylene oxide is Rate= k2 K[CH2CICH2OH][OH-] where K is the equilibrium constant for the first step and k2 is the rate constant for the second step.
The mechanism for the reaction between 2-chloroethanol , CH2CICH2OH, and hydroxide ions in aqueous solution to form ethylene oxide, (CH2CH2)O, is thought to consist of two steps(1) CH2CICH2OH + OH-= CH2CICH2O- + H2O fast(2) CH2CICH2O- = (CH2CH2)O + CI- slowShow that, for this mechanism, the rate of formation of ethylene oxide is Rate= k2 K[CH2CICH2OH][OH-] where K is the equilibrium constant for the first step and k2 is the rate constant for the second step.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter13: Chemical Kinetics
Section: Chapter Questions
Problem 13.50QE
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The mechanism for the reaction between 2-chloroethanol , CH2CICH2OH, and hydroxide ions in aqueous solution to form ethylene oxide, (CH2CH2)O, is thought to consist of two steps
(1) CH2CICH2OH + OH-= CH2CICH2O- + H2O fast
(2) CH2CICH2O- = (CH2CH2)O + CI- slow
Show that, for this mechanism, the rate of formation of ethylene oxide is
Rate= k2 K[CH2CICH2OH][OH-]
where K is the equilibrium constant for the first step and k2 is the rate constant for the second step.
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