Consider the proposed mechanism for the reaction, CHCI3(g) + Cl2(g) HCI(g) + CCI4(g) --> (1 - fast) Cl2(g) = 2 CI(g) (2 - slow) CI(g) + CHCI3(g) HCI(g) + CCI3(g) --> (3 - fast) CI(g) + CCI3(g) --> A student proposes that the reaction rate law is rate = k [CI] [CHCI3]. Why is this incorrect? %3D (Choose the best answer.) The student's proposed rate law is not based on the rate-determining step in the mechanism. The rate orders with respect to Cl and CHCI3 match the stoichiometric coefficients for these compounds in step (2). It is always the last step in a mechanism that determines the rate law and CHCI3 is not in step (3). Clis in the proposed rate law. CI is an intermediate and only reactants and products that appear in the ove reaction equation may be in the reaction rate law.
Consider the proposed mechanism for the reaction, CHCI3(g) + Cl2(g) HCI(g) + CCI4(g) --> (1 - fast) Cl2(g) = 2 CI(g) (2 - slow) CI(g) + CHCI3(g) HCI(g) + CCI3(g) --> (3 - fast) CI(g) + CCI3(g) --> A student proposes that the reaction rate law is rate = k [CI] [CHCI3]. Why is this incorrect? %3D (Choose the best answer.) The student's proposed rate law is not based on the rate-determining step in the mechanism. The rate orders with respect to Cl and CHCI3 match the stoichiometric coefficients for these compounds in step (2). It is always the last step in a mechanism that determines the rate law and CHCI3 is not in step (3). Clis in the proposed rate law. CI is an intermediate and only reactants and products that appear in the ove reaction equation may be in the reaction rate law.
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
Related questions
Question
![Consider the proposed mechanism for the reaction, CHCI3(g) + Cl2(g)
HCI(g) + CCI4(g)
-->
(1 - fast) Cl2(g) = 2 CI(g)
(2 - slow) CI(g) + CHCI3(g)
HCI(g) + CCI3(g)
-->
(3 - fast) CI(g) + CCI3(g)
-->
A student proposes that the reaction rate law is rate = k [CI] [CHCI3]. Why is this incorrect?
%3D
(Choose the best answer.)
The student's proposed rate law is not based on the rate-determining step in the mechanism.
The rate orders with respect to Cl and CHCI3 match the stoichiometric coefficients for these compounds in
step (2).
It is always the last step in a mechanism that determines the rate law and CHCI3 is not in step (3).
Clis in the proposed rate law. CI is an intermediate and only reactants and products that appear in the ove
reaction equation may be in the reaction rate law.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F74279ea1-eff5-4403-94c6-eaa833f0d034%2Faf64b6c7-c8e5-4edb-98cb-a3e09b369484%2Fplzlbca.png&w=3840&q=75)
Transcribed Image Text:Consider the proposed mechanism for the reaction, CHCI3(g) + Cl2(g)
HCI(g) + CCI4(g)
-->
(1 - fast) Cl2(g) = 2 CI(g)
(2 - slow) CI(g) + CHCI3(g)
HCI(g) + CCI3(g)
-->
(3 - fast) CI(g) + CCI3(g)
-->
A student proposes that the reaction rate law is rate = k [CI] [CHCI3]. Why is this incorrect?
%3D
(Choose the best answer.)
The student's proposed rate law is not based on the rate-determining step in the mechanism.
The rate orders with respect to Cl and CHCI3 match the stoichiometric coefficients for these compounds in
step (2).
It is always the last step in a mechanism that determines the rate law and CHCI3 is not in step (3).
Clis in the proposed rate law. CI is an intermediate and only reactants and products that appear in the ove
reaction equation may be in the reaction rate law.
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