1The gas phase reaction of chloroform is described by the following equation, experimentalrate law and proposed mechanism.(a.) Does this proposed mechanism agree with the overall reaction?(b.) What intermediates are present in this reaction?(c.) Does the experimental rate law agree with the mechanism provided?(d.) Write the overall reaction rate constant in terms of the rate constants of the elementarysteps.NOTE: The rate law should have Cl2 not Cl in the brackets. The experimental rate law will bek[C12]^(1/2)[CHC13]. Please make this correction. (Non-anonymous questionO)(20 Points)%3DOverall Reaction: Cl2(g) + CHCI3(g) → HCI(g) + CCl4(g)Experimental Rate Law = k[CI]!/2[CHCI3]Proposed Mechanism:1. Cl2(g) E→ 2CI(g)2. Cl(g) + CHCI3(g) → HCI(g) + CCI3(g)3. Cl3(g) + Cl(g) →CCI«(g)fastslowfast

Here we have to determine the overall reaction from the mechanism of reactions, intermediate in…

Overall Reaction: Cl2(g) + CHCI3(g) → HCI(g) + CCl«(g) Experimental Rate Law = k[CI]!/2[CHCI3] Proposed Mechanism: 1. C2(g) E→ 2CI(g) 2. Cl(g) + CHCI3(g) → HCI(g) + CCI3(g) 3. Cla(g) + Cl(g) →Cla(g) fast slow fast

Overall Reaction: Cl2(g) + CHCI3(g) → HCI(g) + CCl«(g) Experimental Rate Law = k[CI]!/2[CHCI3] Proposed Mechanism: 1. C2(g) E→ 2CI(g) 2. Cl(g) + CHCI3(g) → HCI(g) + CCI3(g) 3. Cla(g) + Cl(g) →Cla(g) fast slow fast

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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Question

1
The gas phase reaction of chloroform is described by the following equation, experimental
rate law and proposed mechanism.
(a.) Does this proposed mechanism agree with the overall reaction?
(b.) What intermediates are present in this reaction?
(c.) Does the experimental rate law agree with the mechanism provided?
(d.) Write the overall reaction rate constant in terms of the rate constants of the elementary
steps.
NOTE: The rate law should have Cl2 not Cl in the brackets. The experimental rate law will be
k[C12]^(1/2)[CHC13]. Please make this correction. (Non-anonymous questionO)
(20 Points)
%3D
Overall Reaction: Cl2(g) + CHCI3(g) → HCI(g) + CCl4(g)
Experimental Rate Law = k[CI]!/2[CHCI3]
Proposed Mechanism:
1. Cl2(g) E→ 2CI(g)
2. Cl(g) + CHCI3(g) → HCI(g) + CCI3(g)
3. Cl3(g) + Cl(g) →CCI«(g)
fast
slow
fast

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