1. indicate the activation energy for the overall reaction on the graph. (You may want to use a line for the sake of clarity.)2. Write the elementary reactions that make up the reaction mechanism. 3. What would you propose as the rate law for this reaction? 4. Of course, this proposed law is hypothetical. Using the following data collected experimentally (probably using a UV/vis spectrometer J), determine the rate law for this reaction. Include reaction order and the value and units for k. Please show your work, including any graphs you make. (Note: no credit will be given to correct final answers without supporting work.) Does your experimental rate law match the one you proposed above? Let's spend some time with this reaction of NO2, an important compound in atmosphericchemistry (it's a pollutant and contributes to the formation of acid rain), in manufacturingexplosives, and in fueling rockets:2NO,(g) – 2NO(g) + 0,(g)It follows this reaction mechanism:NO,+NO2NO+0,2NO,Progress of reaction1. Indicate the activation energy for the overall reaction on the graph. (You may want touse a line for the sake of clarity.)2. Write the elementary reactions that make up the reaction mechanism.3. What would you propose as the rate law for this reaction?4. Of course, this proposed law is hypothetical. Using the following data collectedexperimentally (probably using a UV/vis spectrometer O), determine the rate law forthis reaction. Include reaction order and the value and units for k. Please show yourwork, including any graphs you make. (Note: no credit will be given to correct finalanswers without supporting work.) Does your experimental rate law match the one youproposed above?Time (s) [NO.), M1.00x10-2606.83x10-31205.18x10-31804.18x10-32403.50x10-33003.01x10-3Energy

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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

Section: Chapter Questions

Problem 11.ACP: (Section 11-5) A rule of thumb is that for a typical reaction, if concentrations are unchanged, a...

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1. indicate the activation energy for the overall reaction on the graph. (You may want to
use a line for the sake of clarity.)
2. Write the elementary reactions that make up the reaction mechanism.
3. What would you propose as the rate law for this reaction?
4. Of course, this proposed law is hypothetical. Using the following data collected
experimentally (probably using a UV/vis spectrometer J), determine the rate law for
this reaction. Include reaction order and the value and units for k. Please show your
work, including any graphs you make. (Note: no credit will be given to correct final
answers without supporting work.) Does your experimental rate law match the one you
proposed above?

Let's spend some time with this reaction of NO2, an important compound in atmospheric
chemistry (it's a pollutant and contributes to the formation of acid rain), in manufacturing
explosives, and in fueling rockets:
2NO,(g) – 2NO(g) + 0,(g)
It follows this reaction mechanism:
NO,+NO
2NO+0,
2NO,
Progress of reaction
1. Indicate the activation energy for the overall reaction on the graph. (You may want to
use a line for the sake of clarity.)
2. Write the elementary reactions that make up the reaction mechanism.
3. What would you propose as the rate law for this reaction?
4. Of course, this proposed law is hypothetical. Using the following data collected
experimentally (probably using a UV/vis spectrometer O), determine the rate law for
this reaction. Include reaction order and the value and units for k. Please show your
work, including any graphs you make. (Note: no credit will be given to correct final
answers without supporting work.) Does your experimental rate law match the one you
proposed above?
Time (s) [NO.), M
1.00x10-2
60
6.83x10-3
120
5.18x10-3
180
4.18x10-3
240
3.50x10-3
300
3.01x10-3
Energy

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