O 11.The decomposition of ozone in the upper atmosphere to dioxygen occurs by a two-step mechanism.The first step is a fast reversible step and the second is a slow reaction between an oxygen atom andan ozone molecule:Step 1:Step 2:O3(g) = 02(8) + O(g)O3(g) + 0(g) → 202(g)Fast, reversible, reactionSlowa. Which is the rate determining step?b. Write the rate equation for the rate-determining step.Write the rate equation for the overall reaction.с.The rate equation for the reaction of nitrogen dioxide and carbon monoxide in the gas state to formcarbon dioxide and nitric oxide is represented by the equation:12.NO2(g) + CO(g) → NO(g) + CO2(g)The following data were collected at 125°C:eExperiment 1Experiment 2Experiment 3Initial [NO2]mol L5.0 x 1045.0 x 1041.5 x 10-3Initial [CO]mol L-1.6 x 10-23.2 x 1023.2 x 10-2Initial ratemol L'min1.7 x 10-71.7 x 10-71.5 x 10-6What is the order with respect to NO2?b. What is the order with respect to CO?c. What is the overall order of the reaction?d. Write the rate equation.e. How do you know this is not a single step reaction?a.oil boniside stow ssb gniwolkle

The chemical kinetics of the reaction gives us an idea about the speed of reaction that means how…

he decomposition of ozone in the upper atmosphere to dioxygen occurs - he first step is a fast reversible step and the second is a slow reaction between an ozone molecule: Step 1: Step 2: O3(g) = 02(g) + O(g) O3(g) + 0(g) → 202(g) Fast, reversible, rea Slow

he decomposition of ozone in the upper atmosphere to dioxygen occurs - he first step is a fast reversible step and the second is a slow reaction between an ozone molecule: Step 1: Step 2: O3(g) = 02(g) + O(g) O3(g) + 0(g) → 202(g) Fast, reversible, rea Slow

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

100%

O 11.
The decomposition of ozone in the upper atmosphere to dioxygen occurs by a two-step mechanism.
The first step is a fast reversible step and the second is a slow reaction between an oxygen atom and
an ozone molecule:
Step 1:
Step 2:
O3(g) = 02(8) + O(g)
O3(g) + 0(g) → 202(g)
Fast, reversible, reaction
Slow
a. Which is the rate determining step?
b. Write the rate equation for the rate-determining step.
Write the rate equation for the overall reaction.
с.
The rate equation for the reaction of nitrogen dioxide and carbon monoxide in the gas state to form
carbon dioxide and nitric oxide is represented by the equation:
12.
NO2(g) + CO(g) → NO(g) + CO2(g)
The following data were collected at 125°C:e
Experiment 1
Experiment 2
Experiment 3
Initial [NO2]
mol L
5.0 x 104
5.0 x 104
1.5 x 10-3
Initial [CO]
mol L-
1.6 x 10-2
3.2 x 102
3.2 x 10-2
Initial rate
mol L'min
1.7 x 10-7
1.7 x 10-7
1.5 x 10-6
What is the order with respect to NO2?
b. What is the order with respect to CO?
c. What is the overall order of the reaction?
d. Write the rate equation.
e. How do you know this is not a single step reaction?
a.
oil boniside stow ssb gniwolkle

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