5) NO2(g), (a.k.a. smog! And I don't mean the dragon), reacts with and causes the decay of ozone. Determine the rate law and the value of k for the following reaction using the data provided. NO2(g) +03(g) → NO3(g) + O2(g) [NO2]i (M) [03]i (M) Initial Rate 0.10 0.33 1.42 0.10 0.66 0.25 0.66 2.84 7.10 FULL ANSWER: 6) A data for the reaction in #5 was from experiments performed at room temperature (assume 25 °C). The energy of activation of the reaction is 63 kJ/mole. Use the rate constant you determined above to discover rate constant at -3 °C, which is the temperature of the stratosphere. ANSWER:
5) NO2(g), (a.k.a. smog! And I don't mean the dragon), reacts with and causes the decay of ozone. Determine the rate law and the value of k for the following reaction using the data provided. NO2(g) +03(g) → NO3(g) + O2(g) [NO2]i (M) [03]i (M) Initial Rate 0.10 0.33 1.42 0.10 0.66 0.25 0.66 2.84 7.10 FULL ANSWER: 6) A data for the reaction in #5 was from experiments performed at room temperature (assume 25 °C). The energy of activation of the reaction is 63 kJ/mole. Use the rate constant you determined above to discover rate constant at -3 °C, which is the temperature of the stratosphere. ANSWER:
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
![5) NO2(g), (a.k.a. smog! And I don't mean the dragon), reacts with and causes the decay
of ozone.
Determine the rate law and the value of k for the following reaction using the data
provided.
NO2(g) +03(g) → NO3(g) + O2(g)
[NO2]i (M)
[03]i (M)
Initial Rate
0.10
0.33
1.42
0.10
0.66
0.25
0.66
2.84
7.10
FULL ANSWER:
6) A data for the reaction in #5 was from experiments performed at room temperature
(assume 25 °C). The energy of activation of the reaction is 63 kJ/mole.
Use the rate constant you determined above to discover rate constant at -3 °C, which is
the temperature of the stratosphere.
ANSWER:](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d409dbe-0069-4bdd-acc1-9391e01545d6%2F26f5255a-c521-413d-aa57-b988306409ff%2Fx8r1it8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:5) NO2(g), (a.k.a. smog! And I don't mean the dragon), reacts with and causes the decay
of ozone.
Determine the rate law and the value of k for the following reaction using the data
provided.
NO2(g) +03(g) → NO3(g) + O2(g)
[NO2]i (M)
[03]i (M)
Initial Rate
0.10
0.33
1.42
0.10
0.66
0.25
0.66
2.84
7.10
FULL ANSWER:
6) A data for the reaction in #5 was from experiments performed at room temperature
(assume 25 °C). The energy of activation of the reaction is 63 kJ/mole.
Use the rate constant you determined above to discover rate constant at -3 °C, which is
the temperature of the stratosphere.
ANSWER:
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