Reaction Coordinate diagram: Is it possible for the activation energy for the reverse reaction to be less than the activation energy for the forward reaction? Explain.
Reaction Coordinate diagram: Is it possible for the activation energy for the reverse reaction to be less than the activation energy for the forward reaction? Explain.
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
Chapter12: Chemical Kinetics
Section: Chapter Questions
Problem 93AE: At 620. K butadiene dimerizes at a moderate rate. The following data were obtained in an experiment...
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Question
![Reaction Coordinate diagram: Is it possible
for the activation energy for the reverse
reaction to be less than the activation
energy for the forward reaction? Explain.
Integrated rate laws: Consider the
decomposition reaction of HI at 150°C.
This is a zero - order reaction. At the
beginning of the reaction, the
-4 M
[HI] = 0.250M. Given k = 1.2 x 10 a.
S
calculate the half-life, t₁.b. What is the
2
maximum time this reaction can proceed?
2HI → H₂(g) + 1₂ (g) Reaction Mechanisms:
2
One proposed mechanism for the
decomposition of N2O5 to NO₂ involves
the following three elementary steps: Step
12N₂O(g)harrNO(g) Fast and
5
reversible Step
2, NO(g)
4 10
Slow Step
→
4 10
N₂O3(g) + 2NO₂(g) + O₂(g),
2
3, N₂O₂(g) + O₂(g) → 2NO₂(g) + O₂(g),
2
3
Will 140
fast Overall, 2N₂O(g) → 4NO₂(g) + O₂ (g)
5
2
What is the rate law for the overall reaction
based on the proposed mechanism? The
experimentally determined Rate law
= K[NO], is the mechanism correct?
2 5
Ć
4. Reaction Coordinate diagram: Is it possible for tre activation energy for the reverse
reaction to be less than the activation energy for the forward reaction? Explain.
5. Integrated rate laws: Consider the decomposition reaction of HI at 150 °C. This is a
zero-order reaction. At the beginning of the reaction, the [HI] -0.250M. Given k = 1.2 x 10
Mis
a calculate the half-lide. te
b. What is the maximum time this reaction can proceed?
2H1 H₂ (g) lig).
6. Reaction Mechanisms: One proposed mesranism for the decomposition of NO to NO₂
involves the following thros elementary steps:
Step 1
Fast and reversible
2N,Ogla) NaOide
Slow
fast
Step 2 N₂Oolg) N₂O₂(g) + 2NO(g) + Os(g)
Step 3 NyOsig) + Osig)-2NO(g) +0g)
Overall
2N-Os9) 4NO₂(g) + Ogle:
What is the rate law for the overall reaction cosed or the proposed mechanism?
The experimentally determined Rate law = KIN₂O), is the mechanism correct?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9463ea76-927d-4bf5-99b1-5eaf2e001d4a%2Ff25bc2b7-3b9f-48ef-83d1-6d42c628bd84%2F94682os_processed.png&w=3840&q=75)
Transcribed Image Text:Reaction Coordinate diagram: Is it possible
for the activation energy for the reverse
reaction to be less than the activation
energy for the forward reaction? Explain.
Integrated rate laws: Consider the
decomposition reaction of HI at 150°C.
This is a zero - order reaction. At the
beginning of the reaction, the
-4 M
[HI] = 0.250M. Given k = 1.2 x 10 a.
S
calculate the half-life, t₁.b. What is the
2
maximum time this reaction can proceed?
2HI → H₂(g) + 1₂ (g) Reaction Mechanisms:
2
One proposed mechanism for the
decomposition of N2O5 to NO₂ involves
the following three elementary steps: Step
12N₂O(g)harrNO(g) Fast and
5
reversible Step
2, NO(g)
4 10
Slow Step
→
4 10
N₂O3(g) + 2NO₂(g) + O₂(g),
2
3, N₂O₂(g) + O₂(g) → 2NO₂(g) + O₂(g),
2
3
Will 140
fast Overall, 2N₂O(g) → 4NO₂(g) + O₂ (g)
5
2
What is the rate law for the overall reaction
based on the proposed mechanism? The
experimentally determined Rate law
= K[NO], is the mechanism correct?
2 5
Ć
4. Reaction Coordinate diagram: Is it possible for tre activation energy for the reverse
reaction to be less than the activation energy for the forward reaction? Explain.
5. Integrated rate laws: Consider the decomposition reaction of HI at 150 °C. This is a
zero-order reaction. At the beginning of the reaction, the [HI] -0.250M. Given k = 1.2 x 10
Mis
a calculate the half-lide. te
b. What is the maximum time this reaction can proceed?
2H1 H₂ (g) lig).
6. Reaction Mechanisms: One proposed mesranism for the decomposition of NO to NO₂
involves the following thros elementary steps:
Step 1
Fast and reversible
2N,Ogla) NaOide
Slow
fast
Step 2 N₂Oolg) N₂O₂(g) + 2NO(g) + Os(g)
Step 3 NyOsig) + Osig)-2NO(g) +0g)
Overall
2N-Os9) 4NO₂(g) + Ogle:
What is the rate law for the overall reaction cosed or the proposed mechanism?
The experimentally determined Rate law = KIN₂O), is the mechanism correct?
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