1 hentary reaction N₂0(g) → N₂(g) + O(g) - k₁ N₂(g) + O₂(g) k₂. Suppose also k₁k₂. That is, the first step is much faster than the second. 2 N₂0(g) + O(g) Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k₁, k₂, and (if necessary) the rate constants K.1 and k-2 for the reverse of the two elementary reactions in the mechanism. Explanation 1 Check 0 rate = k rate constant k = olo X S
1 hentary reaction N₂0(g) → N₂(g) + O(g) - k₁ N₂(g) + O₂(g) k₂. Suppose also k₁k₂. That is, the first step is much faster than the second. 2 N₂0(g) + O(g) Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k₁, k₂, and (if necessary) the rate constants K.1 and k-2 for the reverse of the two elementary reactions in the mechanism. Explanation 1 Check 0 rate = k rate constant k = olo X S
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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![elementary reaction
rate constant
N₂O(g) → N₂(g) + O(g)
-
k₁
2 N₂0(g) + O(g) N₂(g) + O₂(9)
k₂.
Suppose also k₁k2. That is, the first step is much faster than the second.
1
Pate law implied by a simple mechanism
Write the balanced
chemical equation for the
overall chemical reaction:
Write the experimentally-
observable rate law for the
overall chemical reaction.
Note: your answer should
not contain the
concentrations of any
intermediates.
Express the rate constant
k for the overall chemical
reaction in terms of k₁, K₂,
and (if necessary) the rate
constants k.1 and k-2 for
the reverse of the two
elementary reactions in
the mechanism.
Explanation
Check
0
rate = k
k =
JUL
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00
4
P
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© 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Ce](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F58cffe43-d701-4c21-9740-08fe8d98ee79%2F2e72622c-0e3a-472a-9280-3f8091b0c6be%2Fqqczy1e_processed.jpeg&w=3840&q=75)
Transcribed Image Text:elementary reaction
rate constant
N₂O(g) → N₂(g) + O(g)
-
k₁
2 N₂0(g) + O(g) N₂(g) + O₂(9)
k₂.
Suppose also k₁k2. That is, the first step is much faster than the second.
1
Pate law implied by a simple mechanism
Write the balanced
chemical equation for the
overall chemical reaction:
Write the experimentally-
observable rate law for the
overall chemical reaction.
Note: your answer should
not contain the
concentrations of any
intermediates.
Express the rate constant
k for the overall chemical
reaction in terms of k₁, K₂,
and (if necessary) the rate
constants k.1 and k-2 for
the reverse of the two
elementary reactions in
the mechanism.
Explanation
Check
0
rate = k
k =
JUL
tv
W
X
ローロ On
00
4
P
H
© 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Ce
![Some measurements of the initial rate of a certain reaction are given in the table below.
[H₂] [₂] initial rate of reaction
2.44M 0.639M
56.0M/s
2.44M 0.154M
13.5M/s
7.70M 0.639 M
177.M/s
Use this information to write a rate law for this reaction, and calculate the value of the rate constant k.
Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol.
rate = k
k=
Explanation
Check
JUL
16
x10
0.0
x
00
S
tv
W
2023 McGraw Hill LLC. All Rights Reserved.
Terms of Use](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F58cffe43-d701-4c21-9740-08fe8d98ee79%2F2e72622c-0e3a-472a-9280-3f8091b0c6be%2F27vy7j8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Some measurements of the initial rate of a certain reaction are given in the table below.
[H₂] [₂] initial rate of reaction
2.44M 0.639M
56.0M/s
2.44M 0.154M
13.5M/s
7.70M 0.639 M
177.M/s
Use this information to write a rate law for this reaction, and calculate the value of the rate constant k.
Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol.
rate = k
k=
Explanation
Check
JUL
16
x10
0.0
x
00
S
tv
W
2023 McGraw Hill LLC. All Rights Reserved.
Terms of Use
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