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
![The reaction
NO(g) + 02(g) – NO2(g) + O(g)
plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of
experiments measured the rate of this reaction at a certain temperature and produced the following data:
[02]
(mol L1)
[NO]
Rate
Expt
(mol L)
(mol L1s)
1
0.0020
0.0050
5.0 x 1017
2
0.0020
0.010
1.0 x 1016
0.0060
0.0050
1.5 x 1016
A rate = k[NO]°[O2]?
B rate = k[NO][O2]?
C
rate = k[NO]?[02]
D) rate = k[NO][02]
3.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7441161a-6010-45b0-a993-38b7cdf475f6%2F88d4aa7f-617b-497f-bda7-0a9d92184451%2Fq8fd97l_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The reaction
NO(g) + 02(g) – NO2(g) + O(g)
plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of
experiments measured the rate of this reaction at a certain temperature and produced the following data:
[02]
(mol L1)
[NO]
Rate
Expt
(mol L)
(mol L1s)
1
0.0020
0.0050
5.0 x 1017
2
0.0020
0.010
1.0 x 1016
0.0060
0.0050
1.5 x 1016
A rate = k[NO]°[O2]?
B rate = k[NO][O2]?
C
rate = k[NO]?[02]
D) rate = k[NO][02]
3.
![JUST A REMINDER, TAKE NOTE
IN SOLVING
Summary of molecularity of elementary reactions
Type of Elementary Reaction
Molecularity
Rate Law
A→ products
Unimolecular
Rate = k[A]
%3D
A + B → products
2 A→products
Rate
k[A][B]
%3D
Bimolecular
Rate = k[A]²
%3D
A + B + C → products
2 A + B → products
Rate = k[A][B][C]
%3D
Termolecular
Rate = k[A]°[B]
A + B + C + D→ products
The Arrhenius equation describes the temperature
dependence of the rate constant, k.
Not observed
Ea
k = Ae RT
- E, is the activation energy
- R is the universal gas law constant
• Ris 8.314 J mol K
- T is the absolute temperature,
- A is the proportionality constant called the frequency factor or
0.693
t1/2 =
k
preexponential factor.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7441161a-6010-45b0-a993-38b7cdf475f6%2F88d4aa7f-617b-497f-bda7-0a9d92184451%2Fd2utg2t_processed.jpeg&w=3840&q=75)
Transcribed Image Text:JUST A REMINDER, TAKE NOTE
IN SOLVING
Summary of molecularity of elementary reactions
Type of Elementary Reaction
Molecularity
Rate Law
A→ products
Unimolecular
Rate = k[A]
%3D
A + B → products
2 A→products
Rate
k[A][B]
%3D
Bimolecular
Rate = k[A]²
%3D
A + B + C → products
2 A + B → products
Rate = k[A][B][C]
%3D
Termolecular
Rate = k[A]°[B]
A + B + C + D→ products
The Arrhenius equation describes the temperature
dependence of the rate constant, k.
Not observed
Ea
k = Ae RT
- E, is the activation energy
- R is the universal gas law constant
• Ris 8.314 J mol K
- T is the absolute temperature,
- A is the proportionality constant called the frequency factor or
0.693
t1/2 =
k
preexponential factor.
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