ep By 4 e uld Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1.2A+B+C 2. B+DE+C Part A What is the overall reaction? Express your answer as a chemical equation. ▸ View Available Hint(s) Templates Symbols undo' rego Teset keyboard shortcuts Help Achemical reaction does not occur for this question. Submit Previous Answers * Incorrect: Try Again: 3 attempts remaining Part B Which species is a reaction intermediate? ▸ View Available Hint(s) B C n
ep By 4 e uld Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1.2A+B+C 2. B+DE+C Part A What is the overall reaction? Express your answer as a chemical equation. ▸ View Available Hint(s) Templates Symbols undo' rego Teset keyboard shortcuts Help Achemical reaction does not occur for this question. Submit Previous Answers * Incorrect: Try Again: 3 attempts remaining Part B Which species is a reaction intermediate? ▸ View Available Hint(s) B C n
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter3: Matter-properties And Changes
Section3.4: Elements And Compounds
Problem 25SSC
Related questions
Question
![Learning Goal:
To understand how elementary steps make up a mechanism and how the rate law for an
elementary step can be determined.
Very often, a reaction does not tell us the whole story. For instance, the reaction
NO₂(g) + CO(g) →NO(g) + CO₂(g)
does not involve a collision between an NO₂ molecule and a CO molecule. Based on
experimental data at moderate temperatures, this reaction is thought to occur in the
following two steps:
1. NO₂(g) + NO₂(g) NO(g) + NO(g)
2. NO₂(g) + CO(g)→CO₂(g) +NO₂(g)
Each individual step is called an elementary step. Together, these elementary steps are
called the reaction mechanism.
Overall, the resulting reaction is
NO₂(g) + CO(g) →NO(g) + CO₂(g)
Notice that in the elementary steps NO appears both as a product and then as a
reactant, therefore it cancels out of the final chemical equation. NO, is called a reaction
intermediate. Also notice that 2 molecules of NO₂ appear in the reactants of the first step
and 1 molecule of NO₂ appears as product of the second step, the net effect leaves only
1 molecule of NO2 as a reactant in the net equation.
Moleculanty is the proper term for "how the molecules collide" in a reaction. For example,
step 1 is bimolecular because it involves the collision of two molecules. Step 2 is also
bimolecular for the same reason. Unimolecular reactions involve only one molecule in the
reactants. Though rare, collisions among three molecules can occur. Such a reaction would
be called termolecular.
B
D
OE
Submit
✓ Correct
▾ Part C
What is the rate law for step 1 of this reaction?
Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C]³ type k* [A]*[C]^3.
▸ View Available Hint(s)
Rate =
Submit
Previous Answers
▾ Part D
* Incorrect, Try Again; One attempt remaining
Previous Answers
Rate =
What is the rate law for step 2 of this reaction?
Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C]³ type k*[A]*[C]^3.
▸ View Available Hint(s)
Submit Previous Answers
* Incorrect, Try Again; 4 attempts remaining](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F096b6bb3-2f11-49d8-9074-81efda173389%2Ffe4446ad-ba34-463c-ba92-130aa74635e7%2F9dyd5ml_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Learning Goal:
To understand how elementary steps make up a mechanism and how the rate law for an
elementary step can be determined.
Very often, a reaction does not tell us the whole story. For instance, the reaction
NO₂(g) + CO(g) →NO(g) + CO₂(g)
does not involve a collision between an NO₂ molecule and a CO molecule. Based on
experimental data at moderate temperatures, this reaction is thought to occur in the
following two steps:
1. NO₂(g) + NO₂(g) NO(g) + NO(g)
2. NO₂(g) + CO(g)→CO₂(g) +NO₂(g)
Each individual step is called an elementary step. Together, these elementary steps are
called the reaction mechanism.
Overall, the resulting reaction is
NO₂(g) + CO(g) →NO(g) + CO₂(g)
Notice that in the elementary steps NO appears both as a product and then as a
reactant, therefore it cancels out of the final chemical equation. NO, is called a reaction
intermediate. Also notice that 2 molecules of NO₂ appear in the reactants of the first step
and 1 molecule of NO₂ appears as product of the second step, the net effect leaves only
1 molecule of NO2 as a reactant in the net equation.
Moleculanty is the proper term for "how the molecules collide" in a reaction. For example,
step 1 is bimolecular because it involves the collision of two molecules. Step 2 is also
bimolecular for the same reason. Unimolecular reactions involve only one molecule in the
reactants. Though rare, collisions among three molecules can occur. Such a reaction would
be called termolecular.
B
D
OE
Submit
✓ Correct
▾ Part C
What is the rate law for step 1 of this reaction?
Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C]³ type k* [A]*[C]^3.
▸ View Available Hint(s)
Rate =
Submit
Previous Answers
▾ Part D
* Incorrect, Try Again; One attempt remaining
Previous Answers
Rate =
What is the rate law for step 2 of this reaction?
Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C]³ type k*[A]*[C]^3.
▸ View Available Hint(s)
Submit Previous Answers
* Incorrect, Try Again; 4 attempts remaining
![<Week 1 Assignment: Chemical Kinetics
Mechanisms and Molecularity
Learning Goal:
To understand how elementary steps make up a mechanism and how the rate law for an
elementary step can be determined.
Very often, a reaction does not tell us the whole story. For instance, the reaction
NO₂(g) + CO(g) →NO(g) + CO₂(g)
does not involve a collision between an NO₂ molecule and a CO molecule. Based on
experimental data at moderate temperatures, this reaction is thought to occur in the
following two steps:
1. NO₂(g) + NO₂(g)→NO₁ (g) + NO(g)
2. NO3(g) + CO(g)→CO₂(g) + NO₂(g)
Each individual step is called an elementary step. Together, these elementary steps are
called the reaction mechanism.
Overall, the resulting reaction is
NO₂(g) + CO(g) NO(g) + CO₂(g)
Notice that in the elementary steps NO appears both as a product and then as a
reactant, therefore it cancels out of the final chemical equation. NO₂ is called a reaction
intermediate. Also notice that 2 molecules of NO₂ appear in the reactants of the first step
and 1 molecule of NO₂ appears as product of the second step, the net effect leaves only
1 molecule of NO₂ as a reactant in the net equation.
Molecularity is the proper term for "how the molecules collide" in a reaction. For example,
step 1 is bimolecular because it involves the collision of two molecules. Step 2 is also
bimolecular for the same reason. Unimolecular reactions involve only one molecule in the
reactants. Though rare, collisions among three molecules can occur. Such a reaction would
be called termolecular.
The exponent "2" is used because the reaction involves two NO₂ molecules. The rate law for step 2 is
Order and rate law of a reaction
The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular. Furthermore, the rate law can be determined directly
from the number of each type of molecule in an elementary step. For example, the rate law for step 1 is
rate = k[NO₂)²
because the reaction involves only one molecule of each reactant the exponents are omitted.
Analyzing a new reaction
Consider the following elementary steps that make up the mechanism of a certain reaction:
1.2A+B+C
2. B+DE+C
Part A
What is the overall reaction?
Express your answer as a chemical equation.
▸ View Available Hint(s)
Templates Symbols undo' regio Reset keyboard shortcuts Help
nu
A chemical reaction does not occur for this question.
Submit Previous Angwgra
* Incorrect; Try Again; 3 attempts remaining
▾ Part B
Which species is a reaction intermediate?
▸ View Available Hint(s)
OA
B
rate = k[NO]¹[CO]¹=k[NO][CO]
с
n
<27 of 38 >
Review | Constants | Periodic Table](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F096b6bb3-2f11-49d8-9074-81efda173389%2Ffe4446ad-ba34-463c-ba92-130aa74635e7%2F2wl2hf_processed.jpeg&w=3840&q=75)
Transcribed Image Text:<Week 1 Assignment: Chemical Kinetics
Mechanisms and Molecularity
Learning Goal:
To understand how elementary steps make up a mechanism and how the rate law for an
elementary step can be determined.
Very often, a reaction does not tell us the whole story. For instance, the reaction
NO₂(g) + CO(g) →NO(g) + CO₂(g)
does not involve a collision between an NO₂ molecule and a CO molecule. Based on
experimental data at moderate temperatures, this reaction is thought to occur in the
following two steps:
1. NO₂(g) + NO₂(g)→NO₁ (g) + NO(g)
2. NO3(g) + CO(g)→CO₂(g) + NO₂(g)
Each individual step is called an elementary step. Together, these elementary steps are
called the reaction mechanism.
Overall, the resulting reaction is
NO₂(g) + CO(g) NO(g) + CO₂(g)
Notice that in the elementary steps NO appears both as a product and then as a
reactant, therefore it cancels out of the final chemical equation. NO₂ is called a reaction
intermediate. Also notice that 2 molecules of NO₂ appear in the reactants of the first step
and 1 molecule of NO₂ appears as product of the second step, the net effect leaves only
1 molecule of NO₂ as a reactant in the net equation.
Molecularity is the proper term for "how the molecules collide" in a reaction. For example,
step 1 is bimolecular because it involves the collision of two molecules. Step 2 is also
bimolecular for the same reason. Unimolecular reactions involve only one molecule in the
reactants. Though rare, collisions among three molecules can occur. Such a reaction would
be called termolecular.
The exponent "2" is used because the reaction involves two NO₂ molecules. The rate law for step 2 is
Order and rate law of a reaction
The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular. Furthermore, the rate law can be determined directly
from the number of each type of molecule in an elementary step. For example, the rate law for step 1 is
rate = k[NO₂)²
because the reaction involves only one molecule of each reactant the exponents are omitted.
Analyzing a new reaction
Consider the following elementary steps that make up the mechanism of a certain reaction:
1.2A+B+C
2. B+DE+C
Part A
What is the overall reaction?
Express your answer as a chemical equation.
▸ View Available Hint(s)
Templates Symbols undo' regio Reset keyboard shortcuts Help
nu
A chemical reaction does not occur for this question.
Submit Previous Angwgra
* Incorrect; Try Again; 3 attempts remaining
▾ Part B
Which species is a reaction intermediate?
▸ View Available Hint(s)
OA
B
rate = k[NO]¹[CO]¹=k[NO][CO]
с
n
<27 of 38 >
Review | Constants | Periodic Table
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