Order and rate law of a reaction The overall order of an elementary step directl

Question

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

The exponent "2" is used because the reaction involves two NO2 molecules. The rate law for step 2 is

rate=k[NO3]1[CO]1=k[NO3][CO]

because the reaction involves only one molecule of each reactant the exponents are ommitted.

Analyzing a new reaction

3XE+F

E+MF+N

Part A

What is the overall reaction?

Express your answer as a chemical equation.

Submit

Part B

Part complete

Which species is a reaction intermediate?

View Available Hint(s)

SubmitPrevious Answers

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

Part D

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)

Rate =

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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

The exponent "2" is used because the reaction involves two NO2 molecules. The rate law for step 2 is

rate=k[NO3]1[CO]1=k[NO3][CO]

because the reaction involves only one molecule of each reactant the exponents are ommitted.

Analyzing a new reaction

3XE+F

E+MF+N

Part A

What is the overall reaction?

Express your answer as a chemical equation.

View Available Hint(s)

Submit

Part B

Part complete

Which species is a reaction intermediate?

View Available Hint(s)

SubmitPrevious Answers

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

Part D

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)

Rate =

SubmitPrevious Answers

Incorrect; Try Again; 3 attempts remaining

Next

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

The exponent "2" is used because the reaction involves two NO2 molecules. The rate law for step 2 is

rate=k[NO3]1[CO]1=k[NO3][CO]

because the reaction involves only one molecule of each reactant the exponents are ommitted.

Analyzing a new reaction

3XE+F

E+MF+N

Part A

What is the overall reaction?

Express your answer as a chemical equation.

View Available Hint(s)

Submit

Part B

Part complete

Which species is a reaction intermediate?

View Available Hint(s)

SubmitPrevious Answers

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

Part D

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)

Rate =

SubmitPrevious Answers

Incorrect; Try Again; 3 attempts remaining

Next

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

The exponent "2" is used because the reaction involves two NO2 molecules. The rate law for step 2 is

rate=k[NO3]1[CO]1=k[NO3][CO]

because the reaction involves only one molecule of each reactant the exponents are ommitted.

Analyzing a new reaction

Consider the following elementary steps that make up the mechanism of a certain reaction:

3XE+F

E+MF+N

Part A

What is the overall reaction?

Express your answer as a chemical equation.

Submit

Part B

Part complete

Which species is a reaction intermediate?

View Available Hint(s)

X E F M N

SubmitPrevious Answers

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

Part D

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)

Rate =

SubmitPrevious Answers

Incorrect; Try Again; 3 attempts remaining

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Explanation / Answer

3XE+F

E+MF+N

----------------------------------------

3X + M ---------------> 2F + N

part A )

overall reaction : 3X + M ---------------> 2F + N

part B)

intermediate = E

because that is not found in overall reaction

part C)

rate = k * [X]^3

part D)

rate = k * [E]* [M]

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