the balanced reaction

Question

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Answer 1

Question

Chapter 13, Problem 13.29P

(a)

Interpretation Introduction

To write:

the balanced reaction

b)

Interpretation Introduction

To propose:

a reaction mechanism

Explanaiton:

Proposed Mechanism

1^s^t Step: Determine equilibrium ratios
Rate Law from the slow step

Rate=k2[NO3][NO]

Rate law form the fast step

rateforward=k1[NO][O2]ratereverse=k−1[NO3]

In equilibrium, we know that
rateforward=ratereverse

Then
rate=k−1[NO3]=k1[NO][O2]

2ⁿ^d step: Get this based on the slow step reactants, that is NO3

[NO3]=k1k−1[NO][O2]

3^r^d Step: substitute in rate law
Rate=k2[NO3][NO][NO3]=k1k −1[NO][O2]Rate=k2⋅k1k −1[NO][O2][NO]

Assume all constant as “K”
Rate=K[NO]2[O2]

(c)

To propose:

expression for k.

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Answer 2

Question

Chapter 13, Problem 13.29P

(a)

Interpretation Introduction

To write:

the balanced reaction

b)

Interpretation Introduction

To propose:

a reaction mechanism

Explanaiton:

Proposed Mechanism

1^s^t Step: Determine equilibrium ratios
Rate Law from the slow step

Rate=k2[NO3][NO]

Rate law form the fast step

rateforward=k1[NO][O2]ratereverse=k−1[NO3]

In equilibrium, we know that
rateforward=ratereverse

Then
rate=k−1[NO3]=k1[NO][O2]

2ⁿ^d step: Get this based on the slow step reactants, that is NO3

[NO3]=k1k−1[NO][O2]

3^r^d Step: substitute in rate law
Rate=k2[NO3][NO][NO3]=k1k −1[NO][O2]Rate=k2⋅k1k −1[NO][O2][NO]

Assume all constant as “K”
Rate=K[NO]2[O2]

(c)

To propose:

expression for k.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 13, Problem 13.29P

(a)

Interpretation Introduction

To write:

the balanced reaction

b)

Interpretation Introduction

To propose:

a reaction mechanism

Explanaiton:

Proposed Mechanism

1^s^t Step: Determine equilibrium ratios
Rate Law from the slow step

Rate=k2[NO3][NO]

Rate law form the fast step

rateforward=k1[NO][O2]ratereverse=k−1[NO3]

In equilibrium, we know that
rateforward=ratereverse

Then
rate=k−1[NO3]=k1[NO][O2]

2ⁿ^d step: Get this based on the slow step reactants, that is NO3

[NO3]=k1k−1[NO][O2]

3^r^d Step: substitute in rate law
Rate=k2[NO3][NO][NO3]=k1k −1[NO][O2]Rate=k2⋅k1k −1[NO][O2][NO]

Assume all constant as “K”
Rate=K[NO]2[O2]

(c)

To propose:

expression for k.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 13, Problem 13.29P

(a)

Interpretation Introduction

To write:

the balanced reaction

b)

Interpretation Introduction

To propose:

a reaction mechanism

Explanaiton:

Proposed Mechanism

1^s^t Step: Determine equilibrium ratios
Rate Law from the slow step

Rate=k2[NO3][NO]

Rate law form the fast step

rateforward=k1[NO][O2]ratereverse=k−1[NO3]

In equilibrium, we know that
rateforward=ratereverse

Then
rate=k−1[NO3]=k1[NO][O2]

2ⁿ^d step: Get this based on the slow step reactants, that is NO3

[NO3]=k1k−1[NO][O2]

3^r^d Step: substitute in rate law
Rate=k2[NO3][NO][NO3]=k1k −1[NO][O2]Rate=k2⋅k1k −1[NO][O2][NO]

Assume all constant as “K”
Rate=K[NO]2[O2]

(c)

To propose:

expression for k.

Expert Solution & Answer

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Answer 5

Chapter 13, Problem 13.29P

(a)

Interpretation Introduction

To write:

the balanced reaction

b)

Interpretation Introduction

To propose:

a reaction mechanism

Explanaiton:

Proposed Mechanism

1^s^t Step: Determine equilibrium ratios
Rate Law from the slow step

Rate=k2[NO3][NO]

Rate law form the fast step

rateforward=k1[NO][O2]ratereverse=k−1[NO3]

In equilibrium, we know that
rateforward=ratereverse

Then
rate=k−1[NO3]=k1[NO][O2]

2ⁿ^d step: Get this based on the slow step reactants, that is NO3

[NO3]=k1k−1[NO][O2]

3^r^d Step: substitute in rate law
Rate=k2[NO3][NO][NO3]=k1k −1[NO][O2]Rate=k2⋅k1k −1[NO][O2][NO]

Assume all constant as “K”
Rate=K[NO]2[O2]

(c)

To propose:

expression for k.

Answer 6

Chapter 13, Problem 13.29P

(a)

Interpretation Introduction

To write:

the balanced reaction

Answer 7

Chapter 13, Problem 13.29P

(a)

Interpretation Introduction

To write:

the balanced reaction

Answer 8

b)

Interpretation Introduction

To propose:

a reaction mechanism

Explanaiton:

Proposed Mechanism

1^s^t Step: Determine equilibrium ratios
Rate Law from the slow step

Rate=k2[NO3][NO]

Rate law form the fast step

rateforward=k1[NO][O2]ratereverse=k−1[NO3]

In equilibrium, we know that
rateforward=ratereverse

Then
rate=k−1[NO3]=k1[NO][O2]

2ⁿ^d step: Get this based on the slow step reactants, that is NO3

[NO3]=k1k−1[NO][O2]

3^r^d Step: substitute in rate law
Rate=k2[NO3][NO][NO3]=k1k −1[NO][O2]Rate=k2⋅k1k −1[NO][O2][NO]

Assume all constant as “K”
Rate=K[NO]2[O2]

(c)

To propose:

expression for k.

Answer 9

b)

Interpretation Introduction

To propose:

a reaction mechanism

Explanaiton:

Proposed Mechanism

1^s^t Step: Determine equilibrium ratios
Rate Law from the slow step

Rate=k2[NO3][NO]

Rate law form the fast step

rateforward=k1[NO][O2]ratereverse=k−1[NO3]

In equilibrium, we know that
rateforward=ratereverse

Then
rate=k−1[NO3]=k1[NO][O2]

2ⁿ^d step: Get this based on the slow step reactants, that is NO3

[NO3]=k1k−1[NO][O2]

3^r^d Step: substitute in rate law
Rate=k2[NO3][NO][NO3]=k1k −1[NO][O2]Rate=k2⋅k1k −1[NO][O2][NO]

Assume all constant as “K”
Rate=K[NO]2[O2]

(c)

To propose:

expression for k.

Answer 10

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Answer 11

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Answer 12

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Answer 13

Ch. 13 - Prob. 13.1P Ch. 13 - Prob. 13.2A Ch. 13 - Prob. 13.3P Ch. 13 - Prob. 13.4A Ch. 13 - Prob. 13.5P Ch. 13 - Prob. 13.6A Ch. 13 - Prob. 13.7P Ch. 13 - Prob. 13.8A Ch. 13 - Prob. 13.9P Ch. 13 - Prob. 13.10A

the balanced reaction

To write: the balanced reaction

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Chapter 13 Solutions

To write:

the balanced reaction