The order of the given reaction andits rate constant is to be determined and the probable mechanism, which is consistent with the rate law, is to be suggested. Concept introduction: The branch of chemistry that deals with the relative rates of the chemical reactions and the factors affecting the rates of reactions is known as chemical kinetics . The rate of a reaction is the measurement of concentration change of the reactants, within a given period of time.

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Answer 1

Question

Chapter 14, Problem 80AP

Interpretation Introduction

Interpretation:

The order of the given reaction andits rate constant is to be determined and the probable mechanism, which is consistent with the rate law, is to be suggested.

Concept introduction:

The branch of chemistry that deals with the relative rates of the chemical reactions and the factors affecting the rates of reactions is known as chemical kinetics.

The rate of a reaction is the measurement of concentration change of the reactants, within a given period of time.

Expert Solution & Answer

Answer to Problem 80AP

Solution:

3

0.38 s−1

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

Explanation of Solution

Given information:

The reaction between hydrogen and nitric acid, at 700°C is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

Experiment	[H2](M)	[NO](M)	Initial Rate (M/s)
1	0.010	0.025	2.4×10−6
2	0.0050	0.025	1.2×10−6
3	0.010	0.0125	0.60×10−6

a)The order of reaction

The order of the reaction is given by the following expression as:

Rate2Rate1=([A]2[A]1)x([B]2[B]1)y …… (1)

Here, x is the order with respect to A and y is the order with respect to B.

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 3 in equation (1),

2.4×10−6M/s0.60×10−6M/s=(0.010 M0.010 M)x(0.025 M0.0125 M)y4=2yy=2

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 2 in the equation (1),

2.4×10−6M/s1.2×10−6M/s=(0.010 M0.0050 M)x(0.025 M0.025 M)y2=2xx=1

Hence, the overall order of the reaction is 3.

b) The rate constant

The rate expression for the reaction is given as follows:

rate=k[NO]2[H2]k=rate[NO]2[H2]

Substitute the values of [NO], [H2], and rate of reaction in the above equation:

rate=2.4×10−6M/s[0.025M]2[0.010M]=2.4×10−6M/s3.125×10−6M=0.384s−1

Hence, the rate constant for the reaction is 0.38 s−1.

c) A plausible mechanism that is consistent to rate law.

The reaction between hydrogen with nitric oxide is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

The plausible mechanism of the reaction, which isconsistent with the rate law, is given as follows:

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

The overall reaction is obtained as follows:

H2+2NO→N2O+H2ON2O+H2→N2+H2O_2H2+2NO→N2+2H2O_

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Answer 2

Question

Chapter 14, Problem 80AP

Interpretation Introduction

Interpretation:

The order of the given reaction andits rate constant is to be determined and the probable mechanism, which is consistent with the rate law, is to be suggested.

Concept introduction:

The branch of chemistry that deals with the relative rates of the chemical reactions and the factors affecting the rates of reactions is known as chemical kinetics.

The rate of a reaction is the measurement of concentration change of the reactants, within a given period of time.

Expert Solution & Answer

Answer to Problem 80AP

Solution:

3

0.38 s−1

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

Explanation of Solution

Given information:

The reaction between hydrogen and nitric acid, at 700°C is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

Experiment	[H2](M)	[NO](M)	Initial Rate (M/s)
1	0.010	0.025	2.4×10−6
2	0.0050	0.025	1.2×10−6
3	0.010	0.0125	0.60×10−6

a)The order of reaction

The order of the reaction is given by the following expression as:

Rate2Rate1=([A]2[A]1)x([B]2[B]1)y …… (1)

Here, x is the order with respect to A and y is the order with respect to B.

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 3 in equation (1),

2.4×10−6M/s0.60×10−6M/s=(0.010 M0.010 M)x(0.025 M0.0125 M)y4=2yy=2

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 2 in the equation (1),

2.4×10−6M/s1.2×10−6M/s=(0.010 M0.0050 M)x(0.025 M0.025 M)y2=2xx=1

Hence, the overall order of the reaction is 3.

b) The rate constant

The rate expression for the reaction is given as follows:

rate=k[NO]2[H2]k=rate[NO]2[H2]

Substitute the values of [NO], [H2], and rate of reaction in the above equation:

rate=2.4×10−6M/s[0.025M]2[0.010M]=2.4×10−6M/s3.125×10−6M=0.384s−1

Hence, the rate constant for the reaction is 0.38 s−1.

c) A plausible mechanism that is consistent to rate law.

The reaction between hydrogen with nitric oxide is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

The plausible mechanism of the reaction, which isconsistent with the rate law, is given as follows:

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

The overall reaction is obtained as follows:

H2+2NO→N2O+H2ON2O+H2→N2+H2O_2H2+2NO→N2+2H2O_

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Answer 3

Question

Chapter 14, Problem 80AP

Interpretation Introduction

Interpretation:

The order of the given reaction andits rate constant is to be determined and the probable mechanism, which is consistent with the rate law, is to be suggested.

Concept introduction:

The branch of chemistry that deals with the relative rates of the chemical reactions and the factors affecting the rates of reactions is known as chemical kinetics.

The rate of a reaction is the measurement of concentration change of the reactants, within a given period of time.

Expert Solution & Answer

Answer to Problem 80AP

Solution:

3

0.38 s−1

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

Explanation of Solution

Given information:

The reaction between hydrogen and nitric acid, at 700°C is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

Experiment	[H2](M)	[NO](M)	Initial Rate (M/s)
1	0.010	0.025	2.4×10−6
2	0.0050	0.025	1.2×10−6
3	0.010	0.0125	0.60×10−6

a)The order of reaction

The order of the reaction is given by the following expression as:

Rate2Rate1=([A]2[A]1)x([B]2[B]1)y …… (1)

Here, x is the order with respect to A and y is the order with respect to B.

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 3 in equation (1),

2.4×10−6M/s0.60×10−6M/s=(0.010 M0.010 M)x(0.025 M0.0125 M)y4=2yy=2

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 2 in the equation (1),

2.4×10−6M/s1.2×10−6M/s=(0.010 M0.0050 M)x(0.025 M0.025 M)y2=2xx=1

Hence, the overall order of the reaction is 3.

b) The rate constant

The rate expression for the reaction is given as follows:

rate=k[NO]2[H2]k=rate[NO]2[H2]

Substitute the values of [NO], [H2], and rate of reaction in the above equation:

rate=2.4×10−6M/s[0.025M]2[0.010M]=2.4×10−6M/s3.125×10−6M=0.384s−1

Hence, the rate constant for the reaction is 0.38 s−1.

c) A plausible mechanism that is consistent to rate law.

The reaction between hydrogen with nitric oxide is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

The plausible mechanism of the reaction, which isconsistent with the rate law, is given as follows:

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

The overall reaction is obtained as follows:

H2+2NO→N2O+H2ON2O+H2→N2+H2O_2H2+2NO→N2+2H2O_

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Answer 4

Question

Chapter 14, Problem 80AP

Interpretation Introduction

Interpretation:

The order of the given reaction andits rate constant is to be determined and the probable mechanism, which is consistent with the rate law, is to be suggested.

Concept introduction:

The branch of chemistry that deals with the relative rates of the chemical reactions and the factors affecting the rates of reactions is known as chemical kinetics.

The rate of a reaction is the measurement of concentration change of the reactants, within a given period of time.

Expert Solution & Answer

Answer to Problem 80AP

Solution:

3

0.38 s−1

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

Explanation of Solution

Given information:

The reaction between hydrogen and nitric acid, at 700°C is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

Experiment	[H2](M)	[NO](M)	Initial Rate (M/s)
1	0.010	0.025	2.4×10−6
2	0.0050	0.025	1.2×10−6
3	0.010	0.0125	0.60×10−6

a)The order of reaction

The order of the reaction is given by the following expression as:

Rate2Rate1=([A]2[A]1)x([B]2[B]1)y …… (1)

Here, x is the order with respect to A and y is the order with respect to B.

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 3 in equation (1),

2.4×10−6M/s0.60×10−6M/s=(0.010 M0.010 M)x(0.025 M0.0125 M)y4=2yy=2

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 2 in the equation (1),

2.4×10−6M/s1.2×10−6M/s=(0.010 M0.0050 M)x(0.025 M0.025 M)y2=2xx=1

Hence, the overall order of the reaction is 3.

b) The rate constant

The rate expression for the reaction is given as follows:

rate=k[NO]2[H2]k=rate[NO]2[H2]

Substitute the values of [NO], [H2], and rate of reaction in the above equation:

rate=2.4×10−6M/s[0.025M]2[0.010M]=2.4×10−6M/s3.125×10−6M=0.384s−1

Hence, the rate constant for the reaction is 0.38 s−1.

c) A plausible mechanism that is consistent to rate law.

The reaction between hydrogen with nitric oxide is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

The plausible mechanism of the reaction, which isconsistent with the rate law, is given as follows:

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

The overall reaction is obtained as follows:

H2+2NO→N2O+H2ON2O+H2→N2+H2O_2H2+2NO→N2+2H2O_

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Answer 5

Chapter 14, Problem 80AP

Interpretation Introduction

Interpretation:

The order of the given reaction andits rate constant is to be determined and the probable mechanism, which is consistent with the rate law, is to be suggested.

Concept introduction:

The branch of chemistry that deals with the relative rates of the chemical reactions and the factors affecting the rates of reactions is known as chemical kinetics.

The rate of a reaction is the measurement of concentration change of the reactants, within a given period of time.

Expert Solution & Answer

Answer to Problem 80AP

Solution:

3

0.38 s−1

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

Explanation of Solution

Given information:

The reaction between hydrogen and nitric acid, at 700°C is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

Experiment	[H2](M)	[NO](M)	Initial Rate (M/s)
1	0.010	0.025	2.4×10−6
2	0.0050	0.025	1.2×10−6
3	0.010	0.0125	0.60×10−6

a)The order of reaction

The order of the reaction is given by the following expression as:

Rate2Rate1=([A]2[A]1)x([B]2[B]1)y …… (1)

Here, x is the order with respect to A and y is the order with respect to B.

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 3 in equation (1),

2.4×10−6M/s0.60×10−6M/s=(0.010 M0.010 M)x(0.025 M0.0125 M)y4=2yy=2

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 2 in the equation (1),

2.4×10−6M/s1.2×10−6M/s=(0.010 M0.0050 M)x(0.025 M0.025 M)y2=2xx=1

Hence, the overall order of the reaction is 3.

b) The rate constant

The rate expression for the reaction is given as follows:

rate=k[NO]2[H2]k=rate[NO]2[H2]

Substitute the values of [NO], [H2], and rate of reaction in the above equation:

rate=2.4×10−6M/s[0.025M]2[0.010M]=2.4×10−6M/s3.125×10−6M=0.384s−1

Hence, the rate constant for the reaction is 0.38 s−1.

c) A plausible mechanism that is consistent to rate law.

The reaction between hydrogen with nitric oxide is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

The plausible mechanism of the reaction, which isconsistent with the rate law, is given as follows:

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

The overall reaction is obtained as follows:

H2+2NO→N2O+H2ON2O+H2→N2+H2O_2H2+2NO→N2+2H2O_

Answer 6

Chapter 14, Problem 80AP

Interpretation Introduction

Interpretation:

The order of the given reaction andits rate constant is to be determined and the probable mechanism, which is consistent with the rate law, is to be suggested.

Concept introduction:

The branch of chemistry that deals with the relative rates of the chemical reactions and the factors affecting the rates of reactions is known as chemical kinetics.

The rate of a reaction is the measurement of concentration change of the reactants, within a given period of time.

Expert Solution & Answer

Answer to Problem 80AP

Solution:

3

0.38 s−1

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

Explanation of Solution

Given information:

The reaction between hydrogen and nitric acid, at 700°C is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

Experiment	[H2](M)	[NO](M)	Initial Rate (M/s)
1	0.010	0.025	2.4×10−6
2	0.0050	0.025	1.2×10−6
3	0.010	0.0125	0.60×10−6

a)The order of reaction

The order of the reaction is given by the following expression as:

Rate2Rate1=([A]2[A]1)x([B]2[B]1)y …… (1)

Here, x is the order with respect to A and y is the order with respect to B.

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 3 in equation (1),

2.4×10−6M/s0.60×10−6M/s=(0.010 M0.010 M)x(0.025 M0.0125 M)y4=2yy=2

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 2 in the equation (1),

2.4×10−6M/s1.2×10−6M/s=(0.010 M0.0050 M)x(0.025 M0.025 M)y2=2xx=1

Hence, the overall order of the reaction is 3.

b) The rate constant

The rate expression for the reaction is given as follows:

rate=k[NO]2[H2]k=rate[NO]2[H2]

Substitute the values of [NO], [H2], and rate of reaction in the above equation:

rate=2.4×10−6M/s[0.025M]2[0.010M]=2.4×10−6M/s3.125×10−6M=0.384s−1

Hence, the rate constant for the reaction is 0.38 s−1.

c) A plausible mechanism that is consistent to rate law.

The reaction between hydrogen with nitric oxide is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

The plausible mechanism of the reaction, which isconsistent with the rate law, is given as follows:

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

The overall reaction is obtained as follows:

H2+2NO→N2O+H2ON2O+H2→N2+H2O_2H2+2NO→N2+2H2O_

Answer 7

Chapter 14, Problem 80AP

Interpretation Introduction

Interpretation:

The order of the given reaction andits rate constant is to be determined and the probable mechanism, which is consistent with the rate law, is to be suggested.

Concept introduction:

The branch of chemistry that deals with the relative rates of the chemical reactions and the factors affecting the rates of reactions is known as chemical kinetics.

The rate of a reaction is the measurement of concentration change of the reactants, within a given period of time.

Answer 8

Expert Solution & Answer

Answer to Problem 80AP

Solution:

3

0.38 s−1

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Explanation of Solution

Given information:

The reaction between hydrogen and nitric acid, at 700°C is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

Experiment	[H2](M)	[NO](M)	Initial Rate (M/s)
1	0.010	0.025	2.4×10−6
2	0.0050	0.025	1.2×10−6
3	0.010	0.0125	0.60×10−6

a)The order of reaction

The order of the reaction is given by the following expression as:

Rate2Rate1=([A]2[A]1)x([B]2[B]1)y …… (1)

Here, x is the order with respect to A and y is the order with respect to B.

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 3 in equation (1),

2.4×10−6M/s0.60×10−6M/s=(0.010 M0.010 M)x(0.025 M0.0125 M)y4=2yy=2

Substitute the values of Rate1, Rate2, [A]1, [A]2, [B]1, and [B]2 from experiments 1 and 2 in the equation (1),

2.4×10−6M/s1.2×10−6M/s=(0.010 M0.0050 M)x(0.025 M0.025 M)y2=2xx=1

Hence, the overall order of the reaction is 3.

b) The rate constant

The rate expression for the reaction is given as follows:

rate=k[NO]2[H2]k=rate[NO]2[H2]

Substitute the values of [NO], [H2], and rate of reaction in the above equation:

rate=2.4×10−6M/s[0.025M]2[0.010M]=2.4×10−6M/s3.125×10−6M=0.384s−1

Hence, the rate constant for the reaction is 0.38 s−1.

c) A plausible mechanism that is consistent to rate law.

The reaction between hydrogen with nitric oxide is as follows:

2H2(g)+2NO(g)→2H2O(g)+N2(g)

The plausible mechanism of the reaction, which isconsistent with the rate law, is given as follows:

Step−I: H2+2NO→N2O+H2O (slow)Step−II:N2O+H2→N2+H2O (fast)

The overall reaction is obtained as follows:

H2+2NO→N2O+H2ON2O+H2→N2+H2O_2H2+2NO→N2+2H2O_

Answer 12

Ch. 14.1 - Practice Problem ATTEMPT Write the rate...Ch. 14.1 - Practice ProblemBUILD Write the balanced equation...Ch. 14.1 - Prob. 1PPC Ch. 14.1 - 14.1.1 Which expressions are correct for the rate...Ch. 14.1 - 14.1.2 In the same reaction: if the concentration...Ch. 14.2 - Practice Problem ATTEMPT Consider the reaction:...Ch. 14.2 - Practice Problem BUILD Consider the following...Ch. 14.2 - Practice Problem CONCEPTUALIZE Consider the...Ch. 14.2 - Answer questions 14.2.1 through 14.2.4 using the...Ch. 14.2 - Answer questions 14.2.1 through 14.2.4 using the...

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Answer to Problem 80AP

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