The fraction of the molecules in a gas at 300 K, which collide with energy equal to or greater than E a . and the fraction of the molecules in the gas at the same temperatureif E a is doubled should be identified. Concept introduction: Based on collision theory, a reaction takes place because the reactant molecules collide with each other. However, if the collision is not effective, it does not turn into products. Hence, in order to achieve a product, there must be effective collision taking place. If any molecule can perform effective collisions, there must be some energy. This energy is always greater than the minimum energy of a molecule possesses called Threshold Energy. Any energy which greater than this energy is called Activation Energy, which isa must to form a product from the reactants. Therefore, Activation Energy = Threshold Energy − Average kinetic energy of reactants. From the given Activation Energy, we can calculate the number of fraction of molecules in any of the gaseous reaction at a given temperature. Given: Temperature = 300K Activation Energy = E a = 50 kJ/mol. Activation Energy = E a = 100 kJ/mol.

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Answer 1

Question

Chapter 13, Problem 13.127CP

Interpretation Introduction

Interpretation:

The fraction of the molecules in a gas at 300 K, which collide with energy equal to or greater than E_a. and the fraction of the molecules in the gas at the same temperatureif E_a is doubled should be identified.

Concept introduction:

Based on collision theory, a reaction takes place because the reactant molecules collide with each other. However, if the collision is not effective, it does not turn into products. Hence, in order to achieve a product, there must be effective collision taking place. If any molecule can perform effective collisions, there must be some energy. This energy is always greater than the minimum energy of a molecule possesses called Threshold Energy. Any energy which greater than this energy is called Activation Energy, which isa must to form a product from the reactants.

Therefore, Activation Energy = Threshold Energy − Average kinetic energy of reactants.

From the given Activation Energy, we can calculate the number of fraction of molecules in any of the gaseous reaction at a given temperature.

Given:

Temperature = 300K
Activation Energy = E_a = 50 kJ/mol.
Activation Energy = E_a = 100 kJ/mol.

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Answer 2

Question

Chapter 13, Problem 13.127CP

Interpretation Introduction

Interpretation:

The fraction of the molecules in a gas at 300 K, which collide with energy equal to or greater than E_a. and the fraction of the molecules in the gas at the same temperatureif E_a is doubled should be identified.

Concept introduction:

Based on collision theory, a reaction takes place because the reactant molecules collide with each other. However, if the collision is not effective, it does not turn into products. Hence, in order to achieve a product, there must be effective collision taking place. If any molecule can perform effective collisions, there must be some energy. This energy is always greater than the minimum energy of a molecule possesses called Threshold Energy. Any energy which greater than this energy is called Activation Energy, which isa must to form a product from the reactants.

Therefore, Activation Energy = Threshold Energy − Average kinetic energy of reactants.

From the given Activation Energy, we can calculate the number of fraction of molecules in any of the gaseous reaction at a given temperature.

Given:

Temperature = 300K
Activation Energy = E_a = 50 kJ/mol.
Activation Energy = E_a = 100 kJ/mol.

Expert Solution & Answer

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Check out a sample textbook solution

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Answer 3

Question

Chapter 13, Problem 13.127CP

Interpretation Introduction

Interpretation:

The fraction of the molecules in a gas at 300 K, which collide with energy equal to or greater than E_a. and the fraction of the molecules in the gas at the same temperatureif E_a is doubled should be identified.

Concept introduction:

Based on collision theory, a reaction takes place because the reactant molecules collide with each other. However, if the collision is not effective, it does not turn into products. Hence, in order to achieve a product, there must be effective collision taking place. If any molecule can perform effective collisions, there must be some energy. This energy is always greater than the minimum energy of a molecule possesses called Threshold Energy. Any energy which greater than this energy is called Activation Energy, which isa must to form a product from the reactants.

Therefore, Activation Energy = Threshold Energy − Average kinetic energy of reactants.

From the given Activation Energy, we can calculate the number of fraction of molecules in any of the gaseous reaction at a given temperature.

Given:

Temperature = 300K
Activation Energy = E_a = 50 kJ/mol.
Activation Energy = E_a = 100 kJ/mol.

Expert Solution & Answer

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Answer 4

Question

Chapter 13, Problem 13.127CP

Interpretation Introduction

Interpretation:

The fraction of the molecules in a gas at 300 K, which collide with energy equal to or greater than E_a. and the fraction of the molecules in the gas at the same temperatureif E_a is doubled should be identified.

Concept introduction:

Based on collision theory, a reaction takes place because the reactant molecules collide with each other. However, if the collision is not effective, it does not turn into products. Hence, in order to achieve a product, there must be effective collision taking place. If any molecule can perform effective collisions, there must be some energy. This energy is always greater than the minimum energy of a molecule possesses called Threshold Energy. Any energy which greater than this energy is called Activation Energy, which isa must to form a product from the reactants.

Therefore, Activation Energy = Threshold Energy − Average kinetic energy of reactants.

From the given Activation Energy, we can calculate the number of fraction of molecules in any of the gaseous reaction at a given temperature.

Given:

Temperature = 300K
Activation Energy = E_a = 50 kJ/mol.
Activation Energy = E_a = 100 kJ/mol.

Expert Solution & Answer

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Answer 5

Chapter 13, Problem 13.127CP

Interpretation Introduction

Interpretation:

The fraction of the molecules in a gas at 300 K, which collide with energy equal to or greater than E_a. and the fraction of the molecules in the gas at the same temperatureif E_a is doubled should be identified.

Concept introduction:

Based on collision theory, a reaction takes place because the reactant molecules collide with each other. However, if the collision is not effective, it does not turn into products. Hence, in order to achieve a product, there must be effective collision taking place. If any molecule can perform effective collisions, there must be some energy. This energy is always greater than the minimum energy of a molecule possesses called Threshold Energy. Any energy which greater than this energy is called Activation Energy, which isa must to form a product from the reactants.

Therefore, Activation Energy = Threshold Energy − Average kinetic energy of reactants.

From the given Activation Energy, we can calculate the number of fraction of molecules in any of the gaseous reaction at a given temperature.

Given:

Temperature = 300K
Activation Energy = E_a = 50 kJ/mol.
Activation Energy = E_a = 100 kJ/mol.

Answer 6

Chapter 13, Problem 13.127CP

Interpretation Introduction

Interpretation:

The fraction of the molecules in a gas at 300 K, which collide with energy equal to or greater than E_a. and the fraction of the molecules in the gas at the same temperatureif E_a is doubled should be identified.

Concept introduction:

Based on collision theory, a reaction takes place because the reactant molecules collide with each other. However, if the collision is not effective, it does not turn into products. Hence, in order to achieve a product, there must be effective collision taking place. If any molecule can perform effective collisions, there must be some energy. This energy is always greater than the minimum energy of a molecule possesses called Threshold Energy. Any energy which greater than this energy is called Activation Energy, which isa must to form a product from the reactants.

Therefore, Activation Energy = Threshold Energy − Average kinetic energy of reactants.

From the given Activation Energy, we can calculate the number of fraction of molecules in any of the gaseous reaction at a given temperature.

Given:

Temperature = 300K
Activation Energy = E_a = 50 kJ/mol.
Activation Energy = E_a = 100 kJ/mol.

Answer 7

Chapter 13, Problem 13.127CP

Interpretation Introduction

Interpretation:

The fraction of the molecules in a gas at 300 K, which collide with energy equal to or greater than E_a. and the fraction of the molecules in the gas at the same temperatureif E_a is doubled should be identified.

Concept introduction:

Based on collision theory, a reaction takes place because the reactant molecules collide with each other. However, if the collision is not effective, it does not turn into products. Hence, in order to achieve a product, there must be effective collision taking place. If any molecule can perform effective collisions, there must be some energy. This energy is always greater than the minimum energy of a molecule possesses called Threshold Energy. Any energy which greater than this energy is called Activation Energy, which isa must to form a product from the reactants.

Therefore, Activation Energy = Threshold Energy − Average kinetic energy of reactants.

From the given Activation Energy, we can calculate the number of fraction of molecules in any of the gaseous reaction at a given temperature.

Given:

Temperature = 300K
Activation Energy = E_a = 50 kJ/mol.
Activation Energy = E_a = 100 kJ/mol.

Answer 8

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Answer 9

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Answer 10

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Answer 11

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

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