Using the collision theory the frequency factor for the given reaction has to be estimated. The measured value might be rather lower than that calculated. It has to be reasoned. Concept Introduction: Activation energy ( E a ) : The energy of activation in a chemical reaction is a measure of the energy needed for the conversion of the substrate molecules to the reactive state. The enzyme catalysts are more efficient in lower the energy activation. Example: The decomposition of H 2 O 2 require 18 k c a l / m o l of energy without catalyst, but only 2 k c a l / m o l e in the presence of enzyme catalase. Kinetic-molecular theory of gases: Gases are made up of particles like atoms or molecules which randomly moves and there will be no attractive forces between them. Comparing the space occupied by the gas particles and the space between particles, the former is much smaller than the latter. The average kinetic energy of gas particles and the Kelvin temperature is proportional. There is an elastic collision between gas particles or with the wall of their container and thus no energy is lost during collision and total kinetic energy of the particles is constant.

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Answer 1

Question

Chapter 6, Problem 6D.10E

Interpretation Introduction

Interpretation:

Using the collision theory the frequency factor for the given reaction has to be estimated. The measured value might be rather lower than that calculated. It has to be reasoned.

Concept Introduction:

Activation energy(Ea): The energy of activation in a chemical reaction is a measure of the energy needed for the conversion of the substrate molecules to the reactive state.

The enzyme catalysts are more efficient in lower the energy activation.

Example: The decomposition of H2O2 require 18 kcal/mol of energy without catalyst, but only 2 kcal/mole in the presence of enzyme catalase.

Kinetic-molecular theory of gases:

Gases are made up of particles like atoms or molecules which randomly moves and there will be no attractive forces between them.

Comparing the space occupied by the gas particles and the space between particles, the former is much smaller than the latter.

The average kinetic energy of gas particles and the Kelvin temperature is proportional.

There is an elastic collision between gas particles or with the wall of their container and thus no energy is lost during collision and total kinetic energy of the particles is constant.

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Answer 2

Question

Chapter 6, Problem 6D.10E

Interpretation Introduction

Interpretation:

Using the collision theory the frequency factor for the given reaction has to be estimated. The measured value might be rather lower than that calculated. It has to be reasoned.

Concept Introduction:

Activation energy(Ea): The energy of activation in a chemical reaction is a measure of the energy needed for the conversion of the substrate molecules to the reactive state.

The enzyme catalysts are more efficient in lower the energy activation.

Example: The decomposition of H2O2 require 18 kcal/mol of energy without catalyst, but only 2 kcal/mole in the presence of enzyme catalase.

Kinetic-molecular theory of gases:

Gases are made up of particles like atoms or molecules which randomly moves and there will be no attractive forces between them.

Comparing the space occupied by the gas particles and the space between particles, the former is much smaller than the latter.

The average kinetic energy of gas particles and the Kelvin temperature is proportional.

There is an elastic collision between gas particles or with the wall of their container and thus no energy is lost during collision and total kinetic energy of the particles is constant.

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Answer 3

Question

Chapter 6, Problem 6D.10E

Interpretation Introduction

Interpretation:

Using the collision theory the frequency factor for the given reaction has to be estimated. The measured value might be rather lower than that calculated. It has to be reasoned.

Concept Introduction:

Activation energy(Ea): The energy of activation in a chemical reaction is a measure of the energy needed for the conversion of the substrate molecules to the reactive state.

The enzyme catalysts are more efficient in lower the energy activation.

Example: The decomposition of H2O2 require 18 kcal/mol of energy without catalyst, but only 2 kcal/mole in the presence of enzyme catalase.

Kinetic-molecular theory of gases:

Gases are made up of particles like atoms or molecules which randomly moves and there will be no attractive forces between them.

Comparing the space occupied by the gas particles and the space between particles, the former is much smaller than the latter.

The average kinetic energy of gas particles and the Kelvin temperature is proportional.

There is an elastic collision between gas particles or with the wall of their container and thus no energy is lost during collision and total kinetic energy of the particles is constant.

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Answer 4

Question

Chapter 6, Problem 6D.10E

Interpretation Introduction

Interpretation:

Using the collision theory the frequency factor for the given reaction has to be estimated. The measured value might be rather lower than that calculated. It has to be reasoned.

Concept Introduction:

Activation energy(Ea): The energy of activation in a chemical reaction is a measure of the energy needed for the conversion of the substrate molecules to the reactive state.

The enzyme catalysts are more efficient in lower the energy activation.

Example: The decomposition of H2O2 require 18 kcal/mol of energy without catalyst, but only 2 kcal/mole in the presence of enzyme catalase.

Kinetic-molecular theory of gases:

Gases are made up of particles like atoms or molecules which randomly moves and there will be no attractive forces between them.

Comparing the space occupied by the gas particles and the space between particles, the former is much smaller than the latter.

The average kinetic energy of gas particles and the Kelvin temperature is proportional.

There is an elastic collision between gas particles or with the wall of their container and thus no energy is lost during collision and total kinetic energy of the particles is constant.

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Answer 5

Chapter 6, Problem 6D.10E

Interpretation Introduction

Interpretation:

Using the collision theory the frequency factor for the given reaction has to be estimated. The measured value might be rather lower than that calculated. It has to be reasoned.

Concept Introduction:

Activation energy(Ea): The energy of activation in a chemical reaction is a measure of the energy needed for the conversion of the substrate molecules to the reactive state.

The enzyme catalysts are more efficient in lower the energy activation.

Example: The decomposition of H2O2 require 18 kcal/mol of energy without catalyst, but only 2 kcal/mole in the presence of enzyme catalase.

Kinetic-molecular theory of gases:

Gases are made up of particles like atoms or molecules which randomly moves and there will be no attractive forces between them.

Comparing the space occupied by the gas particles and the space between particles, the former is much smaller than the latter.

The average kinetic energy of gas particles and the Kelvin temperature is proportional.

There is an elastic collision between gas particles or with the wall of their container and thus no energy is lost during collision and total kinetic energy of the particles is constant.

Answer 6

Chapter 6, Problem 6D.10E

Interpretation Introduction

Interpretation:

Using the collision theory the frequency factor for the given reaction has to be estimated. The measured value might be rather lower than that calculated. It has to be reasoned.

Concept Introduction:

Activation energy(Ea): The energy of activation in a chemical reaction is a measure of the energy needed for the conversion of the substrate molecules to the reactive state.

The enzyme catalysts are more efficient in lower the energy activation.

Example: The decomposition of H2O2 require 18 kcal/mol of energy without catalyst, but only 2 kcal/mole in the presence of enzyme catalase.

Kinetic-molecular theory of gases:

Gases are made up of particles like atoms or molecules which randomly moves and there will be no attractive forces between them.

Comparing the space occupied by the gas particles and the space between particles, the former is much smaller than the latter.

The average kinetic energy of gas particles and the Kelvin temperature is proportional.

There is an elastic collision between gas particles or with the wall of their container and thus no energy is lost during collision and total kinetic energy of the particles is constant.

Answer 7

Chapter 6, Problem 6D.10E

Interpretation Introduction

Interpretation:

Using the collision theory the frequency factor for the given reaction has to be estimated. The measured value might be rather lower than that calculated. It has to be reasoned.

Concept Introduction:

Activation energy(Ea): The energy of activation in a chemical reaction is a measure of the energy needed for the conversion of the substrate molecules to the reactive state.

The enzyme catalysts are more efficient in lower the energy activation.

Example: The decomposition of H2O2 require 18 kcal/mol of energy without catalyst, but only 2 kcal/mole in the presence of enzyme catalase.

Kinetic-molecular theory of gases:

Gases are made up of particles like atoms or molecules which randomly moves and there will be no attractive forces between them.

Comparing the space occupied by the gas particles and the space between particles, the former is much smaller than the latter.

The average kinetic energy of gas particles and the Kelvin temperature is proportional.

There is an elastic collision between gas particles or with the wall of their container and thus no energy is lost during collision and total kinetic energy of the particles is constant.

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 6 - Prob. 6A.1ST Ch. 6 - Prob. 6A.2ST Ch. 6 - Prob. 6A.3ST Ch. 6 - Prob. 6B.1ST Ch. 6 - Prob. 6B.2ST Ch. 6 - Prob. 6B.3ST Ch. 6 - Prob. 6B.4ST Ch. 6 - Prob. 6C.1ST Ch. 6 - Prob. 6C.2ST Ch. 6 - Prob. 6C.3ST

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