Standard enthalpy of hydrogenation of cyclohexene into cyclohexane has to be calculated. Concept Introduction: Heat of vaporization: At constant temperature and pressure, the amount of heat entails to convert a liquid into a gas. A gas produced same quantity of heat when it converts liquid. Enthalpy ( H ) : it is the total amount of heat in a particular system. The value of heat formed in a reaction ΔH is calculated by the formula, ΔH= ∑ ( B o n d D i s s o c i a t i o n E n e r g y ) ( reactants ) − ∑ ( B o n d D i s s o c i a t i o n E n e r g y ) ( products ) If the value obtained for ΔH in a reaction is positive then it is an endothermic reaction whereas the value obtained for ΔH is negative it is an exothermic reaction. Energy of Combustion: The energy released in the form of heat when given substance undergoes combustion reaction. Enthalpy change: It is defined as the amount of heat released or absorbed by the chemical reaction at constant pressure conditions.

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Answer 1

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Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 2, Problem 2F.7E

Interpretation Introduction

Interpretation:

Standard enthalpy of hydrogenation of cyclohexene into cyclohexane has to be calculated.

Concept Introduction:

Heat of vaporization: At constant temperature and pressure, the amount of heat entails to convert a liquid into a gas. A gas produced same quantity of heat when it converts liquid.

Enthalpy(H): it is the total amount of heat in a particular system.

The value of heat formed in a reaction ΔH is calculated by the formula,

ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)

If the value obtained for ΔH in a reaction is positive then it is an endothermic reaction whereas the value obtained for ΔH is negative it is an exothermic reaction.

Energy of Combustion: The energy released in the form of heat when given substance undergoes combustion reaction.

Enthalpy change: It is defined as the amount of heat released or absorbed by the chemical reaction at constant pressure conditions.

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Answer 2

Question

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 2, Problem 2F.7E

Interpretation Introduction

Interpretation:

Standard enthalpy of hydrogenation of cyclohexene into cyclohexane has to be calculated.

Concept Introduction:

Heat of vaporization: At constant temperature and pressure, the amount of heat entails to convert a liquid into a gas. A gas produced same quantity of heat when it converts liquid.

Enthalpy(H): it is the total amount of heat in a particular system.

The value of heat formed in a reaction ΔH is calculated by the formula,

ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)

If the value obtained for ΔH in a reaction is positive then it is an endothermic reaction whereas the value obtained for ΔH is negative it is an exothermic reaction.

Energy of Combustion: The energy released in the form of heat when given substance undergoes combustion reaction.

Enthalpy change: It is defined as the amount of heat released or absorbed by the chemical reaction at constant pressure conditions.

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Answer 3

Question

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 2, Problem 2F.7E

Interpretation Introduction

Interpretation:

Standard enthalpy of hydrogenation of cyclohexene into cyclohexane has to be calculated.

Concept Introduction:

Heat of vaporization: At constant temperature and pressure, the amount of heat entails to convert a liquid into a gas. A gas produced same quantity of heat when it converts liquid.

Enthalpy(H): it is the total amount of heat in a particular system.

The value of heat formed in a reaction ΔH is calculated by the formula,

ΔH=∑(Bond Dissociation Energy)(reactants) −∑(Bond Dissociation Energy)(products)

If the value obtained for ΔH in a reaction is positive then it is an endothermic reaction whereas the value obtained for ΔH is negative it is an exothermic reaction.

Energy of Combustion: The energy released in the form of heat when given substance undergoes combustion reaction.

Enthalpy change: It is defined as the amount of heat released or absorbed by the chemical reaction at constant pressure conditions.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.

Chapter 2, Problem 2F.7E

Interpretation Introduction