The bond dissociation energy of NO using the bond dissociation energies of O 2 and N 2 and their formation enthalpy values should be determined. Concept introduction: NO ( g ) is formed from N 2 ( g ) and O 2 ( g ) . Therefore, formation enthalpies can be used to determine the reaction enthalpy that occur between N 2 ( g ) and O 2 ( g ) to form NO ( g ) and from which bond dissociation energy of NO ( g ) can be calculated.

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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 10, Problem 108IAE

Interpretation Introduction

Interpretation:

The bond dissociation energy of NO using the bond dissociation energies of O₂ and N₂ and their formation enthalpy values should be determined.

Concept introduction:

NO₍_g₎ is formed from N₂₍_g₎ and O₂₍_g₎. Therefore, formation enthalpies can be used to determine the reaction enthalpy that occur between N₂₍_g₎ and O₂₍_g₎ to form NO₍_g₎ and from which bond dissociation energy of NO₍_g₎ can be calculated.

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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 10, Problem 108IAE

Interpretation Introduction

Interpretation:

The bond dissociation energy of NO using the bond dissociation energies of O₂ and N₂ and their formation enthalpy values should be determined.

Concept introduction:

NO₍_g₎ is formed from N₂₍_g₎ and O₂₍_g₎. Therefore, formation enthalpies can be used to determine the reaction enthalpy that occur between N₂₍_g₎ and O₂₍_g₎ to form NO₍_g₎ and from which bond dissociation energy of NO₍_g₎ can be calculated.

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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 10, Problem 108IAE

Interpretation Introduction

Interpretation:

The bond dissociation energy of NO using the bond dissociation energies of O₂ and N₂ and their formation enthalpy values should be determined.

Concept introduction:

NO₍_g₎ is formed from N₂₍_g₎ and O₂₍_g₎. Therefore, formation enthalpies can be used to determine the reaction enthalpy that occur between N₂₍_g₎ and O₂₍_g₎ to form NO₍_g₎ and from which bond dissociation energy of NO₍_g₎ can be calculated.

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 10, Problem 108IAE

Interpretation Introduction