The bond dissociation enthalpy required to estimate the enthalpy change for the given reaction should be identified. Concept Introduction: Bond dissociation enthalpy: Bond energy or more correctly the bond dissociation enthalpy is the enthalpy change when breaking a bond in a molecule with the reactant and products in the gas phase. The process of breaking bonds in a molecule is always endothermic, so Δ r H for bond breaking is always positive.

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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 8, Problem 63GQ

Interpretation Introduction

Interpretation: The bond dissociation enthalpy required to estimate the enthalpy change for the given reaction should be identified.

Concept Introduction:

Bond dissociation enthalpy:

Bond energy or more correctly the bond dissociation enthalpy is the enthalpy change when breaking a bond in a molecule with the reactant and products in the gas phase.

The process of breaking bonds in a molecule is always endothermic, so ΔrH for bond breaking is always positive.

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Calculate the enthalpy change from bond energies for each of these reactions: 1. Н-(g) + F:(g) — 2 HF(g) AH= 2. CH(g) + 20-(g) — СО2(g) + 2H-0 (g) AH= 3. CO(g) + 2H2(g) → CH;OH(I) AH= 4. 2H2(g) + Oz(g) – 2H;O(g) AH= 5. 2H2O(g) → 2H2(g) + O2(g) AH= 6. H2CCH2(g) + Cl2(g) → CIH2CCH2CI(g) AH=

Based on the given bond energy values, calculate the enthalpy of reaction, AHran- (in kJ). No need to write the units "kJ" in your answer on the provided space. Answer only with 3 Significant figures (so put appropriate number after decimal point). (e.g. 24.0) for 24.0 kJ ½ N2(g) + 3/2 X2(g) NX3(g) BE (in kJ): N= N: 940; X-X: 160; N-X: 240

Predict the enthalpy of reaction from the average bond enthalpies for the following reaction: 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(g) Bond Enthalpy (kJ/mol) H―H 436.4 H―O 460 C―H 414 C―C 347 C═C 620 C―O 351 O―O 142 O═O 498.7 C═O 745 C═O(in carbondioxide) 799 ______ kJ

Answer 2

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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 8, Problem 63GQ

Interpretation Introduction

Interpretation: The bond dissociation enthalpy required to estimate the enthalpy change for the given reaction should be identified.

Concept Introduction:

Bond dissociation enthalpy:

Bond energy or more correctly the bond dissociation enthalpy is the enthalpy change when breaking a bond in a molecule with the reactant and products in the gas phase.

The process of breaking bonds in a molecule is always endothermic, so ΔrH for bond breaking is always positive.

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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 8, Problem 63GQ

Interpretation Introduction

Interpretation: The bond dissociation enthalpy required to estimate the enthalpy change for the given reaction should be identified.

Concept Introduction:

Bond dissociation enthalpy:

Bond energy or more correctly the bond dissociation enthalpy is the enthalpy change when breaking a bond in a molecule with the reactant and products in the gas phase.

The process of breaking bonds in a molecule is always endothermic, so ΔrH for bond breaking is always positive.

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 8, Problem 63GQ

Interpretation Introduction