The heat of combustion of acetylene has to be calculated and the answer should be reported in kilojoules per mole (kJ/mol) and in kilojoules per gram (kJ/g). Concept Introduction: Heat of combustion: It is also known as potential heat of fuel. Heat of combustion of carbon depends on its allotropic form. A fuel is a substance which releases energy in the form of heat while undergoing combustion. Hydrocarbons which have high heats of combustion make it a best fuel. Combustion reaction: It is the reaction in which hydrocarbons are heated in presence of oxygen results to give water and carbon dioxide with heat. 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. Δ r H 0 = Σ Δ H ( b o n d s b r o k e n ) − Σ Δ H ( b o n d s f o r m e d )

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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 5.5, Problem 5.13YT

Interpretation Introduction

Interpretation:

The heat of combustion of acetylene has to be calculated and the answer should be reported in kilojoules per mole (kJ/mol) and in kilojoules per gram (kJ/g).

Concept Introduction:

Heat of combustion: It is also known as potential heat of fuel. Heat of combustion of carbon depends on its allotropic form.

A fuel is a substance which releases energy in the form of heat while undergoing combustion. Hydrocarbons which have high heats of combustion make it a best fuel.

Combustion reaction: It is the reaction in which hydrocarbons are heated in presence of oxygen results to give water and carbon dioxide with heat.

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.

ΔrH0 = Σ ΔH (bonds broken) −Σ ΔH (bonds formed)

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Practice Exercise 1If the heat of formation of H2O1l2 is -286 kJ>mol, whichof the following thermochemical equations is correct?(a) 2 H1g2 + O1g2¡H2O1l2 ΔH = -286 kJ(b) 2 H21g2 + O21g2¡2 H2O1l2 ΔH = -286 kJ(c) H21g2 + 12 O21g2¡H2O1l2 ΔH = -286 kJ(d) H21g2 + O1g2¡H2O1g2 ΔH = -286 kJ(e) H2O1l2¡H21g2 + 12O21g2 ΔH = -286 kJ

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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 5.5, Problem 5.13YT

Interpretation Introduction

Interpretation:

The heat of combustion of acetylene has to be calculated and the answer should be reported in kilojoules per mole (kJ/mol) and in kilojoules per gram (kJ/g).

Concept Introduction:

Heat of combustion: It is also known as potential heat of fuel. Heat of combustion of carbon depends on its allotropic form.

A fuel is a substance which releases energy in the form of heat while undergoing combustion. Hydrocarbons which have high heats of combustion make it a best fuel.

Combustion reaction: It is the reaction in which hydrocarbons are heated in presence of oxygen results to give water and carbon dioxide with heat.

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.

ΔrH0 = Σ ΔH (bonds broken) −Σ ΔH (bonds formed)

Expert Solution & Answer

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Check out a sample textbook solution

See solution

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 5.5, Problem 5.13YT

Interpretation Introduction

Interpretation:

The heat of combustion of acetylene has to be calculated and the answer should be reported in kilojoules per mole (kJ/mol) and in kilojoules per gram (kJ/g).

Concept Introduction:

Heat of combustion: It is also known as potential heat of fuel. Heat of combustion of carbon depends on its allotropic form.

A fuel is a substance which releases energy in the form of heat while undergoing combustion. Hydrocarbons which have high heats of combustion make it a best fuel.

Combustion reaction: It is the reaction in which hydrocarbons are heated in presence of oxygen results to give water and carbon dioxide with heat.

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.

ΔrH0 = Σ ΔH (bonds broken) −Σ ΔH (bonds formed)

Expert Solution & Answer

Want to see the full answer?

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 5.5, Problem 5.13YT

Interpretation Introduction