The value of Δ H ° involved in formation of CH 3 Cl and HCl should be calculated. Concept introduction: Thermodynamics is a study of energy transfers that can be done by either heat or work. The energy transferred through work involves force. When work is positive then system gains energy while when work is negative then system loses energy. Heat is not a state function and therefore change in enthalpy of reaction ( Δ H ° rxn ) has been introduced. The formula that Δ H ° from bond dissociation of reactants and products is as follows: Δ H ° = Sum of D H ° of bonds broken − Sum of D H ° of bonds formed

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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 3, Problem 51P

Interpretation Introduction

Interpretation: The value of ΔH° involved in formation of CH3Cl and HCl should be calculated.

Concept introduction: Thermodynamics is a study of energy transfers that can be done by either heat or work. The energy transferred through work involves force. When work is positive then system gains energy while when work is negative then system loses energy. Heat is not a state function and therefore change in enthalpy of reaction (ΔH°rxn) has been introduced. The formula that ΔH° from bond dissociation of reactants and products is as follows:

ΔH°=Sum of DH° of bonds broken−Sum of DH° of bonds formed

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MISSED THIS? Read Section 19.9 (Pages 878-881); Watch IWE 19.10 Consider the following reaction: CH3OH(g) CO(g) + 2H2(g) (Note that AG,CH3OH(g) = -162.3 kJ/mol and AG,co(g)=-137.2 kJ/mol.) Part A Calculate AG for this reaction at 25 °C under the following conditions: PCH₂OH Pco PH2 0.815 atm = 0.140 atm 0.170 atm Express your answer in kilojoules to three significant figures. Ο ΑΣΦ AG = -150 Submit Previous Answers Request Answer □? kJ × Incorrect; Try Again; 2 attempts remaining Calculate the free energy change under nonstandard conditions (AGrxn) by using the following relationship: AGrxn = AGrxn + RTInQ, AGxn+RTInQ, where AGxn is the standard free energy change, R is the ideal gas constant, T is the temperature in kelvins, a is the reaction quotient. Provide Feedback Next >

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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 3, Problem 51P

Interpretation Introduction

Interpretation: The value of ΔH° involved in formation of CH3Cl and HCl should be calculated.

Concept introduction: Thermodynamics is a study of energy transfers that can be done by either heat or work. The energy transferred through work involves force. When work is positive then system gains energy while when work is negative then system loses energy. Heat is not a state function and therefore change in enthalpy of reaction (ΔH°rxn) has been introduced. The formula that ΔH° from bond dissociation of reactants and products is as follows:

ΔH°=Sum of DH° of bonds broken−Sum of DH° of bonds formed

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Answer 3

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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 3, Problem 51P

Interpretation Introduction

Interpretation: The value of ΔH° involved in formation of CH3Cl and HCl should be calculated.

Concept introduction: Thermodynamics is a study of energy transfers that can be done by either heat or work. The energy transferred through work involves force. When work is positive then system gains energy while when work is negative then system loses energy. Heat is not a state function and therefore change in enthalpy of reaction (ΔH°rxn) has been introduced. The formula that ΔH° from bond dissociation of reactants and products is as follows:

ΔH°=Sum of DH° of bonds broken−Sum of DH° of bonds formed

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Answer 4

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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 3, Problem 51P

Interpretation Introduction