Chapter 3, Problem 19P

(a)

Interpretation Introduction

Interpretation: The value of $\Delta H°$ involved in formation of $\text{HF}$ 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 the system gains energy while when work is negative then the system loses energy. Heat is not a state function and therefore change in enthalpy of reaction $\left(\Delta H{°}_{\text{rxn}}\right)$ has been introduced. The formula to calculate $\Delta H°$ from bond dissociation of reactants and products is as follows:

  $\Delta H°=\text{Sum of }DH°\text{ of bonds broken}-\text{Sum of }DH°\text{ of bonds formed}$

(b)

Interpretation Introduction

Interpretation: The value of $\Delta H°$ involved in the formation of $\text{HCl}$ 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 the system gains energy while when work is negative then the system loses energy. Heat is not a state function and therefore change in enthalpy of reaction $\left(\Delta H{°}_{\text{rxn}}\right)$ has been introduced. The formula to calculate $\Delta H°$ from bond dissociation of reactants and products is as follows:

  $\Delta H°=\text{Sum of }DH°\text{ of bonds broken}-\text{Sum of }DH°\text{ of bonds formed}$

(c)

Interpretation Introduction

Interpretation: The value of $\Delta H°$ involved in formation of $\text{HBr}$ 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 the system gains energy while when work is negative then the system loses energy. Heat is not a state function and therefore change in enthalpy of reaction $\left(\Delta H{°}_{\text{rxn}}\right)$ has been introduced. The formula to calculate $\Delta H°$ from bond dissociation of reactants and products is as follows:

  $\Delta H°=\text{Sum of }DH°\text{ of bonds broken}-\text{Sum of }DH°\text{ of bonds formed}$

(d)

Interpretation Introduction

Interpretation: The value of $\Delta H°$ involved in formation of $\text{HI}$ 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 the system gains energy while when work is negative then the system loses energy. Heat is not a state function and therefore change in enthalpy of reaction $\left(\Delta H{°}_{\text{rxn}}\right)$ has been introduced. The formula to calculate $\Delta H°$ from bond dissociation of reactants and products is as follows:

  $\Delta H°=\text{Sum of }DH°\text{ of bonds broken}-\text{Sum of }DH°\text{ of bonds formed}$

(e)

Interpretation Introduction

Interpretation: The value of $\Delta H°$ involved in formation of $\left({\text{CH}}_3\right)\text{CF}$ and $\text{HF}$ 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 the system gains energy while when work is negative then the system loses energy. Heat is not a state function and therefore change in enthalpy of reaction $\left(\Delta H{°}_{\text{rxn}}\right)$ has been introduced. The formula to calculate $\Delta H°$ from bond dissociation of reactants and products is as follows:

  $\Delta H°=\text{Sum of }DH°\text{ of bonds broken}-\text{Sum of }DH°\text{ of bonds formed}$

(f)

Interpretation Introduction

Interpretation: The value of $\Delta H°$ involved in formation of $\left({\text{CH}}_3\right)\text{CCl}$ and $\text{HCl}$ 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 the system gains energy while when work is negative then the system loses energy. Heat is not a state function and therefore change in enthalpy of reaction $\left(\Delta H{°}_{\text{rxn}}\right)$ has been introduced. The formula to calculate $\Delta H°$ from bond dissociation of reactants and products is as follows:

  $\Delta H°=\text{Sum of }DH°\text{ of bonds broken}-\text{Sum of }DH°\text{ of bonds formed}$

(g)

Interpretation Introduction

Interpretation: The value of $\Delta H°$ involved in formation of $\left({\text{CH}}_3\right)\text{CBr}$ and $\text{HBr}$ 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 the system gains energy while when work is negative then the system loses energy. Heat is not a state function and therefore change in enthalpy of reaction $\left(\Delta H{°}_{\text{rxn}}\right)$ has been introduced. The formula to calculate $\Delta H°$ from bond dissociation of reactants and products is as follows:

  $\Delta H°=\text{Sum of }DH°\text{ of bonds broken}-\text{Sum of }DH°\text{ of bonds formed}$

(h)

Interpretation Introduction

Interpretation: The value of $\Delta H°$ involved in formation of $\left({\text{CH}}_3\right)\text{CI}$ and $\text{HI}$ 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 the system gains energy while when work is negative then the system loses energy. Heat is not a state function and therefore change in enthalpy of reaction $\left(\Delta H{°}_{\text{rxn}}\right)$ has been introduced. The formula to calculate $\Delta H°$ from bond dissociation of reactants and products is as follows:

  $\Delta H°=\text{Sum of }DH°\text{ of bonds broken}-\text{Sum of }DH°\text{ of bonds formed}$