Chapter 2, Problem 32P

(a)

Interpretation Introduction

Interpretation: The value of $\Delta H°$ of below reactions is to be calculated from the bond strength data.

  

Concept introduction: 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 $\Delta S°$ should be assigned for each below reaction and reason should be briefly explained.

  

Concept introduction: The formula that determines spontaneity of the reaction is,

  $\Delta G°=\Delta H°-T\Delta S°$

Where,

• $\Delta S°$denotes entropy change of reaction.
• $\Delta H°$denotes enthalpy change of reaction.
• $T$denotes temperature.
• $\Delta G°$denotes standard Gibbs energy.

(c)

Interpretation Introduction

Interpretation: The value of $\Delta G°$ is to be calculated for each reaction at $25°\text{C}$ and $\text{600 }°\text{C}$ also, whether reactions are thermodynamically favorable at $25°\text{C}$ and $\text{600 }°\text{C}$ should be determined.

Concept introduction: The formula that determines spontaneity of the reaction is,

  $\Delta G°=\Delta H°-T\Delta S°$

Where,

• $\Delta S°$denotes entropy change of reaction.
• $\Delta H°$denotes enthalpy change of reaction.
• $T$denotes temperature.
• $\Delta G°$denotes standard Gibbs energy.