Chapter 6.3, Problem 4CC

(a)

Interpretation Introduction

Interpretation:

For the given set of reaction conditions the sign of $\text{ΔG}$ and its behavior in response to increase in temperature should be predicted.

Concept introduction:

Gibbs free energy: The Gibbs free energy depends on the two terms entropy change and the enthalpy change which is affected by the temperature.

General formula to calculate the Gibbs free energy is $\text{ΔG = ΔΗ –TΔS}$

When the heat energy was absorbed by the system from the surrounding is called endothermic reaction

When heat energy or light energy was unconfined to the surrounding from the system is called exothermic reaction.

Entropy: It is usually defined as the degree of the randomness or disorder present in the respective system.

The total entropy change associated with given reaction is equal to the sum of both entropy change associated with the system and the surrounding.

The entropy change within the system is the difference between the final and the initial states in the system. The entropy change in the given chemical reaction is as follows

$\text{ΔS = Number of products – Number of reactants}$

Enthalpy:

The enthalpy change for the reaction is determined by bond breaks and bond formation in the reaction.

$\text{ΔΗ}$ (Enthalpy), $\text{ΔS}$ (Entropy) and $\text{ΔG}$ (Gibbs free energy) can be identified by using formula.

$\text{ΔΗ}$ (Enthalpy) could be determined by using following formula

$\text{ΔΗ}$ (Enthalpy of the reaction) = $\text{ΔΗ }\left(\text{bonds broken}\right)\text{ – ΔΗ (bonds formed)}$

(b)

Interpretation Introduction

Interpretation:

For the given set of reaction conditions the sign of $\text{ΔG}$ and its behavior in response to increase in temperature should be predicted.

Concept introduction:

Gibbs free energy: The Gibbs free energy depends on the two terms entropy change and the enthalpy change which is affected by the temperature.

General formula to calculate the Gibbs free energy is $\text{ΔG = ΔΗ –TΔS}$

When the heat energy was absorbed by the system from the surrounding is called endothermic reaction

When heat energy or light energy was unconfined to the surrounding from the system is called exothermic reaction.

Entropy: It is usually defined as the degree of the randomness or disorder present in the respective system.

The total entropy change associated with given reaction is equal to the sum of both entropy change associated with the system and the surrounding.

The entropy change within the system is the difference between the final and the initial states in the system. The entropy change in the given chemical reaction is as follows

$\text{ΔS = Number of products – Number of reactants}$

Enthalpy:

The enthalpy change for the reaction is determined by bond breaks and bond formation in the reaction.

$\text{ΔΗ}$ (Enthalpy), $\text{ΔS}$ (Entropy) and $\text{ΔG}$ (Gibbs free energy) can be identified by using formula.

$\text{ΔΗ}$ (Enthalpy) could be determined by using following formula

$\text{ΔΗ}$ (Enthalpy of the reaction) = $\text{ΔΗ }\left(\text{bonds broken}\right)\text{ – ΔΗ (bonds formed)}$

(c)

Interpretation Introduction

Interpretation:

For the given set of reaction conditions the sign of $\text{ΔG}$ and its behavior in response to increase in temperature should be predicted.

Concept introduction:

Gibbs free energy: The Gibbs free energy depends on the two terms entropy change and the enthalpy change which is affected by the temperature.

General formula to calculate the Gibbs free energy is $\text{ΔG = ΔΗ –TΔS}$

When the heat energy was absorbed by the system from the surrounding is called endothermic reaction

When heat energy or light energy was unconfined to the surrounding from the system is called exothermic reaction.

Entropy: It is usually defined as the degree of the randomness or disorder present in the respective system.

The total entropy change associated with given reaction is equal to the sum of both entropy change associated with the system and the surrounding.

The entropy change within the system is the difference between the final and the initial states in the system. The entropy change in the given chemical reaction is as follows

$\text{ΔS = Number of products – Number of reactants}$

Enthalpy:

The enthalpy change for the reaction is determined by bond breaks and bond formation in the reaction.

$\text{ΔΗ}$ (Enthalpy), $\text{ΔS}$ (Entropy) and $\text{ΔG}$ (Gibbs free energy) can be identified by using formula.

$\text{ΔΗ}$ (Enthalpy) could be determined by using following formula

$\text{ΔΗ}$ (Enthalpy of the reaction) = $\text{ΔΗ }\left(\text{bonds broken}\right)\text{ – ΔΗ (bonds formed)}$

(d)

Interpretation Introduction

Interpretation:

For the given set of reaction conditions the sign of $\text{ΔG}$ and its behavior in response to increase in temperature should be predicted.

Concept introduction:

Gibbs free energy: The Gibbs free energy depends on the two terms entropy change and the enthalpy change which is affected by the temperature.

General formula to calculate the Gibbs free energy is $\text{ΔG = ΔΗ –TΔS}$

When the heat energy was absorbed by the system from the surrounding is called endothermic reaction

When heat energy or light energy was unconfined to the surrounding from the system is called exothermic reaction.

Entropy: It is usually defined as the degree of the randomness or disorder present in the respective system.

The total entropy change associated with given reaction is equal to the sum of both entropy change associated with the system and the surrounding.

The entropy change within the system is the difference between the final and the initial states in the system. The entropy change in the given chemical reaction is as follows

$\text{ΔS = Number of products – Number of reactants}$

Enthalpy:

The enthalpy change for the reaction is determined by bond breaks and bond formation in the reaction.

$\text{ΔΗ}$ (Enthalpy), $\text{ΔS}$ (Entropy) and $\text{ΔG}$ (Gibbs free energy) can be identified by using formula.

$\text{ΔΗ}$ (Enthalpy) could be determined by using following formula

$\text{ΔΗ}$ (Enthalpy of the reaction) = $\text{ΔΗ }\left(\text{bonds broken}\right)\text{ – ΔΗ (bonds formed)}$