Chapter 6.9, Problem 22P

Interpretation Introduction

(a)

Interpretation: Whether the given statement is true for a reaction with $K_{\text{eq}}=0.8$ and $E_{\text{a}}=80\text{kJ}/\text{mol}$ is to be stated. The false statement is to be corrected.

Concept introduction: The activation energy $\left(E_{\text{a}}\right)$ aids in determining the rate of the chemical reactions. The small value of $E_{\text{a}}$ exhibits that less energy is required to convert the reactants into products. It results in the increases of a rate of reaction.

The change in Gibbs free energy, enthalpy and entropy is represented by $\text{Δ}G°$, $\text{Δ}H\text{°}$ and $\text{Δ}S\text{°}$ respectively. They are state functions. The relation $\text{Δ}G°$ with $\text{Δ}H\text{°}$ and $\text{Δ}S\text{°}$ is shown as,

$\text{Δ}G\text{°}=\text{Δ}H\text{°}-T\text{Δ}S\text{°}$

The change in Gibbs free energy describes the spontaneity of the reaction. The change in enthalpy describes the relative bond strength in the substance, whereas the change in entropy describes the randomness in the system.

Interpretation Introduction

(b)

Interpretation: Whether the given statement is true for a reaction with $K_{\text{eq}}=0.8$ and $E_{\text{a}}=80\text{kJ}/\text{mol}$ is to be stated. The false statement is to be corrected.

Concept introduction: The activation energy $\left(E_{\text{a}}\right)$ aids in determining the rate of the chemical reactions. The small value of $E_{\text{a}}$ exhibits that less energy is required to convert the reactants into products. It results in the increases of a rate of reaction.

The change in Gibbs free energy, enthalpy and entropy is represented by $\text{Δ}G°$, $\text{Δ}H\text{°}$ and $\text{Δ}S\text{°}$ respectively. They are state functions. The relation $\text{Δ}G°$ with $\text{Δ}H\text{°}$ and $\text{Δ}S\text{°}$ is shown as,

$\text{Δ}G\text{°}=\text{Δ}H\text{°}-T\text{Δ}S\text{°}$

The change in Gibbs free energy describes the spontaneity of the reaction. The change in enthalpy describes the relative bond strength in the substance, whereas the change in entropy describes the randomness in the system.

Interpretation Introduction

(c)

Interpretation: Whether the given statement is true for a reaction with $K_{\text{eq}}=0.8$ and $E_{\text{a}}=80\text{kJ}/\text{mol}$ is to be stated. The false statement is to be corrected.

Concept introduction: The activation energy $\left(E_{\text{a}}\right)$ aids in determining the rate of the chemical reactions. The small value of $E_{\text{a}}$ exhibits that less energy is required to convert the reactants into products. It results in the increases of a rate of reaction.

The change in Gibbs free energy, enthalpy and entropy is represented by $\text{Δ}G°$, $\text{Δ}H\text{°}$ and $\text{Δ}S\text{°}$ respectively. They are state functions. The relation $\text{Δ}G°$ with $\text{Δ}H\text{°}$ and $\text{Δ}S\text{°}$ is shown as,

$\text{Δ}G\text{°}=\text{Δ}H\text{°}-T\text{Δ}S\text{°}$

The change in Gibbs free energy describes the spontaneity of the reaction. The change in enthalpy describes the relative bond strength in the substance, whereas the change in entropy describes the randomness in the system.

Interpretation Introduction

(d)

Interpretation: Whether the given statement is true for a reaction with $K_{\text{eq}}=0.8$ and $E_{\text{a}}=80\text{kJ}/\text{mol}$ is to be stated. The false statement is to be corrected.

Concept introduction: The activation energy $\left(E_{\text{a}}\right)$ aids in determining the rate of the chemical reactions. The small value of $E_{\text{a}}$ exhibits that less energy is required to convert the reactants into products. It results in the increases of a rate of reaction.

The change in Gibbs free energy, enthalpy and entropy is represented by $\text{Δ}G°$, $\text{Δ}H\text{°}$ and $\text{Δ}S\text{°}$ respectively. They are state functions. The relation $\text{Δ}G°$ with $\text{Δ}H\text{°}$ and $\text{Δ}S\text{°}$ is shown as,

$\text{Δ}G\text{°}=\text{Δ}H\text{°}-T\text{Δ}S\text{°}$

The change in Gibbs free energy describes the spontaneity of the reaction. The change in enthalpy describes the relative bond strength in the substance, whereas the change in entropy describes the randomness in the system.

Interpretation Introduction

(e)

Interpretation: Whether the given statement is true for a reaction with $K_{\text{eq}}=0.8$ and $E_{\text{a}}=80\text{kJ}/\text{mol}$ is to be stated. The false statement is to be corrected.

Concept introduction: The activation energy $\left(E_{\text{a}}\right)$ aids in determining the rate of the chemical reactions. The small value of $E_{\text{a}}$ exhibits that less energy is required to convert the reactants into products. It results in the increases of a rate of reaction.

The change in Gibbs free energy, enthalpy and entropy is represented by $\text{Δ}G°$, $\text{Δ}H\text{°}$ and $\text{Δ}S\text{°}$ respectively. They are state functions. The relation $\text{Δ}G°$ with $\text{Δ}H\text{°}$ and $\text{Δ}S\text{°}$ is shown as,

$\text{Δ}G\text{°}=\text{Δ}H\text{°}-T\text{Δ}S\text{°}$

The change in Gibbs free energy describes the spontaneity of the reaction. The change in enthalpy describes the relative bond strength in the substance, whereas the change in entropy describes the randomness in the system.