For the steam forming and water-gas shift reaction, the ΔG o and ΔH o values have to be calculated at 1000 o C , using the equilibrium free energy and enthalpy values. Concept introduction: Enthalpy is the amount energy absorbed or released in a process. The enthalpy change in a system (Δ Η sys ) can be calculated by the following equation. ΔH rxn = ∑ ΔH ° produdcts - ∑ ΔH ° reactants Where, ΔH f o ( reactants ) is the standard enthalpy of the reactants ΔH f o ( produdcts ) is the standard enthalpy of the products Entropy is the measure of randomness in the system. Standard entropy change in a reaction is the difference in entropy of the products and reactants. (ΔS ° rxn ) can be calculated by the following equation. ΔS ° rxn = ∑ m S ° Products - ∑ n S ° reactants Where, S ° reactants is the standard entropy of the reactants S ° Products is the standard entropy of the products Standard entropy change in a reaction and entropy change in the system are same. Free energy change is the term that is used to explain the total energy content in a thermodynamic system that can be converted into work. The free energy is represented by the letter G. All spontaneous process is associated with the decrease of free energy in the system. The equation given below helps us to calculate the change in free energy in a system. ΔG o = Δ Η o - T Δ S o Where, Δ Η o is the change in enthalpy of the system ΔG o is the standard change in free energy of the system T is the absolute value of the temperature

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Answer 1

Question

Chapter 20, Problem 20.111P

(a)

Interpretation Introduction

Interpretation:

For the steam forming and water-gas shift reaction, the $ΔGo and ΔHo$ values have to be calculated at $1000 oC$ , using the equilibrium free energy and enthalpy values.

Concept introduction:

Enthalpy is the amount energy absorbed or released in a process.

The enthalpy change in a system $(ΔΗsys)$ can be calculated by the following equation.

$ΔHrxn = ∑ΔH°produdcts-∑ΔH°reactants$

Where,

$ΔHfo(reactants)$ is the standard enthalpy of the reactants

$ΔHfo(produdcts)$ is the standard enthalpy of the products

Entropy is the measure of randomness in the system. Standard entropy change in a reaction is the difference in entropy of the products and reactants. $(ΔS°rxn)$ can be calculated by the following equation.

$ΔS°rxn = ∑m S°Products- ∑n S°reactants$

Where,

$S°reactants$ is the standard entropy of the reactants

$S°Products$ is the standard entropy of the products

Standard entropy change in a reaction and entropy change in the system are same.

Free energy change is the term that is used to explain the total energy content in a thermodynamic system that can be converted into work. The free energy is represented by the letter G. All spontaneous process is associated with the decrease of free energy in the system. The equation given below helps us to calculate the change in free energy in a system.

$ΔGo = ΔΗo- TΔSo$

Where,

$ΔΗo$ is the change in enthalpy of the system

$ΔGo$ is the standard change in free energy of the system

$T$ is the absolute value of the temperature

(b)

Interpretation Introduction

Interpretation:

The given reaction is become a spontaneous at $1000 oC$ and standard $ΔGo$ state of this process has to determined.

Concept introduction:

Any natural process or a chemical reaction taking place in a laboratory can be classified into two categories, spontaneous or nonspontaneous. Spontaneous process occurs by itself, without the influence of external energy. In spontaneous process the free energy of the system decreases and entropy of the system increases. Nonspontaneous process requires an external influence for initiation. In nonspontaneous process the free energy of the system increases but entropy of the system decreases.

(c)

Interpretation Introduction

Interpretation:

$ΔG$ at $50%$ conversion has to be determined where $50%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

(d)

Interpretation Introduction

Interpretation:

$ΔG$ at $90%$ conversion has to be determined where $90%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ .

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

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Answer 2

Question

Chapter 20, Problem 20.111P

(a)

Interpretation Introduction

Interpretation:

For the steam forming and water-gas shift reaction, the $ΔGo and ΔHo$ values have to be calculated at $1000 oC$ , using the equilibrium free energy and enthalpy values.

Concept introduction:

Enthalpy is the amount energy absorbed or released in a process.

The enthalpy change in a system $(ΔΗsys)$ can be calculated by the following equation.

$ΔHrxn = ∑ΔH°produdcts-∑ΔH°reactants$

Where,

$ΔHfo(reactants)$ is the standard enthalpy of the reactants

$ΔHfo(produdcts)$ is the standard enthalpy of the products

Entropy is the measure of randomness in the system. Standard entropy change in a reaction is the difference in entropy of the products and reactants. $(ΔS°rxn)$ can be calculated by the following equation.

$ΔS°rxn = ∑m S°Products- ∑n S°reactants$

Where,

$S°reactants$ is the standard entropy of the reactants

$S°Products$ is the standard entropy of the products

Standard entropy change in a reaction and entropy change in the system are same.

Free energy change is the term that is used to explain the total energy content in a thermodynamic system that can be converted into work. The free energy is represented by the letter G. All spontaneous process is associated with the decrease of free energy in the system. The equation given below helps us to calculate the change in free energy in a system.

$ΔGo = ΔΗo- TΔSo$

Where,

$ΔΗo$ is the change in enthalpy of the system

$ΔGo$ is the standard change in free energy of the system

$T$ is the absolute value of the temperature

(b)

Interpretation Introduction

Interpretation:

The given reaction is become a spontaneous at $1000 oC$ and standard $ΔGo$ state of this process has to determined.

Concept introduction:

Any natural process or a chemical reaction taking place in a laboratory can be classified into two categories, spontaneous or nonspontaneous. Spontaneous process occurs by itself, without the influence of external energy. In spontaneous process the free energy of the system decreases and entropy of the system increases. Nonspontaneous process requires an external influence for initiation. In nonspontaneous process the free energy of the system increases but entropy of the system decreases.

(c)

Interpretation Introduction

Interpretation:

$ΔG$ at $50%$ conversion has to be determined where $50%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

(d)

Interpretation Introduction

Interpretation:

$ΔG$ at $90%$ conversion has to be determined where $90%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ .

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

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Answer 3

Question

Chapter 20, Problem 20.111P

(a)

Interpretation Introduction

Interpretation:

For the steam forming and water-gas shift reaction, the $ΔGo and ΔHo$ values have to be calculated at $1000 oC$ , using the equilibrium free energy and enthalpy values.

Concept introduction:

Enthalpy is the amount energy absorbed or released in a process.

The enthalpy change in a system $(ΔΗsys)$ can be calculated by the following equation.

$ΔHrxn = ∑ΔH°produdcts-∑ΔH°reactants$

Where,

$ΔHfo(reactants)$ is the standard enthalpy of the reactants

$ΔHfo(produdcts)$ is the standard enthalpy of the products

Entropy is the measure of randomness in the system. Standard entropy change in a reaction is the difference in entropy of the products and reactants. $(ΔS°rxn)$ can be calculated by the following equation.

$ΔS°rxn = ∑m S°Products- ∑n S°reactants$

Where,

$S°reactants$ is the standard entropy of the reactants

$S°Products$ is the standard entropy of the products

Standard entropy change in a reaction and entropy change in the system are same.

Free energy change is the term that is used to explain the total energy content in a thermodynamic system that can be converted into work. The free energy is represented by the letter G. All spontaneous process is associated with the decrease of free energy in the system. The equation given below helps us to calculate the change in free energy in a system.

$ΔGo = ΔΗo- TΔSo$

Where,

$ΔΗo$ is the change in enthalpy of the system

$ΔGo$ is the standard change in free energy of the system

$T$ is the absolute value of the temperature

(b)

Interpretation Introduction

Interpretation:

The given reaction is become a spontaneous at $1000 oC$ and standard $ΔGo$ state of this process has to determined.

Concept introduction:

Any natural process or a chemical reaction taking place in a laboratory can be classified into two categories, spontaneous or nonspontaneous. Spontaneous process occurs by itself, without the influence of external energy. In spontaneous process the free energy of the system decreases and entropy of the system increases. Nonspontaneous process requires an external influence for initiation. In nonspontaneous process the free energy of the system increases but entropy of the system decreases.

(c)

Interpretation Introduction

Interpretation:

$ΔG$ at $50%$ conversion has to be determined where $50%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

(d)

Interpretation Introduction

Interpretation:

$ΔG$ at $90%$ conversion has to be determined where $90%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ .

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 20, Problem 20.111P

(a)

Interpretation Introduction

Interpretation:

For the steam forming and water-gas shift reaction, the $ΔGo and ΔHo$ values have to be calculated at $1000 oC$ , using the equilibrium free energy and enthalpy values.

Concept introduction:

Enthalpy is the amount energy absorbed or released in a process.

The enthalpy change in a system $(ΔΗsys)$ can be calculated by the following equation.

$ΔHrxn = ∑ΔH°produdcts-∑ΔH°reactants$

Where,

$ΔHfo(reactants)$ is the standard enthalpy of the reactants

$ΔHfo(produdcts)$ is the standard enthalpy of the products

Entropy is the measure of randomness in the system. Standard entropy change in a reaction is the difference in entropy of the products and reactants. $(ΔS°rxn)$ can be calculated by the following equation.

$ΔS°rxn = ∑m S°Products- ∑n S°reactants$

Where,

$S°reactants$ is the standard entropy of the reactants

$S°Products$ is the standard entropy of the products

Standard entropy change in a reaction and entropy change in the system are same.

Free energy change is the term that is used to explain the total energy content in a thermodynamic system that can be converted into work. The free energy is represented by the letter G. All spontaneous process is associated with the decrease of free energy in the system. The equation given below helps us to calculate the change in free energy in a system.

$ΔGo = ΔΗo- TΔSo$

Where,

$ΔΗo$ is the change in enthalpy of the system

$ΔGo$ is the standard change in free energy of the system

$T$ is the absolute value of the temperature

(b)

Interpretation Introduction

Interpretation:

The given reaction is become a spontaneous at $1000 oC$ and standard $ΔGo$ state of this process has to determined.

Concept introduction:

Any natural process or a chemical reaction taking place in a laboratory can be classified into two categories, spontaneous or nonspontaneous. Spontaneous process occurs by itself, without the influence of external energy. In spontaneous process the free energy of the system decreases and entropy of the system increases. Nonspontaneous process requires an external influence for initiation. In nonspontaneous process the free energy of the system increases but entropy of the system decreases.

(c)

Interpretation Introduction

Interpretation:

$ΔG$ at $50%$ conversion has to be determined where $50%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

(d)

Interpretation Introduction

Interpretation:

$ΔG$ at $90%$ conversion has to be determined where $90%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ .

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

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Check out a sample textbook solution

See solution

Answer 5

Chapter 20, Problem 20.111P

(a)

Interpretation Introduction

Interpretation:

For the steam forming and water-gas shift reaction, the $ΔGo and ΔHo$ values have to be calculated at $1000 oC$ , using the equilibrium free energy and enthalpy values.

Concept introduction:

Enthalpy is the amount energy absorbed or released in a process.

The enthalpy change in a system $(ΔΗsys)$ can be calculated by the following equation.

$ΔHrxn = ∑ΔH°produdcts-∑ΔH°reactants$

Where,

$ΔHfo(reactants)$ is the standard enthalpy of the reactants

$ΔHfo(produdcts)$ is the standard enthalpy of the products

Entropy is the measure of randomness in the system. Standard entropy change in a reaction is the difference in entropy of the products and reactants. $(ΔS°rxn)$ can be calculated by the following equation.

$ΔS°rxn = ∑m S°Products- ∑n S°reactants$

Where,

$S°reactants$ is the standard entropy of the reactants

$S°Products$ is the standard entropy of the products

Standard entropy change in a reaction and entropy change in the system are same.

Free energy change is the term that is used to explain the total energy content in a thermodynamic system that can be converted into work. The free energy is represented by the letter G. All spontaneous process is associated with the decrease of free energy in the system. The equation given below helps us to calculate the change in free energy in a system.

$ΔGo = ΔΗo- TΔSo$

Where,

$ΔΗo$ is the change in enthalpy of the system

$ΔGo$ is the standard change in free energy of the system

$T$ is the absolute value of the temperature

(b)

Interpretation Introduction

Interpretation:

The given reaction is become a spontaneous at $1000 oC$ and standard $ΔGo$ state of this process has to determined.

Concept introduction:

Any natural process or a chemical reaction taking place in a laboratory can be classified into two categories, spontaneous or nonspontaneous. Spontaneous process occurs by itself, without the influence of external energy. In spontaneous process the free energy of the system decreases and entropy of the system increases. Nonspontaneous process requires an external influence for initiation. In nonspontaneous process the free energy of the system increases but entropy of the system decreases.

(c)

Interpretation Introduction

Interpretation:

$ΔG$ at $50%$ conversion has to be determined where $50%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

(d)

Interpretation Introduction

Interpretation:

$ΔG$ at $90%$ conversion has to be determined where $90%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ .

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

Answer 6

Chapter 20, Problem 20.111P

(a)

Interpretation Introduction

Interpretation:

For the steam forming and water-gas shift reaction, the $ΔGo and ΔHo$ values have to be calculated at $1000 oC$ , using the equilibrium free energy and enthalpy values.

Concept introduction:

Enthalpy is the amount energy absorbed or released in a process.

The enthalpy change in a system $(ΔΗsys)$ can be calculated by the following equation.

$ΔHrxn = ∑ΔH°produdcts-∑ΔH°reactants$

Where,

$ΔHfo(reactants)$ is the standard enthalpy of the reactants

$ΔHfo(produdcts)$ is the standard enthalpy of the products

Entropy is the measure of randomness in the system. Standard entropy change in a reaction is the difference in entropy of the products and reactants. $(ΔS°rxn)$ can be calculated by the following equation.

$ΔS°rxn = ∑m S°Products- ∑n S°reactants$

Where,

$S°reactants$ is the standard entropy of the reactants

$S°Products$ is the standard entropy of the products

Standard entropy change in a reaction and entropy change in the system are same.

Free energy change is the term that is used to explain the total energy content in a thermodynamic system that can be converted into work. The free energy is represented by the letter G. All spontaneous process is associated with the decrease of free energy in the system. The equation given below helps us to calculate the change in free energy in a system.

$ΔGo = ΔΗo- TΔSo$

Where,

$ΔΗo$ is the change in enthalpy of the system

$ΔGo$ is the standard change in free energy of the system

$T$ is the absolute value of the temperature

Answer 7

Chapter 20, Problem 20.111P

(a)

Interpretation Introduction

Interpretation:

For the steam forming and water-gas shift reaction, the $ΔGo and ΔHo$ values have to be calculated at $1000 oC$ , using the equilibrium free energy and enthalpy values.

Concept introduction:

Enthalpy is the amount energy absorbed or released in a process.

The enthalpy change in a system $(ΔΗsys)$ can be calculated by the following equation.

$ΔHrxn = ∑ΔH°produdcts-∑ΔH°reactants$

Where,

$ΔHfo(reactants)$ is the standard enthalpy of the reactants

$ΔHfo(produdcts)$ is the standard enthalpy of the products

Entropy is the measure of randomness in the system. Standard entropy change in a reaction is the difference in entropy of the products and reactants. $(ΔS°rxn)$ can be calculated by the following equation.

$ΔS°rxn = ∑m S°Products- ∑n S°reactants$

Where,

$S°reactants$ is the standard entropy of the reactants

$S°Products$ is the standard entropy of the products

Standard entropy change in a reaction and entropy change in the system are same.

Free energy change is the term that is used to explain the total energy content in a thermodynamic system that can be converted into work. The free energy is represented by the letter G. All spontaneous process is associated with the decrease of free energy in the system. The equation given below helps us to calculate the change in free energy in a system.

$ΔGo = ΔΗo- TΔSo$

Where,

$ΔΗo$ is the change in enthalpy of the system

$ΔGo$ is the standard change in free energy of the system

$T$ is the absolute value of the temperature

Answer 8

(b)

Interpretation Introduction

Interpretation:

The given reaction is become a spontaneous at $1000 oC$ and standard $ΔGo$ state of this process has to determined.

Concept introduction:

Any natural process or a chemical reaction taking place in a laboratory can be classified into two categories, spontaneous or nonspontaneous. Spontaneous process occurs by itself, without the influence of external energy. In spontaneous process the free energy of the system decreases and entropy of the system increases. Nonspontaneous process requires an external influence for initiation. In nonspontaneous process the free energy of the system increases but entropy of the system decreases.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The given reaction is become a spontaneous at $1000 oC$ and standard $ΔGo$ state of this process has to determined.

Concept introduction:

Any natural process or a chemical reaction taking place in a laboratory can be classified into two categories, spontaneous or nonspontaneous. Spontaneous process occurs by itself, without the influence of external energy. In spontaneous process the free energy of the system decreases and entropy of the system increases. Nonspontaneous process requires an external influence for initiation. In nonspontaneous process the free energy of the system increases but entropy of the system decreases.

Answer 10

(c)

Interpretation Introduction

Interpretation:

$ΔG$ at $50%$ conversion has to be determined where $50%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

Answer 11

(c)

Interpretation Introduction

Interpretation:

$ΔG$ at $50%$ conversion has to be determined where $50%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ ,

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

Answer 12

(d)

Interpretation Introduction

Interpretation:

$ΔG$ at $90%$ conversion has to be determined where $90%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ .

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

Answer 13

(d)

Interpretation Introduction

Interpretation:

$ΔG$ at $90%$ conversion has to be determined where $90%$ of starting material is reacted.

Concept introduction:

Reaction quotient $(Q)$ : Reaction quotient and equilibrium constant has same expression. Reaction quotient is also the ratio between the concentrations of the reactant to product, but these concentrations are not necessarily the equilibrium concentrations.

$Q=[Product][Reactant]$

The reaction quotient $(Q)$ is helpful in predicting the direction of the reaction.

When $Q > Kc$ , the reaction proceeds towards left to increase the concentration of the reactants.

When $Q < Kc$ , the reaction proceeds towards right to increase the concentration of the products.

When $Q = Kc$ , the reaction is at equilibrium.

Free energy change $ΔG$ : change in the free energy takes place while reactants convert to product where both are in standard state. It depends on the equilibrium constant $K$ .

$ΔG = ΔGo+ RT ln (K)ΔGo = ΔHo − TΔSo$

Where,

$T$ is the temperature

$ΔG$ is the free energy

$ΔGo$ is standard free energy.

Answer 14

Expert Solution & Answer

Answer 15

Expert Solution & Answer

Answer 16

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Answer 17

Ch. 20.1 - Prob. 20.1AFP Ch. 20.1 - Prob. 20.1BFP Ch. 20.2 - Prob. 20.2AFP Ch. 20.2 - Prob. 20.2BFP Ch. 20.2 - Prob. 20.3AFP Ch. 20.2 - Prob. 20.3BFP Ch. 20.3 - Prob. 20.4AFP Ch. 20.3 - Prob. 20.4BFP Ch. 20.3 - Prob. 20.5AFP Ch. 20.3 - Prob. 20.5BFP

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