Chapter 6, Problem 21PP

(a)

Interpretation Introduction

Interpretation:

It should be determined that whether or not the equilibrium will favour product over reactants under the given condition.

Concept Introduction:

Equilibrium constant: At equilibrium the ratio of products to reactants has a constant value. And it is represented by the letter K.

For a general reaction, $\text{aA}\text{+}\text{bB}\underset{}{\rightleftharpoons }\text{cC}\text{+}\text{dD}$ .

The equilibrium constant $Kc$ = $\frac{{\text{[C]}}^{\text{c}}{\text{[D]}}^{\text{d}}}{{\text{[A]}}^{\text{a}}{\text{[B]}}^{\text{b}}}$ a, b, c and d are the stoichiometric coefficients of reactant and product in the reaction. Concentration value for solid substance is 1.

If the value of $K>1$ then the reaction will be product-favoured which means product predominates at equilibrium.

If the value of $K<1$ then the reaction will be reactant-favoured which means reactant predominates at equilibrium.

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by $\Delta G$. The expression for the free energy change with respect to the $K_{eq}$ is written below,

 $\text{ΔG}={\text{-RTlnK}}_{\text{eq}}$ where, R is the gas constant, T is the temperature in Kelvin.

(b)

Interpretation Introduction

Interpretation:

It should be determined that whether or not the equilibrium will favour product over reactants under the given condition.

Concept Introduction:

Equilibrium constant: At equilibrium the ratio of products to reactants has a constant value. And it is represented by the letter K.

For a general reaction, $\text{aA}\text{+}\text{bB}\rightleftarrows \text{cC}\text{+}\text{dD}$

The equilibrium constant $Kc$ = $\frac{{\text{[C]}}^{\text{c}}{\text{[D]}}^{\text{d}}}{{\text{[A]}}^{\text{a}}{\text{[B]}}^{\text{b}}}$    a, b, c and d are the stoichiometric coefficients of reactant and product in the reaction. Concentration value for solid substance is 1.

If the value of $K>1$ then the reaction will be product-favoured which means product predominates at equilibrium.

If the value of $K<1$ then the reaction will be reactant-favoured which means reactant predominates at equilibrium.

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by $\Delta G$. The expression for the free energy change with respect to the $K_{eq}$ is written below,

 $\text{ΔG}={\text{-RTlnK}}_{\text{eq}}$  where, R is the gas constant, T is the temperature in Kelvin.

(c)

Interpretation Introduction

Interpretation:

It should be determined that whether or not the equilibrium will favour product over reactants under the given condition.

Concept Introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by $\Delta G$. The expression for the free energy change with respect to the $K_{eq}$ is written below,

 $\text{ΔG}={\text{-RTlnK}}_{\text{eq}}$  where, R is the gas constant, T is the temperature in Kelvin.

If $\Delta G<0$ then the reaction is spontanous in forward reaction and so the reaction will favor products.

If $\Delta G>0$ then the reaction is spontanous in backward reaction and so the reaction will favor reactants.

If $\Delta G=0$ then the reaction is at equilibrium.

(d)

Interpretation Introduction

Interpretation:

It should be determined that whether or not the equilibrium will favour product over reactants under the given condition.

Concept Introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by $\Delta G$. The expression for the free energy change as a function of  entropy $\Delta S$ and enthalpy $\Delta H$, is written below,

 $\text{ΔG}=\Delta H-T\Delta S$  where, T is the temperature in Kelvin.

If $\Delta G<0$ then the reaction is spontanous in forward reaction and so the reaction will favor products.

If $\Delta G>0$ then the reaction is spontanous in backward reaction and so the reaction will favor reactants.

If $\Delta G=0$ then the reaction is at equilibrium.

An exothermic process is one that loses heat to the surroundings.

An endothermic reaction is one that gains heat from the surroundings.

(e)

Interpretation Introduction

Interpretation:

It should be determined that whether or not the equilibrium will favour product over reactants under the given condition.

Concept Introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by $\Delta G$. The expression for the free energy change as a function of  entropy $\Delta S$ and enthalpy $\Delta H$, is written below,

 $\text{ΔG}=\Delta H-T\Delta S$  where, T is the temperature in Kelvin.

If $\Delta G<0$ then the reaction is spontanous in forward reaction and so the reaction will favor products.

If $\Delta G>0$ then the reaction is spontanous in backward reaction and so the reaction will favor reactants.

If $\Delta G=0$ then the reaction is at equilibrium.

An exothermic process is one that loses heat to the surroundings.

An endothermic reaction is one that gains heat from the surroundings.