Chapter 8, Problem 8.40E

Interpretation Introduction

(a)

Interpretation:

The equilibrium expression for the given gaseous reaction is to be stated.

Concept Introduction:

The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their stoichiometric coefficients. A general equilibrium reaction is represented as,$a\text{A}+b\text{B}\rightleftharpoons c\text{C}+d\text{D}$

The equilibrium constant for the above chemical reaction is expressed as,$K=\frac{{\left[\text{C}\right]}^c{\left[\text{D}\right]}^d}{{\left[\text{A}\right]}^a{\left[\text{B}\right]}^b}$

Where,

• $\left[\text{A}\right]$ represents the equilibrium concentration of reactant $\text{A}$.

• $\left[\text{B}\right]$ represents the equilibrium concentration of reactant $\text{B}$.

• $\left[\text{C}\right]$ represents the equilibrium concentration of product $\text{C}$.

• $\left[\text{D}\right]$ represents the equilibrium concentration of product $\text{D}$.

• $a$ represents the stoichiometric coefficient of reactant $\text{A}$.

• $b$ represents the stoichiometric coefficient of reactant $\text{B}$.

• $c$ represents the stoichiometric coefficient of product $\text{C}$.

• $d$ represents the stoichiometric coefficient of product $\text{D}$.

Answer to Problem 8.40E

The equilibrium constant for the given gaseous reaction is expressed as,$K=\frac{{\left[{\text{CO}}_2\right]}^2}{{\left[\text{CO}\right]}^2\left[{\text{O}}_2\right]}$

Explanation of Solution

The given gaseous reaction is represented as,$2\text{CO}+{\text{O}}_2\rightleftarrows 2{\text{CO}}_2$

The concentration of the product ${\text{CO}}_2$ will be in the numerator and is raised to the power $2$. The concentration of reactant $\text{CO}$ and ${\text{O}}_2$ will be in the denominator. The concentration of reactant $\text{CO}$ is raised to the power $2$ and ${\text{O}}_2$ is raised to the power $1$.

Therefore, the equilibrium constant for the above gaseous reaction is expressed as,$K=\frac{{\left[{\text{CO}}_2\right]}^2}{{\left[\text{CO}\right]}^2\left[{\text{O}}_2\right]}$

Conclusion

The equilibrium constant for the given gaseous reaction is expressed as,$K=\frac{{\left[{\text{CO}}_2\right]}^2}{{\left[\text{CO}\right]}^2\left[{\text{O}}_2\right]}$

Interpretation Introduction

(b)

Interpretation:

The equilibrium expression for the given gaseous reaction is to be stated.

Concept Introduction:

The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their stoichiometric coefficients. A general equilibrium reaction is represented as,$a\text{A}+b\text{B}\rightleftharpoons c\text{C}+d\text{D}$

The equilibrium constant for the above chemical reaction is expressed as,$K=\frac{{\left[\text{C}\right]}^c{\left[\text{D}\right]}^d}{{\left[\text{A}\right]}^a{\left[\text{B}\right]}^b}$

Where,

• $\left[\text{A}\right]$ represents the equilibrium concentration of reactant $\text{A}$.

• $\left[\text{B}\right]$ represents the equilibrium concentration of reactant $\text{B}$.

• $\left[\text{C}\right]$ represents the equilibrium concentration of product $\text{C}$.

• $\left[\text{D}\right]$ represents the equilibrium concentration of product $\text{D}$.

• $a$ represents the stoichiometric coefficient of reactant $\text{A}$.

• $b$ represents the stoichiometric coefficient of reactant $\text{B}$.

• $c$ represents the stoichiometric coefficient of product $\text{C}$.

• $d$ represents the stoichiometric coefficient of product $\text{D}$.

Answer to Problem 8.40E

The equilibrium constant for the given gaseous reaction is expressed as,$K=\frac{{\left[{\text{NO}}_2\right]}^2}{\left[{\text{N}}_2{\text{O}}_4\right]}$

Explanation of Solution

The given gaseous reaction is represented as,${\text{N}}_2{\text{O}}_4\rightleftarrows 2{\text{NO}}_2$

The concentration of the product ${\text{NO}}_2$ will be in the numerator and is raised to the power $2$. The concentration of reactant ${\text{N}}_2{\text{O}}_4$ will be in denominator and is raised to the power $1$.

Therefore, the equilibrium constant for the above gaseous reaction is expressed as,$K=\frac{{\left[{\text{NO}}_2\right]}^2}{\left[{\text{N}}_2{\text{O}}_4\right]}$

Conclusion

The equilibrium constant for the given gaseous reaction is expressed as,$K=\frac{{\left[{\text{NO}}_2\right]}^2}{\left[{\text{N}}_2{\text{O}}_4\right]}$

Interpretation Introduction

(c)

Interpretation:

The equilibrium expression for the given gaseous reaction is to be stated.

Concept Introduction:

The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their stoichiometric coefficients. A general equilibrium reaction is represented as,$a\text{A}+b\text{B}\rightleftharpoons c\text{C}+d\text{D}$

The equilibrium constant for the above chemical reaction is expressed as,$K=\frac{{\left[\text{C}\right]}^c{\left[\text{D}\right]}^d}{{\left[\text{A}\right]}^a{\left[\text{B}\right]}^b}$

Where,

• $\left[\text{A}\right]$ represents the equilibrium concentration of reactant $\text{A}$.

• $\left[\text{B}\right]$ represents the equilibrium concentration of reactant $\text{B}$.

• $\left[\text{C}\right]$ represents the equilibrium concentration of product $\text{C}$.

• $\left[\text{D}\right]$ represents the equilibrium concentration of product $\text{D}$.

• $a$ represents the stoichiometric coefficient of reactant $\text{A}$.

• $b$ represents the stoichiometric coefficient of reactant $\text{B}$.

• $c$ represents the stoichiometric coefficient of product $\text{C}$.

• $d$ represents the stoichiometric coefficient of product $\text{D}$.

Answer to Problem 8.40E

The equilibrium constant for the given gaseous reaction is expressed as,$K=\frac{{\left[{\text{CO}}_2\right]}^4{\left[{\text{H}}_2\text{O}\right]}^6}{{\left[{\text{C}}_2{\text{H}}_6\right]}^2{\left[{\text{O}}_2\right]}^7}$

Explanation of Solution

The given gaseous reaction is represented as,$2{\text{C}}_2{\text{H}}_6+7{\text{O}}_2\rightleftarrows 4{\text{CO}}_2+6{\text{H}}_2\text{O}$

The concentration of the product ${\text{CO}}_2$ and ${\text{H}}_2\text{O}$ will be in the numerator. The concentration of the product ${\text{CO}}_2$ is raised to the power $4$ and ${\text{H}}_2\text{O}$ is raised to the power $6$. The concentration of reactant ${\text{C}}_2{\text{H}}_6$ and ${\text{O}}_2$ will be in the denominator. The concentration of reactant ${\text{C}}_2{\text{H}}_6$ is raised to the power $2$ and ${\text{O}}_2$ is raised to the power $7$.

Therefore, the equilibrium constant for the above gaseous reaction is expressed as,$K=\frac{{\left[{\text{CO}}_2\right]}^4{\left[{\text{H}}_2\text{O}\right]}^6}{{\left[{\text{C}}_2{\text{H}}_6\right]}^2{\left[{\text{O}}_2\right]}^7}$

Conclusion

The equilibrium constant for the given gaseous reaction is expressed as,$K=\frac{{\left[{\text{CO}}_2\right]}^4{\left[{\text{H}}_2\text{O}\right]}^6}{{\left[{\text{C}}_2{\text{H}}_6\right]}^2{\left[{\text{O}}_2\right]}^7}$

Interpretation Introduction

(d)

Interpretation:

The equilibrium expression for the given gaseous reaction is to be stated.

Concept Introduction:

The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their stoichiometric coefficients. A general equilibrium reaction is represented as,$a\text{A}+b\text{B}\rightleftharpoons c\text{C}+d\text{D}$

The equilibrium constant for the above chemical reaction is expressed as,$K=\frac{{\left[\text{C}\right]}^c{\left[\text{D}\right]}^d}{{\left[\text{A}\right]}^a{\left[\text{B}\right]}^b}$

Where,

• $\left[\text{A}\right]$ represents the equilibrium concentration of reactant $\text{A}$.

• $\left[\text{B}\right]$ represents the equilibrium concentration of reactant $\text{B}$.

• $\left[\text{C}\right]$ represents the equilibrium concentration of product $\text{C}$.

• $\left[\text{D}\right]$ represents the equilibrium concentration of product $\text{D}$.

• $a$ represents the stoichiometric coefficient of reactant $\text{A}$.

• $b$ represents the stoichiometric coefficient of reactant $\text{B}$.

• $c$ represents the stoichiometric coefficient of product $\text{C}$.

• $d$ represents the stoichiometric coefficient of product $\text{D}$.

Answer to Problem 8.40E

The equilibrium constant for the given gaseous reaction is expressed as,$K=\frac{{\left[\text{NO}\right]}^2\left[{\text{Cl}}_2\right]}{{\left[\text{NOCl}\right]}^2}$

Explanation of Solution

The given gaseous reaction is represented as,$\text{2NOCl}\rightleftarrows 2\text{NO}+{\text{Cl}}_2$

The concentration of the product $\text{NO}$ and ${\text{Cl}}_2$ will be in the numerator. The concentration of the product $\text{NO}$ is raised to the power $2$ and ${\text{Cl}}_2$ is raised to the power $1$. The concentration of reactant $\text{NOCl}$ will be in denominator and is raised to the power $2$.

Therefore, the equilibrium constant for the above gaseous reaction is expressed as,$K=\frac{{\left[\text{NO}\right]}^2\left[{\text{Cl}}_2\right]}{{\left[\text{NOCl}\right]}^2}$

Conclusion

The equilibrium constant for the given gaseous reaction is expressed as,$K=\frac{{\left[\text{NO}\right]}^2\left[{\text{Cl}}_2\right]}{{\left[\text{NOCl}\right]}^2}$

Interpretation Introduction

(e)

Interpretation:

The equilibrium expression for the given gaseous reaction is to be stated.

Concept Introduction:

The equilibrium constant of a reaction is expressed as the ratio of concentration of products and reactants each raised to the power of their stoichiometric coefficients. A general equilibrium reaction is represented as,$a\text{A}+b\text{B}\rightleftharpoons c\text{C}+d\text{D}$

The equilibrium constant for the above chemical reaction is expressed as,$K=\frac{{\left[\text{C}\right]}^c{\left[\text{D}\right]}^d}{{\left[\text{A}\right]}^a{\left[\text{B}\right]}^b}$

Where,

• $\left[\text{A}\right]$ represents the equilibrium concentration of reactant $\text{A}$.

• $\left[\text{B}\right]$ represents the equilibrium concentration of reactant $\text{B}$.

• $\left[\text{C}\right]$ represents the equilibrium concentration of product $\text{C}$.

• $\left[\text{D}\right]$ represents the equilibrium concentration of product $\text{D}$.

• $a$ represents the stoichiometric coefficient of reactant $\text{A}$.

• $b$ represents the stoichiometric coefficient of reactant $\text{B}$.

• $c$ represents the stoichiometric coefficient of product $\text{C}$.

• $d$ represents the stoichiometric coefficient of product $\text{D}$.

Answer to Problem 8.40E

The equilibrium constant for the given gaseous reaction is expressed as,$K=\frac{{\left[{\text{ClO}}_2\right]}^4\left[{\text{O}}_2\right]}{{\left[{\text{Cl}}_2{\text{O}}_5\right]}^2}$

Explanation of Solution

The given gaseous reaction is represented as,${\text{2Cl}}_2{\text{O}}_5\rightleftarrows {\text{O}}_2+4{\text{ClO}}_2$

The concentration of the product ${\text{O}}_2$ and ${\text{ClO}}_2$ will be in the numerator. The concentration of the product ${\text{O}}_2$ is raised to the power $1$ and ${\text{ClO}}_2$ is raised to the power $4$. The concentration of reactant ${\text{Cl}}_2{\text{O}}_5$ will be in denominator and is raised to the power $2$.

Therefore, the equilibrium constant for the above gaseous reaction is expressed as,$K=\frac{{\left[{\text{ClO}}_2\right]}^4\left[{\text{O}}_2\right]}{{\left[{\text{Cl}}_2{\text{O}}_5\right]}^2}$

Conclusion

The equilibrium constant for the given gaseous reaction is expressed as,$K=\frac{{\left[{\text{ClO}}_2\right]}^4\left[{\text{O}}_2\right]}{{\left[{\text{Cl}}_2{\text{O}}_5\right]}^2}$