Chapter U6.4, Problem 3E

(a)

Interpretation Introduction

Interpretation:

The equilibrium constant for the given reaction should be predicted.

  $\text{2CO}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)\rightleftharpoons 2{\text{CO}}_{\text{2}}\left(g\right)$

Concept Introduction:

The equilibrium constant can be written as the ratio of concentration of products to the concentration of reactants raised to some power of their stoichiometric coefficient. It is represented by K_eq or K_c.

The concentration of species only present in aqueous solution and gaseous is mentioned in writing expression for equilibrium constant.

When the gaseous species are present in a chemical reaction then the equilibrium constant is represented in terms of K_p.

Answer to Problem 3E

The equilibrium constant for the given reaction is represented as follows:

  ${\text{K}}_p=\frac{{\left[{\text{CO}}_{\text{2}}\right]}^2}{{\left[\text{CO}\right]}^2\left[{\text{O}}_{\text{2}}\right]}$

Explanation of Solution

The given reaction is represented as follows:

  $\text{2CO}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)\rightleftharpoons 2{\text{CO}}_{\text{2}}\left(g\right)$

Thus, the equilibrium constant for the above reaction is represented as follows:

  ${\text{K}}_p=\frac{{\left[{\text{CO}}_{\text{2}}\right]}^2}{{\left[\text{CO}\right]}^2\left[{\text{O}}_{\text{2}}\right]}$

(b)

Interpretation Introduction

Interpretation:

The equilibrium constant for the given reaction should be predicted.

  ${\text{N}}_{\text{2}}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)\rightleftharpoons {\text{2NH}}_{\text{3}}\left(g\right)$

Concept Introduction:

The equilibrium constant can be written as the ratio of concentration of products to the concentration of reactants raised to some power of their stoichiometric coefficient. It is represented by K_eq or K_c.

The concentration of species only present in aqueous solution and gaseous is mentioned in writing expression for equilibrium constant.

When the gaseous species are present in a chemical reaction then the equilibrium constant is represented in terms of K_p.

Answer to Problem 3E

The equilibrium constant for the given reaction is represented as follows:

  ${\text{K}}_p=\frac{{\left[{\text{NH}}_{\text{3}}\right]}^2}{\left[{\text{N}}_{\text{2}}\right]{\left[{\text{H}}_{\text{2}}\right]}^3}$

Explanation of Solution

The given reaction is represented as follows:

  ${\text{N}}_{\text{2}}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)\rightleftharpoons {\text{2NH}}_{\text{3}}\left(g\right)$

Thus, the equilibrium constant for the above reaction is represented as follows:

  ${\text{K}}_p=\frac{{\left[{\text{NH}}_{\text{3}}\right]}^2}{\left[{\text{N}}_{\text{2}}\right]{\left[{\text{H}}_{\text{2}}\right]}^3}$

(c)

Interpretation Introduction

Interpretation:

The equilibrium constant for the given reaction should be predicted.

  ${\text{H}}_{\text{2}}\left(g\right)+{\text{I}}_2\left(g\right)\rightleftharpoons 2\text{HI}\left(g\right)$

Concept Introduction:

The equilibrium constant can be written as the ratio of concentration of products to the concentration of reactants raised to some power of their stoichiometric coefficient. It is represented by K_eq or K_c.

The concentration of species only present in aqueous solution and gaseous is mentioned in writing expression for equilibrium constant.

When the gaseous species are present in a chemical reaction then the equilibrium constant is represented in terms of K_p.

Answer to Problem 3E

The equilibrium constant for the given reaction is represented as follows:

  ${\text{K}}_p=\frac{{\left[\text{HI}\right]}^2}{\left[{\text{H}}_{\text{2}}\right]\left[{\text{I}}_2\right]}$

Explanation of Solution

The given reaction is represented as follows:

  ${\text{H}}_{\text{2}}\left(g\right)+{\text{I}}_2\left(g\right)\rightleftharpoons 2\text{HI}\left(g\right)$

Thus, the equilibrium constant for the above reaction is represented as follows:

  ${\text{K}}_p=\frac{{\left[\text{HI}\right]}^2}{\left[{\text{H}}_{\text{2}}\right]\left[{\text{I}}_2\right]}$