Chapter U6, Problem C23.4RE

Interpretation Introduction

(a)

Interpretation:

The equilibrium constant for the given reaction should be predicted.

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 C23.4RE

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:

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

Interpretation Introduction

(b)

Interpretation:

The value of equilibrium constant should be predicted for the given reaction.

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 C23.4RE

The value of equilibrium constant is 12.5.

Explanation of Solution

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

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

Now, plugging the values of concentration of N₂, H₂, and NH₃ in the above expression as follows:

$\begin{array}{c}{\text{K}}_p=\frac{{\left[\text{0}\text{.1}\right]}^2}{\left[\text{0}\text{.1}\right]{\left[\text{0}\text{.2}\right]}^3}\\ =\frac{0.01}{0.0008}\\ {\text{K}}_p=12.5\end{array}$

Thus, the value of equilibrium constant is 12.5.

Interpretation Introduction

(c)

Interpretation:

The direction of the reaction should be predicted.

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 C23.4RE

The reaction is product favored.

Explanation of Solution

According to the equilibrium constant calculated in part b, it is found that the value of equilibrium constant is much much greater than 1that means the concentration of the products is higher thus, the reaction will shift to the right or forward direction.

Therefore, the reaction is product favored.