Chapter 8, Problem 8.54E

Interpretation Introduction

(a)

Interpretation:

The direction of the equilibrium shift and the change that will be observed (color, amount of precipitate, etc.) in the given equilibria when the indicated stress is applied is to be predicted using the Le Chȃtelier’s principle.

Concept introduction:

The equilibrium constant is a parameter which describes the relationship between concentration of the reactants and the products at equilibrium stage. Equilibrium constant of a reaction is expressed by the ratio of concentration of product species raised to the power of their stoichiometric coefficients to the concentration of reactant species raised to the power of their stoichiometric coefficients.

Answer to Problem 8.54E

The shift in the equilibrium will be towards the right direction and dark purple color will be observed due to the formation of copper complex.

Explanation of Solution

According to the Le Chȃtelier’s principle the change in concentration, volume, pressure and temperature affects the equilibrium of the reaction.

The given equilibrium reaction is shown below.

$\begin{array}{l}{\text{Co}}^{2+}\left(\text{aq}\right)+4{\text{NH}}_{\text{3}}\left(\text{aq}\right)\rightleftarrows \text{Cu}{\left({\text{NH}}_{\text{3}}\right)}_4{}^{2-}\left(\text{aq}\right)\\ \text{blue}\text{colorless}\text{dark}\text{purple}\end{array}$

It is considered that when ${\text{NH}}_{\text{3}}$ is added to the equilibrium mixture, the amount of ${\text{NH}}_{\text{3}}$ on the left hand side increases. Hence, according to the Le Chȃtelier’s principle, the equilibrium will shift towards right direction to compensate the increased amount of ${\text{NH}}_{\text{3}}$. Thus, the dark purple color will be observed due to the formation of copper complex.

Conclusion

The shift in the equilibrium will be towards the right direction and dark purple color will be observed due to the formation of copper complex.

Interpretation Introduction

(b)

Interpretation:

The direction of the equilibrium shift and the change that will be observed (color, amount of precipitate, etc.) in the given equilibria when the indicated stress is applied is to be predicted using the Le Chȃtelier’s principle.

Concept introduction:

The equilibrium constant is a parameter which describes the relationship between concentration of the reactants and the products at equilibrium stage. Equilibrium constant of a reaction is expressed by the ratio of concentration of product species raised to the power of their stoichiometric coefficients to the concentration of reactant species raised to the power of their stoichiometric coefficients.

Answer to Problem 8.54E

The shift in the equilibrium will be towards the right direction and white solid will be formed due to the formation of lead chloride.

Explanation of Solution

According to the Le Chȃtelier’s principle the change in concentration, volume, pressure and temperature affects the equilibrium of the reaction.

The given equilibrium reaction is shown below.

$\begin{array}{l}{\text{Pb}}^{2+}\left(\text{aq}\right)+2{\text{Cl}}^{-}\left(\text{aq}\right)\rightleftarrows {\text{PbCl}}_2\left(\text{s}\right)+\text{heat}\\ \text{colorless}\text{colorless}\text{white}\text{solid}\end{array}$

It is considered that whenequilibrium mixture is cooled, the temperature on right hand side decreases. Hence, according to the Le Chȃtelier’s principle, the equilibrium will shift towards right direction to compensate the decrease in temperature. Thus, the white solid would be formed due to the formation of lead chloride.

Conclusion

The shift in the equilibrium will be towards the right direction and white solid will be formed due to the formation of lead chloride.

Interpretation Introduction

(c)

Interpretation:

The direction of the equilibrium shift and the change that will be observed (color, amount of precipitate, etc.) in the given equilibria when the indicated stress is applied is to be predicted using the Le Chȃtelier’s principle.

Concept introduction:

The equilibrium constant is a parameter which describes the relationship between concentration of the reactants and the products at equilibrium stage. Equilibrium constant of a reaction is expressed by the ratio of concentration of product species raised to the power of their stoichiometric coefficients to the concentration of reactant species raised to the power of their stoichiometric coefficients.

Answer to Problem 8.54E

The shift in the equilibrium will be towards the right direction and colorless gas will be liberated due to the formation of ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{I}}_{\text{2}}$.

Explanation of Solution

According to the Le Chȃtelier’s principle the change in concentration, volume, pressure and temperature affects the equilibrium of the reaction.

The given equilibrium reaction is shown below.

$\begin{array}{l}{\text{C}}_{\text{2}}{\text{H}}_{\text{4}}+{\text{I}}_{\text{2}}\rightleftarrows {\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{I}}_{\text{2}}+\text{heat}\\ \text{colorless}\text{gas}\text{violet}\text{gas}\text{colorless}\text{gas}\end{array}$

It is considered that when the some amount of ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{I}}_{\text{2}}$ is removed to the equilibrium mixture, thus the amount of ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{I}}_{\text{2}}$ on the right hand side decreases. Hence, according to the Le Chȃtelier’s principle, the equilibrium will shift towards right direction to compensate the decreased amount of ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{I}}_{\text{2}}$. Thus, colorless gas will be liberated due to the formation of ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{I}}_{\text{2}}$.

Conclusion

The shift in the equilibrium will be towards the right direction and colorless gas will be liberated due to the formation of ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{I}}_{\text{2}}$.

Interpretation Introduction

(d)

Interpretation:

The direction of the equilibrium shift and the change that will be observed (color, amount of precipitate, etc.) in the given equilibria when the indicated stress is applied is to be predicted using the Le Chȃtelier’s principle.

Concept introduction:

The equilibrium constant is a parameter which describes the relationship between concentration of the reactants and the products at equilibrium stage. Equilibrium constant of a reaction is expressed by the ratio of concentration of product species raised to the power of their stoichiometric coefficients to the concentration of reactant species raised to the power of their stoichiometric coefficients.

Answer to Problem 8.54E

The shift in the equilibrium will be towards the right direction and colorless gas will be liberated due to the formation of ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{I}}_{\text{2}}$.

Explanation of Solution

According to the Le Chȃtelier’s principle the change in concentration, volume, pressure and temperature affects the equilibrium of the reaction.

The given equilibrium reaction is shown below.

$\begin{array}{l}{\text{C}}_{\text{2}}{\text{H}}_{\text{4}}+{\text{I}}_{\text{2}}\rightleftarrows {\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{I}}_{\text{2}}+\text{heat}\\ \text{colorless}\text{gas}\text{violet}\text{gas}\text{colorless}\text{gas}\end{array}$

It is considered that whenequilibrium mixture is cooled, thus the temperature on right hand side decreases. Hence, according to the Le Chȃtelier’s principle, the equilibrium will shift towards right direction to compensate the decrease in temperature. Thus, the colorless gas will be liberated due to the formation of ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{I}}_{\text{2}}$.

Conclusion

The shift in the equilibrium will be towards the right direction and colorless gas will be liberated due to the formation of ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}{\text{I}}_{\text{2}}$.

Interpretation Introduction

(e)

Interpretation:

The direction of the equilibrium shift and the change that will be observed (color, amount of precipitate, etc.) in the given equilibria when the indicated stress is applied is to be predicted using the Le Chȃtelier’s principle.

Concept introduction:

The equilibrium constant is a parameter which describes the relationship between concentration of the reactants and the products at equilibrium stage. Equilibrium constant of a reaction is expressed by the ratio of concentration of product species raised to the power of their stoichiometric coefficients to the concentration of reactant species raised to the power of their stoichiometric coefficients.

Answer to Problem 8.54E

There will be no effect of catalyst on the equilibrium. The shift in the equilibrium will be towards the left direction due to the addition of ${\text{NH}}_3$ and brown gas will be liberated due to the formation of nitrogen dioxide.

Explanation of Solution

According to the Le Chȃtelier’s principle the change in concentration, volume, pressure and temperature affects the equilibrium of the reaction.

The given equilibrium reaction is shown below.

$\begin{array}{l}\text{heat}+{\text{4NO}}_{\text{2}}+{\text{6H}}_{\text{2}}\text{O}\rightleftarrows {\text{7O}}_{\text{2}}+4{\text{NH}}_3\\ \text{brown}\text{colorless}\text{colorless}\text{colorless}\\ \text{gas}\text{gas}\text{gas}\text{gas}\end{array}$

It is considered that when catalyst and ${\text{NH}}_3$ is added to the equilibrium mixture, there will be no effect of catalyst on the equilibriumbut the amount of ${\text{NH}}_3$ increases. Hence, according to the Le Chȃtelier’s principle, the equilibrium will shift towards left direction to compensate the increased amount of ${\text{NH}}_3$. Thus, the brown gas will be liberated due to the formation of nitrogen dioxide.

Conclusion

There will be no effect of catalyst on the equilibrium. The shift in the equilibrium will be towards the left direction due to the addition of ${\text{NH}}_3$ and brown gas will be liberated due to the formation of nitrogen dioxide.