Chapter 8, Problem 8.58E

Interpretation Introduction

(a)

Interpretation:

The direction of the equilibrium shift in the given equilibrium is to be predicted.

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 8.58E

The shift in the equilibrium will be towards the right direction.

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.

${\text{N}}_2\left(\text{g}\right)+3{\text{H}}_{\text{2}}\left(\text{g}\right)\rightleftarrows 2{\text{NH}}_3\left(\text{g}\right)$

It is considered that when some amount of ${\text{N}}_{\text{2}}$ is added, the concentration of ${\text{N}}_{\text{2}}$ on the left hand side increases. Hence, according to the Le Chȃtelier’s principle, the equilibrium will shift towards the right direction to compensate the increased amount of ${\text{N}}_{\text{2}}$.

Conclusion

The shift in the equilibrium will be towards the right direction.

Interpretation Introduction

(b)

Interpretation:

The direction of the equilibrium shift in the given equilibrium is to be predicted.

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 8.58E

The shift in the equilibrium will be towards the left direction.

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.

${\text{N}}_2\left(\text{g}\right)+3{\text{H}}_{\text{2}}\left(\text{g}\right)\rightleftarrows 2{\text{NH}}_3\left(\text{g}\right)$

The given reaction is exothermic reaction. The reaction is at equilibrium when the heat is given out from the system. It is considered that the temperature of the system increases. Thus, the temperature of the system on the right hand side increases. Hence, according to the Le Chȃtelier’s principle, the equilibrium will shift towards left direction to compensate the increase in temperature.

Conclusion

The shift in the equilibrium will be towards the left direction.

Interpretation Introduction

(c)

Interpretation:

The direction of the equilibrium shift in the given equilibrium is to be predicted.

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 8.58E

The shift in the equilibrium will be towards the right direction.

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.

${\text{N}}_2\left(\text{g}\right)+3{\text{H}}_{\text{2}}\left(\text{g}\right)\rightleftarrows 2{\text{NH}}_3\left(\text{g}\right)$

It is considered that when some amount of ${\text{NH}}_3$ is removed, the concentration of ${\text{NH}}_3$ on the right hand side decreases. Hence, according to the Le Chȃtelier’s principle, the equilibrium will shift towards the right direction to compensate the decreased amount of ${\text{NH}}_3$.

Conclusion

The shift in the equilibrium will be towards the right direction.

Interpretation Introduction

(d)

Interpretation:

The direction of the equilibrium shift in the given equilibrium is to be predicted.

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 8.58E

The shift in the equilibrium will be towards the left direction.

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.

${\text{N}}_2\left(\text{g}\right)+3{\text{H}}_{\text{2}}\left(\text{g}\right)\rightleftarrows 2{\text{NH}}_3\left(\text{g}\right)$

It is considered that when some amount of ${\text{H}}_{\text{2}}$ is removed, the concentration of ${\text{H}}_{\text{2}}$ on the left hand side decreases. Hence, according to the Le Chȃtelier’s principle, the equilibrium will shift towards the left direction to compensate the decreased amount of ${\text{H}}_{\text{2}}$.

Conclusion

The shift in the equilibrium will be towards the left direction.

Interpretation Introduction

(e)

Interpretation:

The direction of the equilibrium shift in the given equilibrium is to be predicted.

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 8.58E

The equilibrium does not shift on addition of a catalyst.

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.

${\text{N}}_2\left(\text{g}\right)+3{\text{H}}_{\text{2}}\left(\text{g}\right)\rightleftarrows 2{\text{NH}}_3\left(\text{g}\right)$

It is considered that when a catalyst is added, it will only increase the rate of reaction. Hence, there will be no effect on the equilibrium.

Conclusion

The equilibrium does not shift on addition of a catalyst.

Interpretation Introduction

(f)

Interpretation:

The direction of the equilibrium shift in the given equilibrium is to be predicted.

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 8.58E

The shift in the equilibrium will be towards the left direction.

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.

${\text{N}}_2\left(\text{g}\right)+3{\text{H}}_{\text{2}}\left(\text{g}\right)\rightleftarrows 2{\text{NH}}_3\left(\text{g}\right)$

The given reaction is exothermic reaction. The reaction is at equilibrium when the heat is given out from the system. It is considered that the temperature of the system increases and some amount of ${\text{H}}_{\text{2}}$ is removed. Thus, the concentration of ${\text{H}}_{\text{2}}$ on the left hand side decreases. Hence, according to the Le Chȃtelier’s principle, the equilibrium will shift towards the left direction to compensate the decreased amount of ${\text{H}}_{\text{2}}$ and increased temperature.

Conclusion

The shift in the equilibrium will be towards the left direction.