Chapter 15.6, Problem 15.6.2SR

(a)

Interpretation Introduction

Interpretation:

The equilibrium directions should be identified given the gas phase equilibrium reaction with different conditions.

Concept Introduction:

Concept of equilibrium process: The any system at equilibrium subject to change in concentration, temperature, volume or pressure then the system readjusts itself to partly counteract the effect of the applied change and new equilibrium is formed.  This equilibrium explain to simple way, a system equilibrium is distributed the system will adjust itself in such a way that the effect of the change will be reduced.

Le Chatelier's Principle: A change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.  In other words the closed system is an increase in pressure; the equilibrium will shift towards the sides of the reaction with some moles of gas.  The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Homogeneous equilibrium: A homogeneous equilibrium involved has everything present in the same phase and same conditions, for example reactions where everything is a gas, or everything is present in the same solution.

Heterogeneous equilibrium: This equilibrium reaction does not depend on the amounts of pure solid and liquid present, in other words heterogeneous equilibrium, substances are in different phases.

Answer to Problem 15.6.2SR

The equilibrium directions for given the statements of addition, removal and addition of reactants are given below.

$\begin{array}{l}{\text{A}}_{\text{2}}{}_{\text{(g)}}+{\text{B}}_{\text{2}}{}_{(g)}\rightleftharpoons {\text{2AB}}_{\text{(g)}}\text{----------Equilibrium shift to right}\\ [Additionof{\text{A}}_{\text{2}}]\end{array}$

Explanation of Solution

To Identify: Given the equilibrium reactions addition, removal of $\left({\text{A}}_{\text{2}}{\text{and B}}_{\text{2}}\right)$ should be analysed.

First we identify given both reactions the directions should be identified, with respective statements of equilibrium reactions. Further we writing the reaction quotient $\left(\text{Qc}\right)$ expression fallowed.

$\begin{array}{l}{\text{A}}_{\text{2}}\text{(g)}+{\text{B}}_{\text{2}}(g)\rightleftharpoons \text{2AB(g)}\\ \text{Qc=}\frac{{[AB]}^2}{[A_2][B_2]}\end{array}$

Here both components will be appeared in this equation, because these molecules are gases phase.

$\begin{array}{l}{\text{A}}_{\text{2}}{}_{\text{(g)}}+{\text{B}}_{\text{2}}{}_{(g)}\rightleftharpoons {\text{2AB}}_{\text{(g)}}\text{----------Equilibrium shift to right}\\ [Additionof{\text{A}}_{\text{2}}]\end{array}$

Let us consider the reaction process, Le Chatelier's Principle to determine which of the following process will cause the equilibrium shift to the right or left.

The equal mole ratio of reactant (A and B) to produce in two moles of product in gas phase conditions, hence these equilibrium reactions has homogeneous reaction.

Reaction (a): The given reaction if we addition of sufficient amount of reactant $\left({\text{B}}_{\text{2}}\right)$ this process will undergoes for right side, process will be re-established in such a way that $\left(\text{Qc}\right)$ is again to the equilibrium constant, highest mole amount of products has to be formed. Hence the system of equilibrium shifted to the right side to established concentration equilibrium.

(b)

Interpretation Introduction

Interpretation:

The equilibrium directions should be identified given the gas phase equilibrium reaction with different conditions.

Concept Introduction:

Concept of equilibrium process: The any system at equilibrium subject to change in concentration, temperature, volume or pressure then the system readjusts itself to partly counteract the effect of the applied change and new equilibrium is formed.  This equilibrium explain to simple way, a system equilibrium is distributed the system will adjust itself in such a way that the effect of the change will be reduced.

Le Chatelier's Principle: A change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.  In other words the closed system is an increase in pressure; the equilibrium will shift towards the sides of the reaction with some moles of gas.  The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Homogeneous equilibrium: A homogeneous equilibrium involved has everything present in the same phase and same conditions, for example reactions where everything is a gas, or everything is present in the same solution.

Heterogeneous equilibrium: This equilibrium reaction does not depend on the amounts of pure solid and liquid present, in other words heterogeneous equilibrium, substances are in different phases.

Answer to Problem 15.6.2SR

The equilibrium directions for given the statements of addition, removal and addition of reactants are given below.

$\begin{array}{l}{\text{A}}_{\text{2}}{}_{\text{(g)}}+{\text{B}}_{\text{2}}{}_{(g)}\rightleftharpoons {\text{2AB}}_{\text{(g)}}\text{----------Equilibrium shift to left}\\ [Removalof{\text{B}}_{\text{2}}]\end{array}$

Explanation of Solution

To Identify: Given the equilibrium reactions addition, removal of $\left({\text{A}}_{\text{2}}{\text{and B}}_{\text{2}}\right)$ should be analyzed.

First we identify given both reactions the directions should be identified, with respective statements of equilibrium reactions. Further we writing the reaction quotient $\left(\text{Qc}\right)$ expression fallowed.

$\begin{array}{l}{\text{A}}_{\text{2}}\text{(g)}+{\text{B}}_{\text{2}}(g)\rightleftharpoons \text{2AB(g)}\\ \text{Qc=}\frac{{[AB]}^2}{[A_2][B_2]}\end{array}$

Here both components will be appeared in this equation, because these molecules are gases phase.

$\begin{array}{l}{\text{A}}_{\text{2}}{}_{\text{(g)}}+{\text{B}}_{\text{2}}{}_{(g)}\rightleftharpoons {\text{2AB}}_{\text{(g)}}\text{----------Equilibrium shift to left}\\ [Removalof{\text{B}}_{\text{2}}]\end{array}$

Let us consider the reaction process, Le Chatelier's Principle to determine which of the following process will cause the equilibrium shift to the right or left.

The equal mole ratio of reactant (A and B) to produce in two moles of product in gas phase conditions, hence these equilibrium reactions has homogeneous reaction.

Reaction (b): If we removed for another one of reactant molecule $\left({\text{B}}_{\text{2}}\right)$ in this equilibrium process, the total directions will back into left side, because equal moles of reactant molecule only proceeds in product formation. So removed one of reactant molecules it cannot be proceeds in right side.

(c)

Interpretation Introduction

Interpretation:

The equilibrium directions should be identified given the gas phase equilibrium reaction with different conditions.

Concept Introduction:

Concept of equilibrium process: The any system at equilibrium subject to change in concentration, temperature, volume or pressure then the system readjusts itself to partly counteract the effect of the applied change and new equilibrium is formed.  This equilibrium explain to simple way, a system equilibrium is distributed the system will adjust itself in such a way that the effect of the change will be reduced.

Le Chatelier's Principle: A change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.  In other words the closed system is an increase in pressure; the equilibrium will shift towards the sides of the reaction with some moles of gas.  The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Homogeneous equilibrium: A homogeneous equilibrium involved has everything present in the same phase and same conditions, for example reactions where everything is a gas, or everything is present in the same solution.

Heterogeneous equilibrium: This equilibrium reaction does not depend on the amounts of pure solid and liquid present, in other words heterogeneous equilibrium, substances are in different phases.

Answer to Problem 15.6.2SR

The equilibrium directions for given the statements of addition, removal and addition of reactants are given below.

$\begin{array}{l}{\text{A}}_{\text{2}}{}_{\text{(g)}}+{\text{B}}_{\text{2}}{}_{(g)}\rightleftharpoons {\text{2AB}}_{\text{(g)}}----\text{Equilibrium unaffected}\\ [IncreaseinVolume(V)]\end{array}$

Explanation of Solution

To Identify: Given the equilibrium reactions (c and d) volume, addition of (reactant and product species) should be analyzed.

Given both reactions (c and d) equilibrium directions must be analyzed.

$\begin{array}{l}{\text{A}}_{\text{2}}{}_{\text{(g)}}+{\text{B}}_{\text{2}}{}_{(g)}\rightleftharpoons {\text{2AB}}_{\text{(g)}}----\text{Equilibrium unaffected}\\ [IncreaseinVolume(V)]\end{array}$

Here also we will identify given the reaction process, Le Chatelier's Principle to determine which of the following process will cause the equilibrium shift to the right or left.   

Volume Increased: The given the reactions, if volume will increased, the pressure will be reduced or dropped, the boyle’s law explained pressure and volume are inversely proportional to the (P). So the (AB) will break down to produce more product molecules, hence the system of equilibrium will unaffected in this process.

Added a reactant (AB): The given the reactions (d) added some amount of (A and B) this is not a large that volume of the system is alternated, so equilibrium will shifted in to right side. If a highest amount of (AB) was added, this equilibrium will have the changing volume of the container.

(d)

Interpretation Introduction

Interpretation:

The equilibrium directions should be identified given the gas phase equilibrium reaction with different conditions.

Concept Introduction:

Concept of equilibrium process: The any system at equilibrium subject to change in concentration, temperature, volume or pressure then the system readjusts itself to partly counteract the effect of the applied change and new equilibrium is formed.  This equilibrium explain to simple way, a system equilibrium is distributed the system will adjust itself in such a way that the effect of the change will be reduced.

Le Chatelier's Principle: A change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.  In other words the closed system is an increase in pressure; the equilibrium will shift towards the sides of the reaction with some moles of gas.  The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Homogeneous equilibrium: A homogeneous equilibrium involved has everything present in the same phase and same conditions, for example reactions where everything is a gas, or everything is present in the same solution.

Heterogeneous equilibrium: This equilibrium reaction does not depend on the amounts of pure solid and liquid present, in other words heterogeneous equilibrium, substances are in different phases.

Answer to Problem 15.6.2SR

The equilibrium directions for given the statements of addition, removal and addition of reactants are given below.

$\begin{array}{l}{\text{A}}_{\text{2}}{}_{\text{(g)}}+{\text{B}}_{\text{2}}{}_{(g)}\rightleftharpoons {\text{2AB}}_{\text{(g)}}\text{----------Equilibrium shift to right}\\ [Additionof{\text{AB}}_{\text{(g)}}]\end{array}$

Explanation of Solution

To Identify: Given the equilibrium reactions volume, addition of (reactant and product species) should be analyzed.

Given both reactions equilibrium directions must be analyzed.

$\begin{array}{l}{\text{A}}_{\text{2}}{}_{\text{(g)}}+{\text{B}}_{\text{2}}{}_{(g)}\rightleftharpoons {\text{2AB}}_{\text{(g)}}\text{----------Equilibrium shift to right}\\ [Additionof{\text{AB}}_{\text{(g)}}]\end{array}$

Here also we will identify given the reaction process, Le Chatelier's Principle to determine which of the following process will cause the equilibrium shift to the right or left.   

Volume Increased: The given the reactions, if volume will increased, the pressure will be reduced or dropped, the boyle’s law explained pressure and volume are inversely proportional to the (P). So the (AB) will break down to produce more product molecules, hence the system of equilibrium will unaffected in this process.

Added a reactant (AB): The given the reactions (d) added some amount of ( A and B) this is not a large that volume of the system is alternated, so equilibrium will shifted in to right side. If a highest amount of (AB) was added, this equilibrium will have the changing volume of the container.