Chapter U6, Problem C24.I2RE

Interpretation Introduction

Interpretation:

The effect of adding ${\text{SO}}_{\text{2}}\text{(g)}$ to the following equilibrium mixture needs to be describe:

${\text{SO}}_{\text{2}}{\text{(g) + NO}}_{\text{2}}\text{(g) }\rightleftharpoons {\text{ SO}}_{\text{3}}\text{(g) + NO(g)}$

Concept introduction:

According to LeChatlier's principle, when a dynamic equilibrium is subjected to a change in either concentration or temperature or pressure, then the position of equilibrium will shift in such a direction that it nullifies the change.

For example:

$\text{A + B }\rightleftharpoons \text{ C}$ is a system at equilibrium.

If concentration of A is increased by adding some more amount of A at equilibrium, then left side concentration is increasing, so to nullify this change, equilibrium shifts towards right side. Hence, forward reaction or formation of C is favoured in this case.

Answer to Problem C24.I2RE

The concentration of reactants will decrease and that of products will increase and hence, resulting in increase in ${\text{K}}_{\text{eq}}$ value.

Explanation of Solution

The given equilibrium mixture described by equation is:

${\text{SO}}_{\text{2}}{\text{(g) + NO}}_{\text{2}}\text{(g) }\rightleftharpoons {\text{ SO}}_{\text{3}}\text{(g) + NO(g)}$

The addition of ${\text{SO}}_{\text{2}}\text{(g)}$ to the above equilibrium mixture means that the concentration of the reactant increases. Now, according to LeChatlier's principle, the equilibrium will shift in forward direction (product side as the concentration of reactant is increasing) in order to nullify the change. Thus, on adding ${\text{SO}}_{\text{2}}\text{(g)}$ to the given equilibrium equation, the concentration of reactants will decrease and that of products will increase and hence, resulting in increase in ${\text{K}}_{\text{eq}}$ value.

Interpretation Introduction

Interpretation:

The effect of adding $\text{NO(g)}$ to the following equilibrium mixture needs to be describe:

${\text{SO}}_{\text{2}}{\text{(g) + NO}}_{\text{2}}\text{(g) }\rightleftharpoons {\text{ SO}}_{\text{3}}\text{(g) + NO(g)}$

Concept introduction:

According to LeChatlier's principle, when a dynamic equilibrium is subjected to a change in either concentration or temperature or pressure, then the position of equilibrium will shift in such a direction that it nullifies the change.

For example:

$\text{A + B }\rightleftharpoons \text{ C}$ is a system at equilibrium.

If concentration of A is increased by adding some more amount of A at equilibrium, then left side concentration is increasing, so to nullify this change, equilibrium shifts towards right side. Hence, forward reaction or formation of C is favoured in this case.

Answer to Problem C24.I2RE

The concentration of reactants will increase and that of products will decrease and hence, resulting in decrease in ${\text{K}}_{\text{eq}}$ value.

Explanation of Solution

The given equilibrium mixture described by equation is:

${\text{SO}}_{\text{2}}{\text{(g) + NO}}_{\text{2}}\text{(g) }\rightleftharpoons {\text{ SO}}_{\text{3}}\text{(g) + NO(g)}$

The addition of $\text{NO(g)}$ to the above equilibrium mixture means that the concentration of the product increases. Now, according to LeChatlier's principle, the equilibrium will shift in backward direction (reactant side as the concentration of product is increasing) in order to nullify the change. Thus, on adding $\text{NO(g)}$ to the given equilibrium equation, the concentration of reactants will increase and that of products will decrease and hence, resulting in decrease in ${\text{K}}_{\text{eq}}$ value.

Interpretation Introduction

Interpretation:

The effect of removing ${\text{SO}}_{\text{3}}\text{(g)}$ to the following equilibrium mixture needs to be describe:

${\text{SO}}_{\text{2}}{\text{(g) + NO}}_{\text{2}}\text{(g) }\rightleftharpoons {\text{ SO}}_{\text{3}}\text{(g) + NO(g)}$

Concept introduction:

According to LeChatlier's principle, when a dynamic equilibrium is subjected to a change in either concentration or temperature or pressure, then the position of equilibrium will shift in such a direction that it nullifies the change.

For example:

$\text{A + B }\rightleftharpoons \text{ C}$ is a system at equilibrium.

If concentration of A is increased by adding some more amount of A at equilibrium, then left side concentration is increasing, so to nullify this change, equilibrium shifts towards right side. Hence, forward reaction or formation of C is favoured in this case.

Answer to Problem C24.I2RE

The concentration of reactants will decrease and that of products will increase and hence, resulting in increase in ${\text{K}}_{\text{eq}}$ value.

Explanation of Solution

The given equilibrium mixture described by equation is:

${\text{SO}}_{\text{2}}{\text{(g) + NO}}_{\text{2}}\text{(g) }\rightleftharpoons {\text{ SO}}_{\text{3}}\text{(g) + NO(g)}$

The removal of ${\text{SO}}_{\text{3}}\text{(g)}$ from the above equilibrium mixture means that the concentration of the product decreases. Now, according to LeChatlier's principle, the equilibrium will shift in forward direction (product side as the concentration of product is decreasing) in order to nullify the change. Thus, on removing ${\text{SO}}_{\text{3}}\text{(g)}$ from the given equilibrium equation, the concentration of reactants will decrease and that of products will increase and hence, resulting in increase in ${\text{K}}_{\text{eq}}$ value.

Interpretation Introduction

Interpretation:

The effect on adding equal amount of ${\text{SO}}_{\text{3}}\text{(g)}$ and ${\text{SO}}_2\text{(g)}$ to the following equilibrium mixture needs to be describe:

${\text{SO}}_{\text{2}}{\text{(g) + NO}}_{\text{2}}\text{(g) }\rightleftharpoons {\text{ SO}}_{\text{3}}\text{(g) + NO(g)}$

Concept introduction:

According to LeChatlier's principle, when a dynamic equilibrium is subjected to a change in either concentration or temperature or pressure, then the position of equilibrium will shift in such a direction that it nullifies the change.

For example:

$\text{A + B }\rightleftharpoons \text{ C}$ is a system at equilibrium.

If concentration of A is increased by adding some more amount of A at equilibrium, then left side concentration is increasing, so to nullify this change, equilibrium shifts towards right side. Hence, forward reaction or formation of C is favoured in this case.

Answer to Problem C24.I2RE

No change in ${\text{K}}_{\text{eq}}$ value.

Explanation of Solution

The given equilibrium mixture described by equation is:

${\text{SO}}_{\text{2}}{\text{(g) + NO}}_{\text{2}}\text{(g) }\rightleftharpoons {\text{ SO}}_{\text{3}}\text{(g) + NO(g)}$

The adding equal amount of ${\text{SO}}_{\text{3}}\text{(g)}$ and ${\text{SO}}_2\text{(g)}$ to the above equilibrium mixture means that the concentration of both the product and the reactant increase in same amount. Now, according to LeChatlier's principle, there will be no change in equilibrium as the amount added on both sides of equation is equal. Thus, on adding equal amount of ${\text{SO}}_{\text{3}}\text{(g)}$ and ${\text{SO}}_2\text{(g)}$ to the given equilibrium equation, the concentration of reactants and that of products will increase in same amount and hence, resulting in no change in ${\text{K}}_{\text{eq}}$ value.