Chapter 17.2, Problem 14SSC

(a)

Interpretation Introduction

Interpretation:

The decreasing volume of reaction vessels which effects the equilibrium position is to be explained.

Concept introduction:

According to Le chatelier’s principle, when concentration is changes then the equilibrium shifts in response to a change in it. Equilibrium position is changes but its value $\left({\text{K}}_{\text{eq}}\right)$ is constant.

Answer to Problem 14SSC

By increasing the temperature, equilibrium position is shifts towards the reactants side ( ${\text{SO}}_{\text{2}}$ and ${\text{O}}_{\text{2}}$ ) so equilibrium constant is also increases. Thus, volume of the reaction vessels is decreases by increasing the temperature.

Explanation of Solution

According to Le Chatelier’s principle, by changing the temperature the equilibrium position is also changes. As temperature is decreases the equilibrium is shifts towards the right side or product side and vice versa. Changing the temperature favors one reaction over the other. On the other hand, at constant temperature the equilibrium is not affected.

Similarly, by increasing the temperature, equilibrium position is shifts towards the left side or reactants side so equilibrium constant is also increases. Thus, volume of the reaction vessels is decreases by increasing the temperature

In a given reaction

${\text{2SO}}_{\text{2}}\left(\text{g}\right){\text{ + O}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons {\text{2SO}}_{\text{3}}\left(\text{g}\right)$

The volume is decreasing by shifting the equilibrium towards the ${\text{SO}}_{\text{2}}$ and ${\text{O}}_{\text{2}}$ side by increasing the temperature.

(b)

Interpretation Introduction

Interpretation:

The decreasing volume of reaction vessels which effects the equilibrium position is to be explained

Concept introduction:

According to Le chatelier’s principle, when concentration is changes then the equilibrium shifts in response to a change in it. Equilibrium position is changes but equilibrium constant ${\text{K}}_{\text{eq}}$ is constant.

Answer to Problem 14SSC

By increasing the temperature, equilibrium position is shifts towards the reactants side ( ${\text{H}}_{\text{2}}$ and ${\text{Cl}}_{\text{2}}$ ) so equilibrium constant is also increases. Thus, volume of the reaction vessels is decreases by increasing the temperature.

Explanation of Solution

According to Le Chatelier’s principle, by changing the temperature the equilibrium position is also changes. As temperature is decreases the equilibrium is shifts towards the right side or product side and vice versa. Changing the temperature favors one reaction over the other. On the other hand, at constant temperature the equilibrium is not affected.

Similarly, by increasing the temperature, equilibrium position is shifts towards the left side or reactants side so equilibrium constant is also increases. Thus, volume of the reaction vessels is decreases by increasing the temperature

In a given reaction

${\text{H}}_{\text{2}}\left(\text{g}\right){\text{ + Cl}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons \text{2HCL }\left(\text{g}\right)$

The volume is decreasing by shifting the equilibrium towards the ${\text{H}}_{\text{2}}$ and ${\text{Cl}}_{\text{2}}$ side by increasing the temperature.