Chapter 6, Problem 95AE

(a)

Interpretation Introduction

Interpretation:Whether increase in temperature will increase the value of $K$ should be predicted for indicated endothermic equilibrium.

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

Concept introduction:Le Chatelier established the qualitative effects of change in concentration or partial pressure of reactant on reaction equilibrium.

It suggests that if a certain change in concentration of substrates occurs then reaction proceeds so as to minimize the effects of changes. This way the direction of equilibrium can be altered by various changes and yield of desired ${\text{NH}}_{\text{3}}$ product can be enhanced. For example, Le Chatelier has improved the synthesis of ${\text{NH}}_{\text{3}}$ by Haber’s process.

Explanation of Solution

The endothermic equilibrium reaction for decomposition of ${\text{SO}}_3$ is given as follows:

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

The expression of equilibrium constant for above reaction is written as follows:

  $K=\frac{{\left[{\text{SO}}_2\right]}^2\left[{\text{O}}_2\right]}{{\left[{\text{SO}}_3\right]}^2}$

Where,

• $\left[{\text{SO}}_2\right]$ denotes concentration of ${\text{SO}}_2$ .
• $\left[{\text{O}}_2\right]$ denotes concentration of ${\text{O}}_2$ .
• $\left[{\text{SO}}_3\right]$ denotes concentration of ${\text{SO}}_3$ .
• $K$ denotes equilibrium constant.

Increase in temperature favors the equilibrium in forward direction thus more decomposition of ${\text{SO}}_2$ will occur. So this increase in temperature will increase the magnitude of $K$ .

(b)

Interpretation Introduction

Interpretation: Whether decrease in temperature will increase the value of $K$ should be predicted for indicated endothermic equilibrium.

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

Concept introduction:Le Chatelier established the qualitative effects of change in concentration or partial pressure of reactant on reaction equilibrium.

It suggests that if a certain change in concentration of substrates occurs then reaction proceeds so as to minimize the effects of changes. This way the direction of equilibrium can be altered by various changes and yield of desired ${\text{NH}}_{\text{3}}$ product can be enhanced. For example, Le Chatelier has improved the synthesis of ${\text{NH}}_{\text{3}}$ by Haber’s process.

Explanation of Solution

The endothermic equilibrium reaction for decomposition of ${\text{SO}}_3$ is given as follows:

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

The expression of equilibrium constant for above reaction is written as follows:

  $K=\frac{{\left[{\text{SO}}_2\right]}^2\left[{\text{O}}_2\right]}{{\left[{\text{SO}}_3\right]}^2}$

Where,

• $\left[{\text{SO}}_2\right]$ denotes concentration of ${\text{SO}}_2$ .
• $\left[{\text{O}}_2\right]$ denotes concentration of ${\text{O}}_2$ .
• $\left[{\text{SO}}_3\right]$ denotes concentration of ${\text{SO}}_3$ .
• $K$ denotes equilibrium constant.

Decrease in temperature for above endothermic equilibrium will favor reaction in backward direction and so magnitude of $K$ will decrease.

(c)

Interpretation Introduction

Interpretation: Whether decrease in ${\text{SO}}_3$ at constant temperature will increase the value of $K$ should be predicted for indicated endothermic equilibrium.

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

Concept introduction:Le Chatelier established the qualitative effects of change in concentration or partial pressure of reactant on reaction equilibrium.

It suggests that if a certain change in concentration of substrates occurs then reaction proceeds so as to minimize the effects of changes. This way the direction of equilibrium can be altered by various changes and yield of desired ${\text{NH}}_{\text{3}}$ product can be enhanced. For example, Le Chatelierhas improved the synthesis of ${\text{NH}}_{\text{3}}$ by Haber’s process.

Explanation of Solution

The endothermic equilibrium reaction for decomposition of ${\text{SO}}_3$ is given as follows:

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

The expression of equilibrium constant for above reaction is written as follows:

  $K=\frac{{\left[{\text{SO}}_2\right]}^2\left[{\text{O}}_2\right]}{{\left[{\text{SO}}_3\right]}^2}$

Where,

• $\left[{\text{SO}}_2\right]$ denotes concentration of ${\text{SO}}_2$ .
• $\left[{\text{O}}_2\right]$ denotes concentration of ${\text{O}}_2$ .
• $\left[{\text{SO}}_3\right]$ denotes concentration of ${\text{SO}}_3$ .
• $K$ denotes equilibrium constant.

If ${\text{SO}}_3$ is removed at constant temperature the magnitude of $K$ will not change as it remains constant for a particular temperature and so at constant temperature value will not change.

(d)

Interpretation Introduction

Interpretation: Whether reduction in volume at constant temperature will increase the value of $K$ should be predicted for indicated endothermic equilibrium.

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

Concept introduction:Le Chatelier established the qualitative effects of change in concentration or partial pressure of reactant on reaction equilibrium.

It suggests that if a certain change in concentration of substrates occurs then reaction proceeds so as to minimize the effects of changes. This way the direction of equilibrium can be altered by various changes and yield of desired ${\text{NH}}_{\text{3}}$ product can be enhanced. For example, Le Chatelier has improved the synthesis of ${\text{NH}}_{\text{3}}$ by Haber’s process.

Explanation of Solution

The endothermic equilibrium reaction for decomposition of ${\text{SO}}_3$ is given as follows:

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

The expression of equilibrium constant for above reaction is written as follows:

  $K=\frac{{\left[{\text{SO}}_2\right]}^2\left[{\text{O}}_2\right]}{{\left[{\text{SO}}_3\right]}^2}$

Where,

• $\left[{\text{SO}}_2\right]$ denotes concentration of ${\text{SO}}_2$ .
• $\left[{\text{O}}_2\right]$ denotes concentration of ${\text{O}}_2$ .
• $\left[{\text{SO}}_3\right]$ denotes concentration of ${\text{SO}}_3$ .
• $K$ denotes equilibrium constant.

If volume is reduced at constant temperature, the magnitude of $K$ will not change as it remains constant for a particular temperature and so at constant temperature value will not change.

(e)

Interpretation Introduction

Interpretation: Whether addition of inert $\text{Ne}$ at constant temperature will increase the value of $K$ should be predicted for indicated endothermic equilibrium.

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

Concept introduction:Le Chatelier established the qualitative effects of change in concentration or partial pressure of reactant on reaction equilibrium.

It suggests that if a certain change in concentration of substrates occurs then reaction proceeds so as to minimize the effects of changes. This way the direction of equilibrium can be altered by various changes and yield of desired ${\text{NH}}_{\text{3}}$ product can be enhanced. For example, Le Chatelier has improved the synthesis of ${\text{NH}}_{\text{3}}$ by Haber’s process.

Explanation of Solution

The endothermic equilibrium reaction for decomposition of ${\text{SO}}_3$ is given as follows:

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

The expression of equilibrium constant for above reaction is written as follows:

  $K=\frac{{\left[{\text{SO}}_2\right]}^2\left[{\text{O}}_2\right]}{{\left[{\text{SO}}_3\right]}^2}$

Where,

• $\left[{\text{SO}}_2\right]$ denotes concentration of ${\text{SO}}_2$ .
• $\left[{\text{O}}_2\right]$ denotes concentration of ${\text{O}}_2$ .
• $\left[{\text{SO}}_3\right]$ denotes concentration of ${\text{SO}}_3$ .
• $K$ denotes equilibrium constant.

Addition of inert gas such as $\text{Ne}$ at constant temperature again will not change as it remains constant for a particular temperature and so at constant temperature, the value will not change.

(f)

Interpretation Introduction

Interpretation: Whether ${\text{SO}}_2$ addition at constant temperature will increase the value of $K$ should be predicted for indicated endothermic equilibrium.

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

Concept introduction:Le Chatelier established the qualitative effects of change in concentration or partial pressure of reactant on reaction equilibrium.

It suggests that if a certain change in concentration of substrates occurs then reaction proceeds so as to minimize the effects of changes. This way the direction of equilibrium can be altered by various changes and yield of desired ${\text{NH}}_{\text{3}}$ product can be enhanced. For example, the Le Chatelier has improved the synthesis of ${\text{NH}}_{\text{3}}$ by Haber’s process.

Explanation of Solution

The endothermic equilibrium reaction for decomposition of ${\text{SO}}_3$ is given as follows:

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

The expression of equilibrium constant for above reaction is written as follows:

  $K=\frac{{\left[{\text{SO}}_2\right]}^2\left[{\text{O}}_2\right]}{{\left[{\text{SO}}_3\right]}^2}$

Where,

• $\left[{\text{SO}}_2\right]$ denotes concentration of ${\text{SO}}_2$ .
• $\left[{\text{O}}_2\right]$ denotes concentration of ${\text{O}}_2$ .
• $\left[{\text{SO}}_3\right]$ denotes concentration of ${\text{SO}}_3$ .
• $K$ denotes equilibrium constant.

If ${\text{SO}}_2$ is added at constant temperature the magnitude of $K$ will not change as it remains constant for a particular temperature and so at constant temperature value will not change.

(h)

Interpretation Introduction

Interpretation: Whether catalyst addition at constant temperature will increase the value of $K$ should be predicted for indicated endothermic equilibrium.

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

Concept introduction: Le Chatelier established the qualitative effects of change in concentration or partial pressure of reactant on reaction equilibrium.

It suggests that if a certain change in concentration of substrates occurs then reaction proceeds so as to minimize the effects of changes. This way the direction of equilibrium can be altered by various changes and yield of desired ${\text{NH}}_{\text{3}}$ product can be enhanced. For example, Le Chatelier has improved the synthesis of ${\text{NH}}_{\text{3}}$ by Haber’s process.

Explanation of Solution

The endothermic equilibrium reaction for decomposition of ${\text{SO}}_3$ is given as follows:

  ${\text{2SO}}_3\left(g\right)\rightleftharpoons 2{\text{SO}}_2\left(g\right)+{\text{O}}_2\left(g\right)$

The expression of equilibrium constant for above reaction is written as follows:

  $K=\frac{{\left[{\text{SO}}_2\right]}^2\left[{\text{O}}_2\right]}{{\left[{\text{SO}}_3\right]}^2}$

Where,

Where,

• $\left[{\text{SO}}_2\right]$ denotes concentration of ${\text{SO}}_2$ .
• $\left[{\text{O}}_2\right]$ denotes concentration of ${\text{O}}_2$ .
• $\left[{\text{SO}}_3\right]$ denotes concentration of ${\text{SO}}_3$ .
• $K$ denotes equilibrium constant.

If catalyst is added at constant temperature to attain the equilibrium quickly butkinetics is independent upon the equilibrium of the reaction and thus moles of each species will remain unchanged.