Chapter 9, Problem 9.92EP

(a)

Interpretation Introduction

Interpretation:

For the reaction ${\text{CO(g) + H}}_{\text{2}}\text{O(g) + heat }\underset{}{\overset{}{\rightleftharpoons }}{\text{ CO}}_2{\text{(g) + H}}_2(g)$ the change in equilibrium shift has to be determined when the equilibrium mixture is heated.

Concept Introduction:

Le Chatelier’s principle:

If some forces applied, the system at equilibrium will get disrupted.  This change in equilibrium can be due to the change in pressure or temperature.  The change in reactant concentration can also disrupt the equilibrium.  Over time, the forward and backward reaction become equal and will attain a new equilibrium.  The equilibrium will shifts to right, if more products are formed and the system will shifts to left, if more reactants are formed.

The principle states that if some stress is applied to the system at equilibrium, the system will adjust itself in a direction which reduces the stress.

Temperature Changes:

Heat is one of the product in exothermic reaction and heat is used up in endothermic reaction.

Consider an exothermic reaction;

    ${\text{H}}_{\text{2}}{\text{(g)+F}}_{\text{2}}\text{(g)}\underset{}{\rightleftharpoons }\text{2HF(g)+heat}$

If heat is added up, then the reaction will shift to left so that the amount of heat will decrease.

Lowering the temperature will make the reaction to shift towards right.

Consider an endothermic reaction;

    ${\text{Heat+2CO}}_{\text{2}}\text{(g)}\underset{}{\rightleftharpoons }{\text{2CO(g)+O}}_{\text{2}}\text{(g)}$

Increase in temperature will shift the reaction towards right.

If heat is added up, then the reaction will shift towards right.

(b)

Interpretation Introduction

Interpretation:

For the reaction ${\text{CO(g) + H}}_{\text{2}}\text{O(g) + heat }\underset{}{\overset{}{\rightleftharpoons }}{\text{ CO}}_2{\text{(g) + H}}_2(g)$ the change in equilibrium shift has to be determined when pressure is increased by adding a nonreactive gas.

Concept Introduction:

Le Chatelier’s principle:

The principle states that if some stress is applied to the system at equilibrium, the system will adjust itself in a direction which reduces the stress.

(c)

Interpretation Introduction

Interpretation:

For the reaction ${\text{CO(g) + H}}_{\text{2}}\text{O(g) + heat }\underset{}{\overset{}{\rightleftharpoons }}{\text{ CO}}_2{\text{(g) + H}}_2(g)$ the change in equilibrium shift has to be determined when ${\text{H}}_{\text{2}}$ is added to the equilibrium mixture.

Concept Introduction:

Le Chatelier’s principle:

If some forces applied, the system at equilibrium will get disrupted.  This change in equilibrium can be due to the change in pressure or temperature.  The change in reactant concentration can also disrupt the equilibrium.  Over time, the forward and backward reaction become equal and will attain a new equilibrium.  The equilibrium will shifts to right, if more products are formed and the system will shifts to left, if more reactants are formed.

The principle states that if some stress is applied to the system at equilibrium, the system will adjust itself in a direction which reduces the stress

Concentration Changes:

Addition of reactant or product or removal of reactant or product from a system at equilibrium will affects the equilibrium.  If some reactant is added to a system at equilibrium, then the equilibrium will shifts to the product side, so that the added reactant get consumed.  If product is added then the equilibrium will shift towards left side.

Example:

  ${\text{N}}_{\text{2}}{\text{(g)+3H}}_{\text{2}}\text{(g)}\stackrel{}{\rightleftharpoons }{\text{2NH}}_{\text{3}}\text{(g)}$

If ${\text{N}}_{\text{2}}$ is added then the equilibrium will shift towards right.

If ${\text{NH}}_{\text{3}}$ is added then the equilibrium will shift towards left.

If ${\text{N}}_{\text{2}}$ is removed then the equilibrium will shift towards left.

(d)

Interpretation Introduction

Interpretation:

For the reaction ${\text{CO(g) + H}}_{\text{2}}\text{O(g) + heat }\underset{}{\overset{}{\rightleftharpoons }}{\text{ CO}}_2{\text{(g) + H}}_2(g)$ the change in equilibrium shift has to be determined when the size of the container is decreased.

Concept Introduction:

Le Chatelier’s principle:

If some forces applied, the system at equilibrium will get disrupted.  This change in equilibrium can be due to the change in pressure or temperature.  The change in reactant concentration can also disrupt the equilibrium.  Over time, the forward and backward reaction become equal and will attain a new equilibrium.  The equilibrium will shifts to right, if more products are formed and the system will shifts to left, if more reactants are formed.

The principle states that if some stress is applied to the system at equilibrium, the system will adjust itself in a direction which reduces the stress.