Chapter 9, Problem 9.96EP

(a)

Interpretation Introduction

Interpretation:

For the reaction ${\text{heat + H}}_{\text{2}}{\text{(g) + I}}_{\text{2}}\text{(g) }\underset{}{\rightleftharpoons }\text{ 2HI(g)}$, whether the product formation increases or not with increasing temperature has to be indicated.

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 ${\text{CO(g) + 2H}}_{\text{2}}\text{(g) }\underset{}{\rightleftharpoons }{\text{ CH}}_{\text{4}}\text{O(g) + heat}$, whether the product formation increases or not with increasing temperature has to be indicated.

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.

(c)

Interpretation Introduction

Interpretation:

For the reaction ${\text{4NH}}_3{\text{(g) + 5O}}_{\text{2}}\text{(g) }\underset{}{\rightleftharpoons }{\text{ heat + 4NO(g) + 6H}}_{\text{2}}\text{O(g) }$, whether the product formation increases or not with increasing temperature has to be indicated.

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 and attain a new equilibrium.

(d)

Interpretation Introduction

Interpretation:

For the reaction ${\text{heat + 2NaHCO}}_3\text{(s) }\underset{}{\rightleftharpoons }{\text{ Na}}_2{\text{CO}}_3{\text{(s) + CO}}_2{\text{(g) + H}}_{\text{2}}\text{O(g)}$, whether the product formation increases or not with increasing temperature has to be indicated.

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 and attain a new equilibrium.