Chapter 17, Problem 17.72P

(a)

Interpretation Introduction

Interpretation:

The effect of increase in the temperature has to be predicted on the amount of products formed in the given reaction.

  ${\text{CO (g)+2H}}_{\text{2}}\text{ (g)}\rightleftharpoons {\text{CH}}_{\text{3}}\text{OH (g)}{\text{ΔH}}_{\text{r×n}}^{\text{°}}\text{ = -90}\text{.7kJ}$

Concept Introduction:

Le Chatelier’s principle:

Le Chatelier’s principle states that the changes in the temperature, pressure, volume and concentration of the system results in the change in system to attain new equilibrium.  It is used to understand the conditions of a reaction which favours increased product formation.

The reactions of heat are of two types:

1. 1. Exothermic reaction – releases heat
2. 2. Endothermic reaction – absorbs heat

Change in equilibrium due to temperature changes:

If the temperature is increased for the system, the equilibrium shifts away from the heat because of the reaction needs extra heat to use.

If the temperature is decreased for the system, the equilibrium shifts towards the heat because the heat needs to be produced to make up for the loss.

(b)

Interpretation Introduction

Interpretation:

The effect of increase in the temperature has to be predicted on the amount of products formed in the given reaction.

  ${\text{C (s) + H}}_{\text{2}}\text{O (g)}\rightleftharpoons {\text{CO (g) + H}}_{\text{2}}\text{(g)}{\text{ΔH}}_{\text{r×n}}^{\text{°}}\text{ = 131kJ}$

Concept Introduction:

Le Chatelier’s principle:

Le Chatelier’s principle states that the changes in the temperature, pressure, volume and concentration of the system results in the change in system to attain new equilibrium.  It is used to understand the conditions of a reaction which favours increased product formation.

The reactions of heat are of two types:

1. 1. Exothermic reaction – releases heat
2. 2. Endothermic reaction – absorbs heat

Change in equilibrium due to temperature changes:

If the temperature is increased for the system, the equilibrium shifts away from the heat because of the reaction needs extra heat to use.

If the temperature is decreased for the system, the equilibrium shifts towards the heat because the heat needs to be produced to make up for the loss.

(c)

Interpretation Introduction

Interpretation:

The effect of increase in the temperature has to be predicted on the amount of products formed in the given reaction.

  ${\text{2NO}}_{\text{2}}\text{ (g)}\rightleftharpoons {\text{2NO (g) + O}}_{\text{2}}\text{(g)}\text{(endothermic)}$

Concept Introduction:

Le Chatelier’s principle:

Le Chatelier’s principle states that the changes in the temperature, pressure, volume and concentration of the system results in the change in system to attain new equilibrium.  It is used to understand the conditions of a reaction which favours increased product formation.

The reactions of heat are of two types:

1. 1. Exothermic reaction – releases heat
2. 2. Endothermic reaction – absorbs heat

Change in equilibrium due to temperature changes:

If the temperature is increased for the system, the equilibrium shifts away from the heat because of the reaction needs extra heat to use.

If the temperature is decreased for the system, the equilibrium shifts towards the heat because the heat needs to be produced to make up for the loss.

(d)

Interpretation Introduction

Interpretation:

The effect of increase in the temperature has to be predicted on the amount of products formed in the given reaction.

  ${\text{2C (s) + O}}_{\text{2}}\text{(g)}\rightleftharpoons \text{2CO (g)}\text{(exothermic)}$

Concept Introduction:

Le Chatelier’s principle:

Le Chatelier’s principle states that the changes in the temperature, pressure, volume and concentration of the system results in the change in system to attain new equilibrium.  It is used to understand the conditions of a reaction which favours increased product formation.

The reactions of heat are of two types:

1. 1. Exothermic reaction – releases heat
2. 2. Endothermic reaction – absorbs heat

Change in equilibrium due to temperature changes:

If the temperature is increased for the system, the equilibrium shifts away from the heat because of the reaction needs extra heat to use.

If the temperature is decreased for the system, the equilibrium shifts towards the heat because the heat needs to be produced to make up for the loss.