Chapter 9.6, Problem 9.38QAP

Interpretation Introduction

(a)

Interpretation:

The given reaction should be classified as exothermic and endothermic reaction with their respective $\text{ΔH}$ values.

Concept Introduction:

A chemical reaction can be classified as endothermic and exothermic based on energy change. An endothermic reaction is the reaction which absorbs some heat during reaction whereas during exothermic reaction, heat or energy is released and product is formed.

  $\Delta H= \sum \Delta H_{product}- \sum \Delta H_{reactant}{}_{}$

The value and sign of $\text{ΔH}$ indicates the reaction as endothermic and exothermic reaction. $\text{ΔH}$ for any reaction is the energy difference between energy level of product and reactant molecules. The negative sign of $\text{ΔH}$ indicates the exothermic reaction and it is positive for endothermic reaction.

Interpretation Introduction

(b)

Interpretation:

The given reaction should be classified as exothermic and endothermic reaction with their respective $\text{ΔH}$ values.

Concept Introduction:

A chemical reaction can be classified as endothermic and exothermic based on energy change. An endothermic reaction is the reaction which absorbs some heat during reaction whereas during exothermic reaction, heat or energy is released and product is formed.

  $\Delta H= \sum \Delta H_{product}- \sum \Delta H_{reactant}{}_{}$

The value and sign of $\text{ΔH}$ indicates the reaction as endothermic and exothermic reaction. $\text{ΔH}$ for any reaction is the energy difference between energy level of product and reactant molecules. The negative sign of $\text{ΔH}$ indicates the exothermic reaction and it is positive for endothermic reaction.

Interpretation Introduction

(c)

Interpretation:

The given reaction should be classified as exothermic and endothermic reaction with their respective $\text{ΔH}$ values.

Concept Introduction:

A chemical reaction can be classified as endothermic and exothermic based on energy change. An endothermic reaction is the reaction which absorbs some heat during reaction whereas during exothermic reaction, heat or energy is released and product is formed.

  $\Delta H= \sum \Delta H_{product}- \sum \Delta H_{reactant}{}_{}$

The value and sign of $\text{ΔH}$ indicates the reaction as endothermic and exothermic reaction. $\text{ΔH}$ for any reaction is the energy difference between energy level of product and reactant molecules. The negative sign of $\text{ΔH}$ indicates the exothermic reaction and it is positive for endothermic reaction.