The reason for relation between the activation energy and enthalpy change for endothermic reaction and no such relation for exothermic reaction needs to be explained. Concept introduction: A chemical reaction is said to be endothermic, if energy is given to the system. In such cases, heat is in the reactant side. The value of change in enthalpy is positive as it is added to the system. The energy of reactant is less than that of product in this case. On the other hand, for exothermic reaction heat is released and it is present in product side. The energy of product is less than that of reactant in this case. The value of change in enthalpy is negative for exothermic reactions. The activation energy is defined as the minimum amount of energy needed to start a reaction.

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Chapter 20, Problem 48E

Interpretation Introduction

Interpretation:

The reason for relation between the activation energy and enthalpy change for endothermic reaction and no such relation for exothermic reaction needs to be explained.

Concept introduction:

A chemical reaction is said to be endothermic, if energy is given to the system. In such cases, heat is in the reactant side. The value of change in enthalpy is positive as it is added to the system. The energy of reactant is less than that of product in this case. On the other hand, for exothermic reaction heat is released and it is present in product side. The energy of product is less than that of reactant in this case. The value of change in enthalpy is negative for exothermic reactions.

The activation energy is defined as the minimum amount of energy needed to start a reaction.

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