Chapter 16.4, Problem 38SSC

Interpretation Introduction

Interpretation:

The relation of size of the activation energy of an elementary step in a complex reaction and the rate of that step needs to be explained.

Concept introduction:

Chemical kinetic is the branch of chemistry that deals with kinetic or rate of a chemical reaction. The rate of reaction can be defined as the change in the concentration of reactant and product with time. The rate of reaction mainly depends on the activation energy.

In a chemical reaction to be occurred; two most important requirements are activation energy to reactant molecule and correct orientation of reactant molecules to colloid and form product. The minimum energy that is required for the conversion reactant to product is called as activation energy.

Answer to Problem 38SSC

The high activation energy of an elementary step will slow down the rate of that step of the reaction.

Explanation of Solution

Given information:

The activation energy of an elementary step is related to the rate of that step.

A chemical reaction can involve one or multiple steps during the conversion of reactant to product.

Once the reactant molecules acquire activation energy, they form activated complex which is highly unstable due to highest energy and readily converts to product.

The elementary step with high activation energy will move with slow rate as it will take more time and energy for reactant molecules to acquire the activation energy and get convert to product. Thus high activation energy of an elementary step will slow down the rate of that step of the reaction.

Conclusion

The activation energy of an elementary step determines the rate of that step of the reaction.