Chapter 16.1, Problem 8SSC

Interpretation Introduction

Interpretation:

The relationship between activation energy and rate of a chemical reaction needs to be explained.

Concept introduction:

According to the collision theory, collision of reacting molecules in correct orientation with sufficient energy leads to form an activated complex. Activated complex is also termed as transition state, which is temporary and possess unstable arrangement of atoms where old bonds breaks and new bonds formed. As a result, the activated complex might form products or might break apart to form the reactants.

Answer to Problem 8SSC

Higher activation energy indicates reaction rate is slow and low activation energy indication faster reaction rate.

Explanation of Solution

The collision of molecules results in the formation of activated complex. Activation energy is the minimum amount of energy that the reacting molecules have to form the activation energy. High activation energy indicates the need of few collisions to form the activated complex and thus the reaction rate is slow. Low activation energy indicates the more collisions have sufficient energy to react and the reaction rate is faster.

Conclusion

The collision theory states the product will form when the reacting molecules collide with each other with proper orientation.