Chapter 16.2, Problem 14SSC

Interpretation Introduction

Interpretation:

The explanation for the collision theory that accounts for the effect of concentration on reaction rate needs to be given.

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. Due to this, activated complex may form products or may breaks to form reactants.

Answer to Problem 14SSC

Increase of concentration increases rate of reaction.

Explanation of Solution

Collision theory states that collision of particles is needed to undergo reaction. The more number of particles present, more the collision will occur. In case of a reaction of A and B, molecules of A and B undergoes collision to produce AB at particular rate. If the concentration of B increased, molecules of A undergoes more frequent collision with molecules of B because of higher availability of molecules of B. More collision thus increases rate of reaction.

Conclusion

According to collision theory rate of reaction increases because of increase of concentration of reactants.