Chapter 16, Problem 88A

Interpretation Introduction

Interpretation:

The reason due to which increasing the temperature of a reaction by 10 k doubles the reaction rate needs to be explained using the collision theory.

Concept introduction:

Molecules undergo collision in the presence of the required amount of energy needed for collision to form some new molecules as well as in the presence of correct molecular orientation.

Answer to Problem 88A

The rate of the reaction doubles when the temperature is raised by 10 K because, the particles present in the reaction start moving faster with a greater amount of kinetic energy due to which, the collision will have sufficient energy to overcome the activation energy.

Explanation of Solution

Collision between two particles needs a sufficient amount of energy for the collision. The collision also needs a proper colliding orientation to take place. When the colliding particles break their bonds to form new bonds with the atoms of the particles it has undergo collision, a temporary transition state is generated which is an activated complex. Proper collision results in the formation of products.

If the temperature of a reaction is raised by 10 k, the particles present in the reaction start moving faster with a greater amount of kinetic energy. Because of this, more correctly oriented collision will have sufficient energy to overcome the activation energy. This is result in the increase in rate of the reaction.

Therefore, the rate of the reaction doubles when the temperature is raised by 10 K.

Conclusion

The rate of the reaction doubles when the temperature is raised by 10 K due to increase in the kinetic energy generated as the particles start moving faster.