Chapter 17, Problem 63A

Interpretation Introduction

Interpretation:

The fact that number of collisions between the reactant molecules increases when the temperature of the reaction is increased has to be explained. Increase in the temperature of the reaction on a molecular basis has to be explained.

Concept Introduction:

Collision theory: According to this theory, for a chemical reaction to take place, the collision must occur between the reactant molecules. However, all the collisions are not effective. Only those collisions are effective in result in chemical reaction in which colliding molecules must possess a certain minimum energy called threshold energy.

Answer to Problem 63A

With increasing the temperature, the chance of collisions increases because the average kinetic energy of the molecules increase..

With increasing temperature, the molecules get threshold energy. So, reaction proceeds at faster rate.

Explanation of Solution

The rate of the reaction increases with increasing the temperature of the reaction. With increasing the temperature of the reaction the reactant molecules move at a faster rate. Therefore the chance of collisions to take place increases. Thus the rate of the reaction increases. Again with increasing the temperature the average kinetic energy of the molecules increase. So, the collisions between the reacting molecules are more at higher temperatures than at lower temperatures.

With increasing temperature more number of molecules with lower energy can reach the threshold energy. The reaction proceeds at faster rate.