Question

How does the collision model account for the fact that a reaction proceeds faster when the concentrations of the reactants are increased?

Short answer

The collision model explains that a reaction occurs when reactant molecules collide with sufficient energy and proper orientation. When the concentrations of the reactants are increased, there are more molecules present, leading to a higher probability of collisions. This results in a higher frequency of successful collisions, which in turn increases the reaction rate. Therefore, the collision model accounts for the fact that a reaction proceeds faster when the concentrations of the reactants are increased due to the higher probability of successful collisions between reactant molecules.

Step-by-step solution

Understand the Collision Model

The collision model explains how the reaction rates are affected by the number of collisions between reactant molecules. For a reaction to occur, the molecules must collide with sufficient energy (known as activation energy) and proper orientation. The more collisions that meet these criteria, the faster the reaction will proceed.

Discuss the Effect of Concentration on Collisions

When the concentration of reactants increases, there are more molecules present in the reaction mixture. This leads to a higher probability of collisions between these molecules. The more collisions that occur, the higher the chances for successful collisions that result in a reaction.

Explain the Relationship Between Concentration and Reaction Rate

An increase in concentration leads to a higher frequency of successful collisions between reactant molecules. As a result, the reaction rate increases. Conversely, a decrease in concentration will lower the frequency of successful collisions and reduce the reaction rate.

Summarize the Collision Model's Explanation for Higher Concentrations

In summary, the collision model accounts for the fact that a reaction proceeds faster when the concentrations of the reactants are increased due to the higher probability of successful collisions between reactant molecules. An increase in concentration leads to more collisions, which in turn increases the reaction rate.