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 accounts for the increased reaction rate when the concentrations of reactants are increased by explaining that higher concentrations lead to a higher frequency of collisions between reactant molecules and a higher probability of successful collisions. This ultimately results in a faster reaction rate.

Step-by-step solution

Understand the collision model

The collision model is a theory that explains how chemical reactions occur and why they have certain reaction rates. It is based on the idea that molecules must collide with each other with a certain minimum energy (called the activation energy) and in the correct orientation for a reaction to occur.

Explain the role of concentration in the collision model

In the collision model, the concentration of reactants plays an important role in determining the rate of the reaction. As the concentration of reactants increases, there are more molecules in a given volume. This higher molecular density leads to a higher frequency of collisions between the reactant molecules.

Relate increased concentrations to increased collision frequency

When the concentrations of reactants are increased, there are more molecules available to collide with each other in a given space. As a result, the likelihood of collisions between reactant molecules also increases. This means that there is a higher probability of successful collisions, leading to the formation of product molecules.

Describe how increased collision frequency affects reaction rate

According to the collision model, a faster reaction rate is observed when the number of successful collisions per unit time is larger. Since increasing the concentration of reactants leads to more frequent collisions, the probability of successful collisions also increases, resulting in a faster reaction rate. In conclusion, the collision model accounts for the fact that a reaction proceeds faster when the concentrations of the reactants are increased by explaining that higher concentrations lead to more frequent and successful collisions, ultimately increasing the reaction rate.