Question

How do you explain the effect of concentration on the rate of reaction on the basis of collision theory?

Short answer

Based on the collision theory, explain the effect of concentration on the rate of reaction. An increase in the concentration of one or both reactants results in a higher frequency of collisions between the reactant molecules, leading to an increased rate of reaction. This is because there are more reacting molecules present in a given volume, which increases the probability of successful collisions between reactant particles. The collision theory models this relationship, explaining that the number of collisions between reacting molecules per unit time determines the rate of a chemical reaction.

Step-by-step solution

Understand the Collision Theory

The collision theory is a model used to explain the relationship between the rate of a chemical reaction and the concentration of reactants. The theory states that a reaction occurs when reacting molecules collide with each other with the proper orientation and sufficient energy. This means that the more collisions that occur per unit time, the greater the rate of the reaction.

Define the Relationship between Concentration and Number of Collisions

As the concentration of the reactants increases, there are more reacting molecules present in the same given volume. This leads to a higher probability of collisions between the reactant particles, which in turn increases the frequency of successful collisions and thus increases the rate of reaction.

Describe the Effect of Concentration on Collision Frequency

When the concentration of one or both reactants is increased, the frequency of collisions between the reactant molecules also increases. As there are more reactant particles in a given volume, they are more likely to collide with each other. Consequently, the rate of reaction increases, reflecting the greater number of successful collisions that occur per unit time.

Explain the Relationship between Concentration and the Rate of Reaction

The relationship between concentration and the rate of reaction can be formulated as a rate equation: Rate = k[A]^m[B]^n, where 'Rate' is the rate of reaction, 'k' is the rate constant, '[A]' and '[B]' are the concentrations of the reactants, and 'm' and 'n' are the order of reaction with respect to the reactants A and B. The values of 'm' and 'n' indicate the effect of concentration on the rate of reaction, with larger values meaning a stronger effect. Ultimately, an increase in the concentration of one or both reactants results in a higher frequency of collisions between the reactant molecules, leading to an increased rate of reaction, as explained by the collision theory.