Collision Theory Chemistry Example 2

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Example 2

medium
Use collision theory to explain why increasing the concentration of reactants increases the reaction rate.

Solution

  1. 1
    Increasing concentration means there are more reactant particles per unit volume.
  2. 2
    More particles in the same space leads to more frequent collisions between reactant molecules.
  3. 3
    More frequent collisions means more effective collisions per unit time (collisions with sufficient energy and correct orientation), which increases the reaction rate.

Answer

HigherĀ concentrationĀ ā†’Ā moreĀ collisionsĀ ā†’Ā fasterĀ reactionĀ rate\text{Higher concentration ā†’ more collisions ā†’ faster reaction rate}
Collision theory quantitatively connects concentration to rate. If you double the concentration of a reactant, you approximately double the collision frequency, which approximately doubles the rate (for first-order dependence on that reactant).

About Collision Theory

A model explaining that chemical reactions occur only when reactant particles collide with sufficient kinetic energy (at least equal to the activation energy) and in.

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More Collision Theory Examples

Example 1 easy

State the three conditions required for a successful chemical reaction according to collision theory

Example 3 medium

Using collision theory, explain why a finely ground powder reacts faster than a large chunk of the s

Example 4 hard

Two reactions have the same activation energy, but Reaction A involves small, linear molecules while

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