Collision Theory and Kinetics Quiz

Collision Theory

Explains how reactant collisions lead to chemical reactions

Activation Energy

Energy required to start a chemical reaction

Stirring Effect

Increases collisions, affecting reaction rate

Concentration Change Effect

Increasing concentration speeds up reaction due to more collisions

Temperature Change Effect

Increasing temperature speeds up reaction due to faster particle movement

Activation Energy (uncatalyzed)

Energy needed for the reaction to start without a catalyst

Activation Energy (catalyzed)

Energy needed for the reaction to start with a catalyst

Catalyst Function

Lowers activation energy, altering reaction rate

Surface Area Effect

Increasing surface area speeds up reaction by allowing more collisions

Iron Rusting Experiment

Demonstrates how surface area affects reaction time

Nature of Reactants

Factor affecting substance burning rate in different environments

Temperature Change Impact

Affects activation energy and reaction rate

Solid Reactant Surface Area

Breaking into smaller pieces speeds up the reaction