Explain how various environmental and physical factors affect reaction rates by applying collision theory.
Understand that chemical reactions can only occur when reacting particles successfully collide with each other and possess sufficient energy.
Define activation energy as the absolute minimum amount of energy that reacting particles must have to successfully react.
Explain that increasing the concentration of solutions, the pressure of gases, and the surface area of solid reactants directly increases the frequency of particle collisions, subsequently increasing the overall reaction rate.
Explain that increasing the temperature increases both the frequency of collisions and the proportion of collisions that are energetic enough to react, leading to an increased rate of reaction.
Predict and explain the effects of changing concentration, pressure, and temperature on reaction rates using the principles of collision theory.
Predict and explain the effects of altering the size of solid reactant pieces by referencing the surface area to volume ratio.
Apply simple concepts of mathematical proportionality to collision theory when explaining the effect of a specific factor on the rate of a reaction.
