Unit 10: Chemical Kinetics

Description

In this unit the focus will be on determining differential and integrated rate laws. Graphic representation of zero, first and second-order reactions and their half-lives will be emphasized. Simplification by writing pseudo rate laws will be discussed. Reaction mechanisms and a model for chemical kinetics will be introduced. Activation energy will be calculated from the Arrhenius equation and from rate constant and temperature data. Catalyzed and non-catalyzed reaction data will be reviewed.

Enduring Understandings

Students will understand that:

• A spontaneous reaction may or may not happen fast.
• Chemical kinetics deals with the rate at which a reaction does occur.
• Most reactions actually occur in a series of steps known as the reaction mechanism with the reactants being the initial step and the products being the final step.

Essential Questions

• Why wouldn't a spontaneous reaction happen quickly?
• How does reaction rate change over time?
• How are reaction mechanisms determined?