Unit 1: Reaction Kinetics – Learning Standards

Use the following learning outcomes to keep tract of your understanding of Reaction Kinetics:


  • A:     REACTION KINETICS (Introduction)
  • A1.      give examples of reactions proceeding at different rates
  • A2.      describe rate in terms of some quantity (produced or consumed) per unit of time
  • A3.      experimentally determine rate of a reaction
  • A4.      identify properties that could be monitored in order to determine a reaction rate
  • A5.      recognize some of the factors that control reaction rates
  • A6.      compare and contrast factors affecting the rates of both homogeneous and heterogeneous reactions
  • A7.      discuss situations in which the rate of reaction must be controlled
  • B:     REACTION KINETICS (Collision Theory)
  • B1.      demonstrate an awareness of the following:     
  • •            reactions are the result of collisions between reactant particles
  • •            not all collisions are successful
  • •            sufficient kinetic energy (KE) and favourable geometry are required
  • •            to increase the rate of a reaction one must increase the frequency of successful collisions
  • •            energy changes are involved in reactions as bonds are broken and formed
  • B2.      describe the activated complex in terms of its potential energy (PE), stability and structure
  • B3.      define activation energy
  • B4.      describe the relationship between activation energy and rate of reaction
  • B5.      describe the changes in KE and PE as reactant molecules approach each other
  • B6.      draw and label PE diagrams for both exothermic and endothermic reactions, including ∆H, activation energy and the energy of the activated complex
  • B7.      relate the sign of ∆H to whether the reaction is exothermic or endothermic
  • B8.      write a chemical equation including the energy term (given a ∆H value)and vice versa
  • B9.      describe the role of the following factors in reaction rate:     
  • •            nature of reactants
  • •            concentration
  • •            temperature
  • •            surface area
  • C:     REACTION KINETICS (Reaction Mechanisms and Catalysts)
  • C1.      use examples to demonstrate that most reactions involve more than one step
  • C2.      describe a reaction mechanism as the series of steps (collisions) that result in the overall reaction
  • C3.      define catalyst
  • C4.      compare and contrast the PE diagrams for a catalyzed and uncatalyzed reaction in terms of:
  • •            reaction mechanism
  • •            ∆H
  • •            activation energy
  • C5.      identify reactant, product, reaction intermediate and catalyst from a given reaction mechanism
  • C6.      describe the uses of specific catalysts in a variety of situations

Leave a Reply

Fill in your details below or click an icon to log in:

WordPress.com Logo

You are commenting using your WordPress.com account. Log Out /  Change )

Google photo

You are commenting using your Google account. Log Out /  Change )

Twitter picture

You are commenting using your Twitter account. Log Out /  Change )

Facebook photo

You are commenting using your Facebook account. Log Out /  Change )

Connecting to %s