Unit 14: Chemical Kinetics: How fast does a reaction occur
Reading
BJU Chemistry: Ch. 14 "Chemical Kinetics"
AP Classroom: Unit 5 "Kinetics"
AP Princeton Review: Unit 5
Topics
Labs
The Chemistry of NASCAR assignment
Instructions below
BJU Chemistry: Ch. 14 "Chemical Kinetics"
AP Classroom: Unit 5 "Kinetics"
AP Princeton Review: Unit 5
Topics
- Energy diagrams, activation energy
- Factors that affect reaction rates
- Using the rate formula
Labs
- New 2024: Nickel electroplating lab is a perfect illustration of Chemical Kinetics and Equilibrium concepts. We will prepare our own nickel salt from pure nickel metal, build our own electrochemical plating cell, and plate various objects with bright-nickel. This will take two lab sessions. Handouts will be provided when we get here.
- Reactions and Rates weblab - handout below
The Chemistry of NASCAR assignment
Instructions below
Below: Placing a gummy bear in potassium chlorate illustrates fast reaction kinetics. The candy provides the source of carbon, and the chlorate radical (ClO3 -) provides quick oxygen.
| 14._kinetics_lecture_notes_2022.docx |
Lecture outline
Thermodynamics (our previous topic) answers the question of whether a reaction will go forward or not. If the change in Gibbs Free Energy is negative, the reaction is favorable. However, we didn't discuss how FAST a reaction would occur - it might take years to go forward (the rusting of steel would be an example of a slow chemical reaction).
Kinetics (this topic) addresses the 'how fast' question. If a reaction proceeds at all, how quickly does it do so? A reaction might not have any commercial usefulness if it doesn't take place relatively quickly. Thus, the field of reaction kinetics is very important in any commercial, real-life setting.
Thermodynamics (our previous topic) answers the question of whether a reaction will go forward or not. If the change in Gibbs Free Energy is negative, the reaction is favorable. However, we didn't discuss how FAST a reaction would occur - it might take years to go forward (the rusting of steel would be an example of a slow chemical reaction).
Kinetics (this topic) addresses the 'how fast' question. If a reaction proceeds at all, how quickly does it do so? A reaction might not have any commercial usefulness if it doesn't take place relatively quickly. Thus, the field of reaction kinetics is very important in any commercial, real-life setting.
The concept of spontaneity:
- A reaction might be spontaneous, but proceed at a really slow rate. Example: rusting of iron.
- Thus, spontaneous does not necessarily mean "fast".
- On the other hand, non-spontaneous means a reaction won't go forward at all on its own. A non-spontaneous reaction needs help to get over the activation barrier. This needed "help" might be in the form of a lit match, increasing the temperature of the reactor, increasing the pressure, using a catalyst, and so on.
"Reactions and Rates" weblab
Lab handout with instructions is posted below. Upload your completed work to Canvas. The answer key is here to help you, BUT DO YOUR OWN WORK FIRST!! Then use the answer key to self-check your answers.
Lab handout with instructions is posted below. Upload your completed work to Canvas. The answer key is here to help you, BUT DO YOUR OWN WORK FIRST!! Then use the answer key to self-check your answers.
| reactions_and_rates_weblab__2021_.docx |
| reactions_and_rates_weblab__answer_key_.docx |
"The Chemistry of NASCAR"
This assignment is posted in Canvas in multiple choice format. The handout below is for background information.
This assignment is posted in Canvas in multiple choice format. The handout below is for background information.
| 14._the_chemistry_of_nascar.pdf |