1 / 6

Kinetics

Kinetics. Collision Theory: How reactions takes place. Why are kinetics important?. In order to control processes. speed up useful reactions that occur to slowly slow down reactions that are harmful Example:

evangelina
Download Presentation

Kinetics

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Kinetics Collision Theory: How reactions takes place

  2. Why are kinetics important? • In order to control processes. • speed up useful reactions that occur to slowly • slow down reactions that are harmful • Example: • Catalysts are used in our cars to rapidly convert toxic substances into safer substances • Refrigerators are used to slow the process of spoiling in food

  3. Collision Theory • How do reactions occur at the molecular level? • Molecules collide with each other • Form activated complex • Svante Arrhenius • Did some fancy math to figure out that number of collisions alone don’t account for reaction rates • He found that reactants also require: • Activation energy (Ea - energy to break bonds) Animation • Right orientation (Animation)

  4. What affects reaction rate? • Temperature (Animation) • Increased number of collisions • More molecules have enough activation energy • Remember Maxwell-Boltzmann distribution • Increased temperature, distribution flattens out • More molecules have Ea

  5. What affects reaction rate? • Higher concentration • Number of collisions increased • Animation • Animation 2 • Increased surface area • Number of collisions increased • Animation

  6. What affects reaction rate? • Catalysts • Def’n: substance that speeds up a rxn w/o being used up itself • Number of collisions with Ea increase • Ea lowers • Catalysts hold molecules in right orientation • Homogeneous catalyst (same phase of matter) • Demo: Catalysis by Co2+ (demo) • Heterogeneous catalyst (different phase) Animation

More Related