Week 1 Notes
Week 1 Notes Chem 122A
Popular in Gen Chemistry 2
Popular in Chemistry
This 2 page Class Notes was uploaded by Josilynn Stokes on Tuesday September 6, 2016. The Class Notes belongs to Chem 122A at University of Nevada - Las Vegas taught by Marykay Orgill in Fall 2016. Since its upload, it has received 87 views. For similar materials see Gen Chemistry 2 in Chemistry at University of Nevada - Las Vegas.
Reviews for Week 1 Notes
Report this Material
What is Karma?
Karma is the currency of StudySoup.
You can buy or earn more Karma at anytime and redeem it for class notes, study guides, flashcards, and more!
Date Created: 09/06/16
Chapter 14: Chemical Kinetics Kinetics is the study of reaction rates and how much of the concentration of the product changes with time Products concentration tends to increase while Reactants concentration tends to increase Concentration is shown with “” Collision theory Reactant particles must collide Reactant must come into contact in the proper orientation (has to be lined up the right way) Reactants must have a sufficient amount of energy to react Surface Area and the effect on reaction rate Ex. If there was an iron nail in a bottle of oxygen the reaction would occur slowly because it is only reacting with the outer layer of molecules. If the iron nail was replaced with iron wool the reaction rate is higher because there is more molecules throughout the wool. Orientation and the effect on reaction rates The second part of the collision theory says that molecules have to be in the right orientation to react There are certain enzymes that aid in this process. Enzymes hold the molecule in a certain orientation so that other molecules can collide and react. Energy and the effect on reaction rate Higher temperature increases the energy the molecule has. The higher the energy the faster the molecule moves. The faster the molecule moves the higher chance of a collision. Higher chance of collision means there is a higher chance of having an effective collision. Rate is how much a quantity changes in a given time period Over time a reaction rate typically slows. This is because the amount of reactant decreases over time. When the amount of reactant decreases, the probability of a proper collision will decrease. Thus, having a decreased probability of an effective collision. Reaction order: the bigger the order of reaction the more reactant effects the rate (this comes from the experiment) th 0 order= [A] vs. time 1 order= ln[A] vs. time 2 order= 1/[A] vs. time
Are you sure you want to buy this material for
You're already Subscribed!
Looks like you've already subscribed to StudySoup, you won't need to purchase another subscription to get this material. To access this material simply click 'View Full Document'