Copyright Information: Penner, Reginald Thermodynamics and Chemical Dynamics 131C (UCI OpenCourseWare: University of California, Irvine), http://ocw.uci.edu/courses/chem_131c_thermodynamics_and_chem... [January 28, 2015]. License: Creative Commons Attribution-ShareAlike 3.0 United States License. (http://creativecommons.org/licenses/by-sa/3.0/us/deed.en_US).
Slide Information 00:09 - Introduction: Integrated Law 00:18 - today... 00:41 - Two types of reactions: take for example the following: 02:19 - stoichiometric 03:12 - for elementary reactions... 04:09 - this is another bimolecular reaction 07:14 - How do we experimentally determine the rate law? 17:48 - Method 3 - Use the integrated rate law to define the half-life of the reaction. 20:30 - vs time for a 2nd order reaction... 21:10 - Method 2: Use an integrated rate law. 21:56 - we've mentioned 1st order and 2nd order reactions...zero order reaction. 23:15 - [A] vs time for a 0 order reaction 23:56 - what kind of reaction does this? 24:36 - the microscopic view of "heterogeneous" catalysis 26:00 - some common integrated rate laws. 27:06 - so in reality, we have three methods for classifying a reaction... 28:30 - Method 3. Measuring the influence of initial reactant concentration... 29:08 - example: what % will decompose after one hour? 30:34 - For reversible reactions, we mentioned... 31:34 - Let's start with the simplest reversible reaction
In Chemistry 131C, students will study how to calculate macroscopic chemical properties of systems. This course will build on the microscopic understanding (Chemical Physics) to reinforce and expand your understanding of the basic thermo-chemistry concepts from General Chemistry (Physical Chemistry.) We then go on to study how chemical reaction rates are measured and calculated from molecular properties. Topics covered include: Energy, entropy, and the thermodynamic potentials; Chemical equilibrium; and Chemical kinetics.
Chemistry Dept. | Physical Sciences Sch. | University of California, Irvine