1. CHEM 433 – 12/2/11 IX. Chemical Kinetics (Handout forthcoming) Context: Where are we now? Reaction Rates Rate Laws (22.2) Determining Rate Laws (22.1, 22.3) - Method of Initial Rates - HW 11 – ALL REC out M. - Final calendar, i.e. when is EXAM #5, etc. – by e-mail on Monday. (It will cover thru T lecture).

2. Where are we now? 4 questions for CHEM 433: What concept/topic provides the answers? 1)What (reactions) can happen? 2)What (reactions) do happen? 3)How far do they go? 4)How Fast ?

3. A comment about transport properties*: * Ability to transfer matter or energy to a new location. Diffusion: Transport of matter along a concentration gradient. Thermal Conduction: Transport of heat along a temperature gradient. Electric Conduction: Migration of charge along a potential gradient (aka “voltage”). Viscosity: Migration of linear momentum along a velocity gradient. (huh?)

4. To measure rate you must Monitor Concentration? How? -Spectroscopy (e.g. UV/VIS) - (in 438) -Pressure measurements (gas phase only) -GC (slow reactions only) -Indicators/competing reactions (CHEM 104/115)

5. 1.Consider the following reaction, and the table of (initial) rate data: H 2 O (g) + SO 3 (g)  H 2 SO 4 (g). a) Write rate law in the blank below. RATE = __________________________ b) Calculate the value of the rate constant, w/ the proper units. c) Does the reaction occur as written, in a single elementary step? Explain. [H 2 O][SO 3 ]Rate 0.01 M 1.0 x 10 4 M/sec 0.02 M0.01 M4.0 x 10 4 M/sec 0.01 M0.02 M2.0 x 10 4 M/sec

6. Show that for: RATE = k [A] 2 A plot of 1/[A] vs. t will be linear, w/ a slope = k. Also show that the half-life is given by: t 1/2 = 1 / k[A 0 ]