Friday, January 29, 2010
Fri-Day 2
Bio - we discussed the circulatory/respiratory system activity that we performed on Thursday. We particularly focused on the changes in blood composition that occur in the lungs and around body tissues due to diffusion of O2 and CO2 in and out of the capillaries at these locations.
We also discussed the threat to homeostasis that occurs when a person is bleeding internally or externally and how the body deals with this threat.
AP Chem - we saw how the "order"/molecularity of a reaction, for each reactant, is calculated using the graphs from kinetics data. We can then write the correct "experimentally determined" RATE LAW for that reaction and also determine the RATE CONSTANT for that reaction at a particular temperature.
We carefully noted the UNITS of the rate constant for EACH or 0th, 1st, 2nd, and even 3rd order reactions.
We then related the experimentally determined rate law to the actual number of molecules that are colliding in the RATE DETERMINING (slow) step of a reaction.
We saw how to propose a reaction MECHANISM that is CONSISTENT with an experimentally determined rate law for a given reaction. The mechanism must have a slow/rate determining step that yields the same rate law as that determined experimentally, AND also the mechanism's elementary steps MUST add up to the NET reaction.
We then saw how, when a mechanism has a fast equilibrium step, followed by a slow step, we may have to substitute for the intermediate formed to see whether a rate law is actually consistent with the experimentally determined rate law.
We also discussed the threat to homeostasis that occurs when a person is bleeding internally or externally and how the body deals with this threat.
AP Chem - we saw how the "order"/molecularity of a reaction, for each reactant, is calculated using the graphs from kinetics data. We can then write the correct "experimentally determined" RATE LAW for that reaction and also determine the RATE CONSTANT for that reaction at a particular temperature.
We carefully noted the UNITS of the rate constant for EACH or 0th, 1st, 2nd, and even 3rd order reactions.
We then related the experimentally determined rate law to the actual number of molecules that are colliding in the RATE DETERMINING (slow) step of a reaction.
We saw how to propose a reaction MECHANISM that is CONSISTENT with an experimentally determined rate law for a given reaction. The mechanism must have a slow/rate determining step that yields the same rate law as that determined experimentally, AND also the mechanism's elementary steps MUST add up to the NET reaction.
We then saw how, when a mechanism has a fast equilibrium step, followed by a slow step, we may have to substitute for the intermediate formed to see whether a rate law is actually consistent with the experimentally determined rate law.
# posted by C @ 11:21 PM 
