Notes taken during lecture

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31 Dec 2010
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NB. 201LM – lab prep on Wednesday 12 - 2
LECTURE 7 – Kinetics
Slide No. Notes
1-how much product is formed
-how much reactant disappears
-2) actual ratio of reactant to product once reaction appears to stop
-3)
2-nothing to do with energy – kinetics
-spontaneous because of thermodynamics
-kinetics deals with how long it takes
3-atmospheric chemistry – ozone depletion
-biochemistry – medicines
-archaeology – carbon dating
-the more we understand of kinetics, more control over processes
industrial reactions preferred to be fast – also slow down food
decomposition, aging
4-more concentrated, more likely to collide earlier
-more surface area, faster/more vigorous reaction
-temperature
5-red line = conc of A decreasing; green line – B conc increasing
-disappearance of reactant or appearance of B
-note negative sign
6- need to take into consideration coefficients
7-Ans: B
-Ans2: D
8-note negative sign in average rate equation
9-these are instantaneous rates
-note that all three are same values
-rate of reaction should be same for all reactants and products
-do not matter which product or reactant examined, as long as
coefficients taken into consideration
-LATER on, slope smaller, so reaction slows down
10 -how rate changes with concentration
-capitals are species of reaction; non-capitals are coefficients
-double rate of N2O5, double rate of reaction – rate is proportional to
concentration
-exponent = order of reaction
-
11 -overall reaction order = sum of all exponents
-Ans1: C
-EX2.
-double conc of A = increasing rate of reaction by four
www.notesolution.com
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Document Summary

201lm lab prep on wednesday 12 - 2. More concentrated, more likely to collide earlier. More surface area, faster/more vigorous reaction temperature red line = conc of a decreasing; green line b conc increasing disappearance of reactant or appearance of b note negative sign. Ex2. double conc of a = increasing rate of reaction by four www. notesolution. com. Halve conc of b = halve rate of reaction. Therefore ans2: c vary the initial concentration of one reactant at a time set of experiments to measure rate and pick it apart by seeing how it is affected by different reactant concentrations. Initially, there is no back reaction -> no products, so products cannot produce reactants and mess up concentrations compare 1 and 2: clo2 differs, so the difference between the experiments" initial rates is due to the clo2. Clo2 first order: both initial conc and initial rate increase by 4, therefore one-to-one therefore ans1: b.

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