Chemistry Kinetics

Chemistry Kinetics - #73 Notes Unit 9: Kinetics and...

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chemistrynoteslecture.com LLC © 2011 #73 Notes Unit 9: Kinetics and Equilibrium Ch. Kinetics and Equilibriums I. Reaction Rates NO 2(g) + CO (g) → NO (g) + CO 2(g) Rate is defined in terms of the rate of disappearance of one of the reactants, but it can also be defined by the rate of appearance of one of the products. Rate = - ∆[NO 2 ] = - ∆[CO] = ∆[NO] = ∆[CO 2 ] ∆t ∆t ∆t ∆t - rate can be measured for a specific time (instantaneous rate = slope) or over a time interval (average rate) II. Integrated Rate Laws Rate = k [reactant 1] x [reactant 2] y -x,y are usually integers concentrations (molarity) rate constant, (k), depends on size, speed, kind of molecule, temperature, etc. Ex. 1) A + B → C initial [A] initial [B] initial rate rate = - ∆[B] row 1 0.100 M 0.100 M 4.0 x 10 -5 ∆t row 2 0.100 M 0.200 M 4.0 x 10 -5 row 3 0.200 M 0.100 M 1.6 x 10 -4 = 16 x 10 -5 Compare two rows where only one concentration is changing (only “A” or only “B”). comparing row 1 & 2:
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This note was uploaded on 09/04/2011 for the course CHM 2046 taught by Professor Haces during the Spring '11 term at FAU.

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Chemistry Kinetics - #73 Notes Unit 9: Kinetics and...

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