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KU CHEM 135 - Rate law and reaction order
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CHEM 135 1st Edition Lecture 12Current Lecture Outline:I. Rate vs. reaction concentrationII. Complex rate law and reaction ordera. Overall reaction orderb. ExamplesIII. Integrated Rate LawRate vs. reaction concentration When placed in a graph format:- Zero order reaction has a straight horizontal line- First order reaction has a straight increasing slope- Second order reaction has an arched increasing slopeComplex rate law and reaction orderaA + bB  cC + dDRate=k[A]m[B]nk= rate constantm & n= reaction order with respect to A & BOverall reaction order = (m + n)Ex: N2 + 3H2  2NH3Reaction order with respect to N2 is first orderThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.Reaction order with respect to H2 is second orderRate law: Rate= k[N2]1[H2]2Overall order=3Ex: This reaction was experimentally determined to be first order with respect to O2 and second order with respect to NO.O2 + 2NO  2NO2Rate= K[O2]1[NO]2Overall order= 3Ex: 2NO2 + F2  2FNO2[NO2] (M) F2 (M) Initial rate of loss of NO2 (M/s)0.100 0.100 0.0260.200 0.100 0.0510.200 0.200 0.1030.400 0.400 0.411a) What is the order with respect to NO2? With respect to F2?NO2 = first orderF2= first orderb) Rate law?Rate= k[N2]1[F2]1c) Overall reaction order?2d) Value of the rate constant>K=2.6M-1s-1e) What would the rate be if [NO2]= .05M and [F2]=.075M?Rate= 2.6[.05][.075]Rate=9.75 x 10-3 M/sIntegrated Rate Law- Shows relationship between time and concentrationln[ A


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KU CHEM 135 - Rate law and reaction order

Type: Lecture Note
Pages: 3
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