CEM142 1nd Edition Lecture 2Outline of Last Lecture I. Introduction to chemical kineticsOutline of Current Lecture II. Reaction ordersCurrent Lecture-relationship between concentration and time: as a reaction proceeds, the concentrations of reactants and products change depending on the reaction order-reaction order: values for m and n in the equation learned in last lecture-review: rate = k[reactant 1]m[reactant 2]n-note: [ ] indicates a concentration of the substance within the brackets-integrated rate equations-ln([R]t/[R]0) = -kt from time 0 to t where [R]0 is the concentration at time 0 and [R]t is the concentration at time t-half life: the time taken for the concentration to reduce to one-half of its original value-when [R]t = ½ [R]0Order Rate law Integrated rate law Linear form Half-life Successivehalf-livesLinear plot0 Rate=k [R]=[R]0-kt [R]=[R]0-kt t1/2=[R]0/(2k) Halves [R] vs t slope=-k1 Rate=k[R] [R]=[R]0e-ktln[R]=ln[R]0-kt t1/2=0.693/k Constant ln[R] vs t slope=-k2 Rate=k[R]2[R]=[R]0/(1+[R]0kt) 1/[R]=(1/[R])+kt t1/2=1/(k[R]0) doubles 1/[R] vs t These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a
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