CHEM 1120 1st Edition Lecture 6Outline of last lecture1. Chemical kinetics2. Factors that affect reaction rates3. Types of rates measured4. Average rates and plotting data, gathering information from plotted data5. Concentration and Rate LawsOutline of Current Lecture 1. Finish up last lectures 14.3 2. Change of concentration with time3. First order reactions4. Second order reactions5. Zeroth order reactionsCurrent LectureChapter 14-Chemical Kinetics Continued- Strategy for Determining Rate Law using initial rateso Rate laws must be determined experimentallyo Method of initial rates Determines reaction orders from the effect of changing a reactants concentration on initial rate of reactionThese 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.o Rate = k[A]m[B]n  Our strategy is to systematically vary the concentrations of A and Bo ***Refer to slides 28-31 on the Chapter 14 Powerpoint for examples and detailedexplanations on this strategy***14.4 The change of concentration with time- concentration and time equations are derived using calculus - resulting equations depend on rate law used called integrated rate lawso First order reaction: Integrated rate law: (next page)Variables: - Logarithm review***Refer to slides 34 through 38 and on Chapter 14 Powerpoint for detailed explanations on two example problems for first-order reactions…as well as picture detailed explanations how to determine reaction order and rate constant (k) ***o Second order reactions 1/[A]t= k t + 1/[A]o- same structure as y=mx+b On a graph, if linear it will be 2nd order reactiono Zeroth-Order Rate Law [A]t = -kt + [A]o or, y=mx+b- Summary of first, second, and zeroth reaction order and ratesZero order First order Second orderRate law Rate=k Rate=k[A] Rate=k[A]Units for k mol/L*s 1/s L/mol*sIntegrated rate law in straight-line formA]t =-kt + [A] ln[A]t =-k t + ln[A]0 1/[A]t =k t + 1/[A]0 Plot for straight line[A]t vs. t ln[A]t vs. t 1/[A]t vs. t Slope, y-intercept-k, [A]0 k, ln[A]0 k, 1/[A]0 Half-life[A]0/2k ln 2/k 1/k