Chem 211 1st Edition Lecture 12 Outline of Last Lecture I. Determining Reaction OrdersOutline of Current Lecture I. Determine the kinetic parameters of a reactionII. Integrated Rate LawsIII. Reaction Half-lifeIV. Half-life EquationsCurrent LectureI. Determine the kinetic parameters of a reactionA. Determine slope of tangent at t0 for each plot.B. Compare initial rates when [A] changes and [B] is held constant (andvice versa).C. Substitute initial rates, orders, and concentrations into rate = k[A]m[B]n, and solve for k.II. Integrated Rate LawsA. An integrated rate law includes time as a variable.B. First-order rate equationa) A plot of ln [A] vs. time gives a straight line for a first-order reaction.C. Second-order rate equationb) A plot of 1/[A] vs. time gives a straight line for a second-order reaction.D. Zero-order rate equationThese 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.c) A plot of [A] vs. time gives a straight line for a first-order reactionE. The concentration data is used to construct three different plots. Since the plot of ln [N2O5] vs. time gives a straight line, the reaction is first order.III. Reaction Half-lifeA. The half-life (t1/2) for a reaction is the time taken for the concentration of a reactant to drop to half its initial value.B. For a first-order reaction, t1/2 does not depend on the starting concentration.C. The half-life for a first-order reaction is a constant.D. Radioactive decay is a first-order process. The half-life for a radioactive nucleus is a useful indicator of its stability.IV. Half-life
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