7_Reaction Kinetics

VICTORIA JUNIOR COLLEGE CHEMISTRY DEPARTMENT Dr WU Jiang (wu.jiang@vjc.sg) REACTION KINETICS Lecture 1 2 3 4 5 Pages 3-8 8-14 15-20 20-25 26-31 Completed by T2W6 T2W7 T2W8 T2W9 Tutorial Q Q1 – Q3 Q4, Q5 Q6, Q7 Q8-Q11 Lecture Outline 1 Introduction 2 Concept of Reaction Rate 3 Experimental methods of finding reaction rates 3.1 Titrimetric Analysis 3.2 Colorimetric Analysis 3.3 Volume measurements 3.4 Pressure measurements 3.5 Conductometric measurements 4 The Rate Equation 4.1 The Rate Constant 4.2 The Order of Reaction 4.2.1 Zero order reaction 4.2.2 First order reaction 4.2.3 Second order reaction 4.2.4 Pseudo order reaction 5 Methods to determine order of reaction 5.1 Graphical method / Continuous method 5.2 Initial rate method 6 Theories of reaction rate 6.1 The Collision Theory 6.2 The Transition State Theory 7 Factors affecting rate of reaction 7.1 Concentration 7.2 Temperature 7.3 Light 7.4 Surface area 7.5 Catalysis 8 Reaction Mechanism Reference Texts 1. Chemistry for Advanced Level by Peter Cahn / Hughes 2. Advanced A Level Chemistry by Ramsden 3. Chemistry in Context by Hill & Holman

Victoria Junior College JC1 2021 Reaction Kinetics Page 2 Learning outcomes (9729 H2 Chemistry) Candidates should be able to: (a) explain and use the terms: rate of reaction; rate equation; order of reaction; rate constant; half –life of a reaction; rate–determining step; activation energy; catalysis (b) construct and use rate equations of the form rate = k[A] m[B]n (limited to simple cases of single –step reactions and of multi –step processes with a rate –determining step, for which m an d n are 0, 1 or 2), including: (i) deducing the order of a reaction by the initial rates method (ii) justifying, for zero– and first–order reactions, the order of reaction from concentration–time graphs (iii) verifying that a suggested reaction mechanism is consistent with the observed kinetics (iv) predicting the order that would result from a given reaction mechanism (v) calculating an initial rate using concentration data [integrated forms of rate equations are not required] (c) (i) show understanding that the half–life of a first–order reaction is independent of concentration (ii) use the half–life of a first–order reaction in calculations (d) calculate a rate constant using the initial rates method (e) devise a suitable experimental technique for studying the rate of a reaction, from given information (f) explain qualitatively, in terms of collisions, the effect of concentration changes on the rate of a reaction (g) show understanding, including reference to the Boltzmann distribution, of what is meant by the term activation energy (h) explain qualitatively, in terms both of the Boltzmann distribution and of collision frequency, the effect of temperature change on a rate constant (and hence, on the rate