ASRJC H2 Chem 6. Reaction Kinetics

2024 JC1 H2 Reaction Kinetics 2024/ASRJC/Chemistry ANDERSON SERANGOON JUNIOR COLLEGE JC1 H2 CHEMISTRY REACTION KINETICS Content 1 Introduction 2 Expressing the reaction rate 2.1 Average, instantaneous, and initial reaction rates 3 Rate Equation (or Rate Law), Rate Constant & Order of Reaction 3.1 Rate equation or (Rate Law) 3.2 Order of reaction 3.3 Rate constant, k 4 Understanding Order of Reaction 4.1 Zero order reaction 4.2 First order reaction 4.3 Second order reaction 4.4 Pseudo-first order reaction 5 Determination of Rate Equation (or Rate Law) 6 Reaction Mechanism 7 Collision Theory and Factors Affecting Rate of Reaction 8 Catalysis (SDL) 9 Thermodynamic Stability versus Kinetic Stability (SDL)

2024 JC1 H2 Reaction Kinetics 2024/ASRJC/Chemistry Learning Outcomes Students must 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 and 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 (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 an 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, 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 the rate constant (and, hence, on the rate) of a reaction (i) (i) explain that, in the presence of a catalyst, a reaction has a different mechanism, i.e. one of lower activation energy, giving a larger rate constant (ii) interpret this catalytic effect on a rate constant in terms of the Boltzmann distribution (j) outline the different modes of action of homogeneous and heterogeneous catalysis, including: (i) the Haber process (ii) the catalytic removal of oxides of nitrogen in the exhaust gases from car engines (iii) the catalytic role of atmospheric oxides of nitrogen in the oxidation of atmospheric sulfur dioxide (iv) catalytic role of Fe