CHAPTER 23: Reaction Kinetics
- Orders of Reaction and Rate Equations
- Reaction Mechanisms
- Catalysis
Learning outcomes:
- explain and use the terms: rate equation, order of reaction, rate constant, half-life of a reaction, rate-determining step
- construct and use rate equations of the form rate = k[A]m[B]ⁿ (limited to simple cases of single step reactions and of multistep processes with a rate-determining step, for which m and n are 0, 1 or 2), including:
i) deducing the order of a reaction from concentration-time graphs, by the initial rates method and half-life methods
ii) deducing, 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 (and vice versa).
- calculating an initial rate using concentration [integrated forms of rate equations are not required]
- (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.
- calculate a rate constant, for example by using the initial rates or half-lifemethod
- devise a suitable experimental technique for studying the rate of a reaction, from given information.
- outline the different modes of action of homogeneous and heterogeneous catalysis, including:
- the Haber process
- the catalytic removal of oxides of nitrogen in the exhaust gases from car engines
- the catalytic role of atmospheric oxides of nitrogen in the oxidation of atmospheric sulfur dioxide.
- catalytic role of Fe³⁺ in the I⁻/S2O8²⁻ reaction.