Physical chemistry - 8. Reaction kinetics


I - Simple rate equations; orders of reaction; rate constants

II - Effect of temperature on rate constants; the concept of activation energy

III - Homogeneous and heterogeneous catalysis

Learning outcomes

Candidates should be able to:

(a) explain and use the terms: rate of reaction, activation energy, catalysis, rate equation, order of reaction, rate constant, half-life of a reaction, rate-determining step

(b) *explain qualitatively, in terms of collisions, the effect of concentration changes on the rate of a reaction

(c) *show understanding, including reference to the Boltzmann distribution, of what is meant by the term activation energy

(d) *explain qualitatively, in terms both of the Boltzmann distribution and of collision frequency, the effect of temperature change on the rate of a reaction

(e)* Catalysts

(f) describe enzymes as biological catalysts (proteins) which may have specific activity

(g) 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:

(h) Reaction order

(i) calculate a rate constant using the initial rates method

(j) devise a suitable experimental technique for studying the rate of a reaction, from given information

(k) outline the different modes of action of homogeneous and heterogeneous catalysis, including:

(iv) catalytic role of Fe3+ in the I–/S2O82– reaction