understand the terms:

i) rate of reaction
ii) rate equation
iii) order with respect to a substance in a rate equation
iv) overall order of reaction
v) rate constant
vi) half-life
vii) rate-determining step
viii) activation energy
ix) heterogeneous and homogenous catalyst

be able to determine and use rate equations of the form:

rate = k[A]^m[ B]ⁿ, where m and n are 0, 1 or 2

be able to select and justify a suitable experimental technique to obtainrate data for a given reaction, including:

i) titration
ii) colorimetry
iii) mass change
iv) volume of gas evolved
v) other suitable technique(s) for a given reaction

understand experiments that can be used to investigate reaction rates by:

i) an initial-rate method, carrying out separate experiments where different initial concentrations of one reagent are used
A ‘clock reaction’ is an acceptable approximation of this method

ii) a continuous monitoring method to generate data to enable concentration-time or volume-time graphs to be plotted

be able to calculate the rate of reaction and the half-life of a first-order reaction using data from a concentration-time or a volume-time graph

be able to deduce the order (0, 1 or 2) with respect to a substance in a rate equation using data from:

i) a concentration-time graph
ii) a rate-concentration graph

be able to deduce the order (0, 1 or 2) with respect to a substance in a rate equation using data from an initial-rate method

understand how to:

i) obtain data to calculate the order with respect to the reactants (and the hydrogen ion) in the acid-catalysed iodination of propanone
ii) use these data to make predictions about species involved in the rate-determining step
iii) deduce a possible mechanism for the reaction

be able to deduce a rate-determining step from a rate equation and vice versa

be able to deduce a reaction mechanism, using knowledge from a rate equation and the stoichiometric equation for a reaction

understand that knowledge of the rate equations for the hydrolysis of halogenoalkanes can be used to provide evidence for S_N1 or S_N2 mechanisms for tertiary and primary halogenoalkane hydrolysis

be able to use graphical methods to find the activation energy for a reaction from experimental data

The Arrhenius equation will be given if needed.

CORE PRACTICAL 13a and 13b: Rates of reaction

Following the rate of the iodine-propanone reaction by a titrimetric method and investigating a ‘clock reaction’ (Harcourt-Esson, iodine clock)

CORE PRACTICAL 14: Finding the activation energy of a reaction