16.1.1

Distinguish between the terms rate constant, overall order of reaction and order of reaction with respect to a particular reactant.

2

16.1.2

Deduce the rate expression for a reaction from experimental data.

3

Aim 7: Virtual experiments can be used here.

16.1.3

Solve problems involving the rate expression.

3

16.1.4

Sketch, identify and analyse graphical representations for zero-, first- and second-order reactions.

3

Students should be familiar with both concentration–time and rate–concentration graphs.

16.2.1

Explain that reactions can occur by more than one step and that the slowest step determines the rate of reaction (rate-determining step).

3

16.2.2

Describe the relationship between reaction mechanism, order of reaction and rate-determining step.

2

Only examples with one- or two-step reactions where the mechanism is given will be assessed.

TOK: Agreement between rate equation and a suggested mechanism only provides evidence to support a reaction mechanism. Disagreement disproves the mechanism.

16.3.1

Describe qualitatively the relationship between the rate constant (k) and temperature (T).

2

16.3.2

Determine activation energy (Ea) values from the Arrhenius equation by a graphical method.

3

The Arrhenius equation and its logarithmic form are provided in the Chemistry data booklet. The use of simultaneous equations will not be assessed.