Syllabus
Topic 6: Kinetics (5 hours)
6.1 Rates of reaction --- 2 hours
6.1.1
Define the term rate of reaction.
6.1.2
Describe suitable experimental procedures for measuring rates of reactions.
Aim 7: Data loggers can be used to collect data and produce graphs.
6.1.3
Analyze data from rate experiments.
Students should be familiar with graphs of changes in concentration, volume and mass against time.
6.2 Collision theory --- 3 hours
6.2.1
Describe the kinetic theory in terms of the movement of particles whose average energy is proportional to temperature in Kelvins
6.2.2
Define the term activation energy, Ea.
6.2.3
Describe the collision theory.
Students should know that reaction rate depends on:
· collision frequency
· number of particles with E ≥ Ea
· appropriate collision geometry or orientation.
6.2.4
Predict and explain, using the collision theory, the qualitative effects of particle size, temperature, concentration and pressure on the rate of a reaction.
Aim 7: Interactive simulations can be used to demonstrate this.
6.2.5
Sketch and explain qualitatively the Maxwell–Boltzmann energy distribution curve for a fixed amount of gas at different temperatures and its consequences for changes in reaction rate.
Students should be able to explain why the area under the curve is constant and does not change with temperature.
aim 7: Interactive simulations can be used to demonstrate this.
6.2.6
Describe the effect of a catalyst on a chemical reaction.
6.2.7
Sketch and explain Maxwell–Boltzmann curves for reactions with and without catalysts.
Topic 16: Kinetics (6 hours)
16.1 Rate expression --- 3 hours
16.1.1
Distinguish between the terms rate constant, overall order of reaction and order of reaction with respect to a particular reactant.
16.1.2
Deduce the rate expression for a reaction from experimental data.
Aim 7: Virtual experiments can be used here.
16.1.3
Solve problems involving the rate expression.
6.1.4
Sketch, identify and analyze graphical representations for zero-, first- and second-order reactions.
Students should be familiar with both concentration–time and rate–concentration graphs.
16.2 Reaction mechanism --- 1 hour
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).
16.2.2
Describe the relationship between reaction mechanism, order of reaction and rate-determining step.
Only examples with one- or two-step reactions where the mechanism is given will be assessed.
16.3 Activation energy --- 2 hours
16.3.1
Describe qualitatively the relationship between the rate constant (k) and temperature (T).
16.3.2
Determine activation energy (Ea) values from the Arrhenius equation by a graphical method.
The Arrhenius equation and its logarithmic form are provided in the Chemistry data booklet. The use of simultaneous equations will not be assessed.
