the terms:

(i) rate of reaction
(ii) rate constant, including units
(iii) order of reaction (both overall and with respect to a given reagent), use of ‘∝’
(iv) rate equations of the form: \(\text{rate} = k[A]^m[ B]^n\) where \(m\) and \(n\) are integers;

calculations based on the rate equation;
the rate constant \(k\) increasing with increasing temperature

the use of given data to calculate half-lives for a reaction

techniques and procedures for experiments in reaction kinetics;
use of experimental data [graphical methods (including rates from tangents of curves), half-lives or initial rates when varying concentrations are used] to find the rate of reaction, order of a reaction (zero-, first- or second-order), rate constant and construction of a rate equation for the reaction

the Arrhenius equation and the determination of E_a and A for a reaction, given data on the rate constants at different temperatures

The Arrhenius equation is given on the Data Sheet.

the term rate-determining step;
relation between rate-determining step and the orders and possible mechanism for a reaction

the effect of changes of temperature and pressure (if any) on the magnitude of the equilibrium constant;
the fact that addition of catalysts has no effect on the position of equilibrium or the magnitude of the equilibrium constant

the determination of the most economical operating conditions for an industrial process using principles of equilibrium and rates of reaction

Data for the industrial process will be given.

calculations, including units, involving K_c and initial and equilibrium concentrations for homogeneous equilibria;
techniques and procedures for experiments to determine equilibrium constants

the chemical reactions occurring during industrial processes

Learners should be able to use given information, no recall is required.

the following aspects of nitrogen chemistry:

(i) bonding in nitrogen gas, ammonia and the ammonium ion
(ii) the appearance and names of the oxides of nitrogen, N₂O, NO, NO₂
(iii) interconversion of the nitrate(V) ion, nitrate(III) ion, ammonium ion, oxides of nitrogen
(iv) tests for nitrate(V) and ammonium ions

Test for nitrate(V): warm with Devarda’s alloy and NaOH.
Test for ammonium: warm with NaOH.
In both cases, ammonia is evolved.

given examples of industrial processes:

(i) costs of raw materials, energy costs, costs associated with plant, co-products and by-products
(ii) the benefits and risks associated with the process in terms of benefits to society of the product(s) and hazards involved.

Learners will be expected to analyse and use given information.