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a) Reaction rates
(i) Following the course of a reaction
Reactions can be followed by measuring changes in concentration, mass and volume of reactants and products.
The average rate of a reaction, or stage in a reaction, can be calculated from initial and
final quantities and the time interval.
The rate of a reaction, or stage in a reaction, is proportional to the reciprocal of the time taken.
(ii) Factors affecting rate
The rates of reactions are affected by changes in concentration, particle size and
temperature.
The collision theory can be used to explain the effects of concentration and surface area on reaction rates.
Temperature is a measure of the average kinetic energy of the particles of a substance.
The activation energy is the minimum kinetic energy required by colliding particles
before reaction will occur.
(iii) The idea of excess
The reactant that is in excess can be calculated.
(iv) Catalysts
Catalysts can be classified as either heterogeneous or homogeneous.
Catalysts are used in many industrial processes.
Heterogeneous catalysts work by the adsorption of reactant molecules.
b) Enthalpy
(i) Potential energy diagrams
Exothermic changes cause heat to be released to the surroundings; endothermic changes cause absorption of heat from the surroundings.
A potential energy diagram can be used to show the energy pathway for a reaction.
(ii) Enthalpy changes
The enthalpy of combustion of a substance is the enthalpy change when one mole of the substance burns completely in oxygen.
The enthalpy of solution of a substance is the enthalpy change when one mole of the
substance dissolves in water.

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