#3.2.3a
explanation that a dynamic equilibrium exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction and the concentrations of reactants and products do not change
#3.2.3b
le Chatelier’s principle and its application for homogeneous equilibria to deduce qualitatively the effect of a change in temperature, pressure or concentration on the position of equilibrium
Definition for le Chatelier's principle not required.
#3.2.3c
explanation that a catalyst increases the rate of both forward and reverse reactions in an equilibrium by the same amount resulting in an unchanged position of equilibrium
#3.2.3d
the techniques and procedures used to investigate changes to the position of equilibrium for changes in concentration and temperature.
Qualitative effects only.
#3.2.3e
explanation of the importance to the chemical industry of a compromise between chemical equilibrium and reaction rate in deciding the operational conditions
#3.2.3f
expressions for the equilibrium constant, Kc , for homogeneous reactions and calculations of the equilibrium constant, Kc , from provided equilibrium concentrations
Learners will not need to determine the units for Kc.
#3.2.3g
estimation of the position of equilibrium from the magnitude of Kc.
A qualitative estimation only is required.