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
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
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.
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
the techniques and procedures used to investigate changes to the position of equilibrium for changes in concentration and temperature.
Qualitative effects only.
explanation of the importance to the chemical industry of a compromise between chemical equilibrium and reaction rate in deciding the operational conditions
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.
estimation of the position of equilibrium from the magnitude of Kc.
A qualitative estimation only is required.