Dynamic equilibrium and le Chatelier’s principle
(a) 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
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(b) 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
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(c) 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
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(d) the techniques and procedures used to investigate changes to the position of equilibrium for changes in concentration and temperature.
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(e) explanation of the importance to the chemical industry of a compromise between chemical equilibrium and reaction rate in deciding the operational conditions
The equilibrium constant, Kc
(f) expressions for the equilibrium constant, Kc  , for homogeneous reactions and calculations of the equilibrium constant, Kc  , from provided equilibrium concentrations
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(g) estimation of the position of equilibrium from the magnitude of Kc .
