Equilibria - A Level Chemistry

OCR H432 · 3.2.3 · 5.1.2

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3.2.3(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 3.2.3(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 3.2.3(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 3.2.3(d) the techniques and procedures used to investigate changes to the position of equilibrium for changes in concentration and temperature. 3.2.3(e) explanation of the importance to the chemical industry of a compromise between chemical equilibrium and reaction rate in deciding the operational conditions 3.2.3(f) expressions for the equilibrium constant, K_c, for homogeneous reactions and calculations of the equilibrium constant, K_c, from provided equilibrium concentrations 3.2.3(g) estimation of the position of equilibrium from the magnitude of K_c. 5.1.2(a) use of the terms mole fraction and partial pressure 5.1.2(b) calculation of quantities present at equilibrium, given appropriate data 5.1.2(c) the techniques and procedures used to determine quantities present at equilibrium 5.1.2(d) expressions for K_c and K_p for homogeneous and heterogeneous equilibria (see also 3.2.3 f) 5.1.2(e) calculations of K_c and K_p, or related quantities, including determination of units (see also 3.2.3 f) 5.1.2(f) (i) the qualitative effect on equilibrium constants of changing temperature for exothermic and endothermic reactions
(ii) the constancy of equilibrium constants with changes in concentration, pressure or in the presence of a catalyst 5.1.2(g) explanation of how an equilibrium constant controls the position of equilibrium on changing concentration, pressure and temperature 5.1.2(h) application of the above principles in 5.1.2 How far? for K_c, K_p to other equilibrium constants, where appropriate (see also 5.1.3 c etc.).

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