7 Equilibria and the Le Chatelier’s principle can MS 0.3: Students 9.3 chemical industry be used to predict the estimate the effect of Describe industrial reactions which are in effects of changes in changing experimental Recap ideas about the dynamic equilibrium temperature, pressure and parameters on a Haber Process and Use Le Châtelier’s principle to predict what the concentration on the measurable value, e.g. introduce the optimum conditions for the reactions are likely position of equilibrium in how the value of Kc manufacture of ethyl to be homogeneous reactions. would change with butanoate and nitric acid Explain why compromises in temperature and temperature, given A catalyst does not affect as industrial reactions in pressure need to be made. different specified the position of dynamic equilibrium. conditions. equilibrium. Analyse these reactions to determine the Students should be able MS 1.1: Students report optimum conditions for to: use Le Chatelier’s calculations to an product yield and principle to predict appropriate number of compare to the actual qualitatively the effect of significant figures, given reaction conditions changes in temperature, raw data quoted to pressure and varying numbers of concentration on the significant figures. position of equilibrium; Students understand explain why for a that calculated results reversible reaction used in can only be reported to an industrial process, a the limits of the least compromise temperature accurate measurement. and pressure may be used. MS 2.2 and 2.3: Students calculate: the concentration of a 3.1.6.2 Equilibrium reagent at equilibrium; constant for Kc the value of an homogeneous systems equilibrium constant Kc The equilibrium constant PS 2.3: Students could Kc is deduced from the determine the equation for a reversible equilibrium constant, Kc, reaction. The for the reaction of concentration, in mol ethanol with ethanoic of a species X involved acid in the presence of a
Le Chatelier’s principle can be used to predict the effects of changes in temperature, pressure and concentration on the position of equilibrium in homogeneous reactions. A catalyst does not affect the position of equilibrium. Students should be able to: use Le Chatelier’s principle to predict qualitatively the effect of changes in temperature, pressure and concentration on the position of equilibrium; explain why for a reversible reaction used in an industrial process, a compromise temperature and pressure may be used. 3.1.6.2 Equilibrium constant Kc for homogeneous systems The equilibrium constant Kc is deduced from the equation for a reversible reaction. The concentration, in mol of a species X involved MS 0.3: Students estimate the effect of changing experimental parameters on a measurable value, e.g. how the value of Kc would change with temperature, given different specified conditions. MS 1.1: Students report calculations to an appropriate number of significant figures, given raw data quoted to varying numbers of significant figures. Students understand that calculated results can only be reported to the limits of the least accurate measurement. MS 2.2 and 2.3: Students calculate: the concentration of a reagent at equilibrium; the value of an equilibrium constant Kc PS 2.3: Students could determine the equilibrium constant, Kc, for the reaction of ethanol with ethanoic acid in the presence of a 7 Equilibria and the chemical industry Recap ideas about the Haber Process and introduce the manufacture of ethyl butanoate and nitric acid as industrial reactions in dynamic equilibrium. Analyse these reactions to determine the optimum conditions for product yield and compare to the actual reaction conditions Describe industrial reactions which are in dynamic equilibrium Use Le Châtelier’s principle to predict what the optimum conditions for the reactions are likely to be Explain why compromises in temperature and pressure need to be made. 9.3
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