The qualitative effect of Students plot graphs of results from changes in other continuous monitoring concentration and experiments, and interpret the data. pressure on collision frequency. 3.1.5.5 0.4 Use a Maxwell–Boltzmann Practical activity: Reaction between June 2012 Hydrogen peroxide and tartrate Catalysts. weeks distribution to help explain hydrogen peroxide and tartrate ions Unit 2 Q1 ions catalysed by Co(II) ions. how a catalyst increases catalysed by Co(II) ions. Define catalyst. the rate of a reaction June 2011 involving a gas. Unit 2 Q1 Catalysts work by providing an alternative January 2003 reaction route of lower Unit 2 Q3 activation energy. January 2011 Unit 2 Q2b 3.1.6.1 0.6 Use Le Chatelier’s principle Practical activity: The effect of June 2013 Ammonia production Chemical equilibria and weeks to predict qualitatively the concentration and temperature Unit 2 Q10a Le Chatelier’s principle. effect of changes in changes on the equilibrium temperature, pressure and between [Co(H2O)6] 2+ and June 2013 Equilibrium between CoCl42-and Know that at equilibrium concentration on the CoCl42- Unit 2 Q1a [Co(H2O)6 ]2+ the forward and reverse position of equilibrium. reactions proceed at Students predict and explain the January 2013 equal rates and the Explain why, for a effect of changes in temperature, Unit 2 Q2 concentrations of reversible reaction used in pressure and concentration on the reactants and products an industrial process, a position of an equilibrium. January 2012 remain constant. compromise temperature Unit 2 Q2 and pressure may be used. Students explain the use of State Le Chatelier’s compromise conditions in a of principle. industrial processes
The qualitative effect of changes in concentration and pressure on collision frequency. Students plot graphs of results from other continuous monitoring experiments, and interpret the data. 3.1.5.5 Catalysts. Define catalyst. Catalysts work by providing an alternative reaction route of lower activation energy. 0.4 weeks Use a Maxwell–Boltzmann distribution to help explain how a catalyst increases the rate of a reaction involving a gas. Practical activity: Reaction between hydrogen peroxide and tartrate ions catalysed by Co(II) ions. June 2012 Unit 2 Q1 June 2011 Unit 2 Q1 January 2003 Unit 2 Q3 January 2011 Unit 2 Q2b Hydrogen peroxide and tartrate ions catalysed by Co(II) ions. 3.1.6.1 Chemical equilibria and Le Chatelier’s principle. Know that at equilibrium the forward and reverse reactions proceed at equal rates and the concentrations of reactants and products remain constant. State Le Chatelier’s principle. 0.6 weeks 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. Practical activity: The effect of concentration and temperature changes on the equilibrium between [Co(H2O)6] 2+ and CoCl42- Students predict and explain the effect of changes in temperature, pressure and concentration on the position of an equilibrium. Students explain the use of compromise conditions in a of industrial processes June 2013 Unit 2 Q10a June 2013 Unit 2 Q1a January 2013 Unit 2 Q2 January 2012 Unit 2 Q2 Ammonia production Equilibrium between CoCl42-and [Co(H2O)6 ]2+
AQA-7404-B-SOW.DOCX