deduce order for a with respect to each of the Enzyme catalysed decomposition reagent. reactants. of H2O2 continuous monitoring by gas collection. That the rate constant Use the orders with respect varies with temperature to reactants to provide Activation energy for as by the equation: information about the thiosulfate/acid reaction. k = Ae-Ea/RT step of a reaction. Know how to use a rearranged Arrhenius equation with experimental data to plot a straight line graph with slope –Ea/R Required practical 7 Measuring the rate of reaction: by an initial rate method by a continuous monitoring method. 1.0 Derive partial pressure from Students use data to calculate mole June 2004 Revision of Starter for 10 3.1.10 Kc: Equilibrium constant Kp weeks mole fraction and total fractions and Kp values for a of Unit 4 Q3 for homogeneous pressure. gaseous reactions. systems. January 2007 Construct an expression for Students predict the qualitative Unit 4 Q2 Know how to calculate Kp for a homogeneous effects of changing temperature partial pressures using system in equilibrium. and pressure on the position of June 2007 mole fractions and total equilibrium and the value of Kp Unit 4 Q1 pressure. Perform calculations involving Kp Practical demonstration: Effect of January 2008 Write expressions for, temperature and pressure on the Unit 4 Q3 and calculate Kp Predict the qualitative NO2/N2O4 equilibrium including units. effects of changes in June 2008 temperature and pressure Unit 4 Q3
deduce order for a reagent. That the rate constant varies with temperature as by the equation: k = Ae-Ea/RT with respect to each of the reactants. Use the orders with respect to reactants to provide information about the step of a reaction. Know how to use a rearranged Arrhenius equation with experimental data to plot a straight line graph with slope –Ea/R Enzyme catalysed decomposition of H2O2 continuous monitoring by gas collection. Activation energy for thiosulfate/acid reaction. Required practical 7 Measuring the rate of reaction: by an initial rate method by a continuous monitoring method. 3.1.10 Equilibrium constant Kp for homogeneous systems. Know how to calculate partial pressures using mole fractions and total pressure. Write expressions for, and calculate Kp including units. 1.0 weeks Derive partial pressure from mole fraction and total pressure. Construct an expression for Kp for a homogeneous system in equilibrium. Perform calculations involving Kp Predict the qualitative effects of changes in temperature and pressure Students use data to calculate mole fractions and Kp values for a of gaseous reactions. Students predict the qualitative effects of changing temperature and pressure on the position of equilibrium and the value of Kp Practical demonstration: Effect of temperature and pressure on the NO2/N2O4 equilibrium June 2004 Unit 4 Q3 January 2007 Unit 4 Q2 June 2007 Unit 4 Q1 January 2008 Unit 4 Q3 June 2008 Unit 4 Q3 Revision of Kc: Starter for 10
AQA-7405-B-SOW.DOCX