The work have to be with two solutions with concentrations 0,2 and 0,4 mol 1^-1 as 2 different experiments. The procedure : Title: This tells you what is going to be
measured, in this case the order of the reaction, and for which reaction. Note the style 'An experiment to ...) and that this is a title so need not be a sentence. Summary: This should begin by saying what you measured and what you discovered from the measurements. Then briefly conclude by quoting the value of kR from the group results and how this compared with the literature value of kR at 25 oC. Method: As the chemical kinetics experiment uses standard apparatus, you did not need to include this. Describe all the procedures you undertook and what apparatus was used, for example 'A 20 ml pipette was used to transfer ...'. Note that this is written in the passive tense and third person i.e. 'The lid was fitted' not 'I fitted the lid'. Give the quantities of chemicals used for each experiment and how you prepared the solutions. You were asked to comment on aspects of the procedure that reduced errors. You should consider possible sources of error and then identify those that the experiment was designed to minimise or remove. Results and discussion: Give a plausible rate equation for the reaction and show how this is simplified using the isolation method in the experiment. Include a straight-line graph showing how you obtained the partial order for the Pt complex and the value of kR' for [en]0= 0.2 mol 1-1. Insert and complete the table in the TMA question with your results for [en]0 = 0.2 mol 1-1 as well as your tutor group results for the rest of the en concentrations. You should comment on the way you analysed the results, assuming that the partial order is one with respect to en, and calculated values for kR at each en concentration. Finally, you should quote the overall rate equation for the reaction including the average value of kR with its units, from your group results. Conclusion: Give a brief statement of the aims and results of the experiment and compare the value of kR, determined, with the literature value./nTitle - An informative title. What did your group set out to determine through this experiment? (Up to 20 words) Summary - This should include a statement of what experiment was done and the main conclusions. (Up to 150 words). Method - Write up the method for your kinetic run with 0.2 mol 1-1 ethylenediamine (en) solution. You should write the method in your own words - avoid simply customising the instructions given. Note that you should use the passive tense as explained in Making notes and writing a report. This experiment uses standard laboratory equipment and so there is no need to include a diagram. Include the following: • concentrations of both reactants used • how you prepared the solutions • brief details of the analytical method used to monitor the reaction • why this method was suitable • the procedure used including temperature control, choice of wavelength and reference solution used. Use the timings given in Table 3.1 of An experiment in chemical kinetics • how the procedure helped reduce errors. (300-400 words) Results and Discussion - Suggest a plausible rate equation for this reaction. Describe how the experiment was simplified to give the kinetic contribution of one reactant. Justify the relative concentrations of reactants used - why they were appropriate for this method and this reaction? Give the equations you used to check whether the pseudo order was 1 or 2 and what your conclusion was, based on these. Insert your straight-line graph for the kinetic run from the initial concentration of en as 0.2 mol 1-1, that led to this conclusion./nConclusion - Write a brief paragraph on whether the overall aim of the experiment was achieved. You should also compare the value of KR, determined, with the literature value which is 5.95 x 10-21 mol-¹ s¹ at 25 °C. (50-70 words)
