Experiment 19: Kinetics : the Rate of an Experiment

demo 17, 2013 March 17, 2013 shout out Ryan annasdass arokiasamy ID 1206875 Group Members Chan Pei Qie,Chong Ven Yen Name Ryan annasdass arokiasamy ID 1206875 Group Members Chan Pei Qie,Chong Ven Yen experiment 19 kinetics the study of a chemic chemical reception experiment 19 kinetics the study of a chemical answer Results Part A I- / jettye dm-3 S2O82- / mol dm-3 S2O32- / mol dm-3 Time /s regularize of I2 formation / mol dm-3 s-1 0. 2 0. 2 0. 01 1. 25 0. 1600 0. 2 0. 15 0. 01 13. 37 0. 0150 0. 2 0. 10 0. 01 26. 00 0. 0077 0. 2 0. 05 0. 01 66. 5 0. 00075 Part B I- / mol dm-3 S2O82- / mol dm-3 S2O32- / mol dm-3 Time /s stride of I2 formation / mol dm-3 0. 2 0. 2 0. 01 3. 45 0. 0580 0. 15 0. 2 0. 01 7. 56 0. 0198 0. 10 0. 2 0. 01 9. 06 0. 0110 0. 05 0. 2 0. 01 23. 91 0. 0021 Part C Initial temperature/ OC last-place temperature/ OC Time t /s lay of I2 formation / mol dm-3 1/T (1/K) Log t 15 21 29 0. 00690 0. 003472 1. 462 24 25 20 0. 01000 0. 003367 1. 301 35 42 1 3 0. 01538 0. 003247 1. 114 45 40 8 0. 02500 0. 003145 0. 903 Calculations & QuestionsAssociated essay cadence Reaction aim Using bulk of Gas ProducedThe effect of temperature is that it increases the assess of reaction, ascertained here by the higher temperatures great(p) a much dissoluteer reaction date a) Is reaction (2) fast or slow with note to reaction (1)? exempt your reasoning or record to to each one one test you do to help pass water your conclusion Reaction (2) is fast with respect to reaction (1). Reaction (2) I2+2 S2O32- 2 I-+ S4O62- occurs extremely fast, I2 formed in the reaction is consumed immediately and when the limiting agent S2O32- is apply up, I2 reacts with the stiffen indicator to form a gritty food coloring solution. ) Does reaction (1) or (2) control the clip required for the blue colour to pop? Reaction (1) 2I-+ S2O82-I2+2SO42- controls the time required for the blue colour to appear as it is the I2 that will react with the starch indica tor to produce the blue color solution to appear c) Calculate the rate of formation of I2 in mol dm-3 s-1 for each experiment at room temperature and plot of land this rate i) Against S2O82- at unbroken I- ii) Against I- at constant S2O82- The rate of formation of I2 peck be calculated by reason of the rate of change of the thiosulphate ion over the time taken Rate of formation of I2=? I2t d) What ar the shapes of these plots? They are straight line interprets ,with the y axis instantly proportional to the x axis e) What is the signifi micklece of this? This shows that the rate is directly proportional to the concentration of I- and S2O82- and by astute the gradient of the graph we will engender the rate of reaction. f) Write the rate equivalence for reaction (1) dI2dt=kS2O82- And calculate the rate constant , k Rate = kI-S2O82- k = Rate / I-S2O82- k = slope / S2O82- k = (0. 015-0. 0008)/(0. 15-0. 05)Rate constant k = 0. 142 mol-1 dm3 s-1 g) Calculate the nix of activat ion of the reaction If we plot a graph of log t against 1/T, we can obtain the Ea by calculating the slope. ramp of the graph = Ea / 2. 303R Ea / 2. 303R = (1. 462-0. 903)(0. 003472-0. 003145) Ea / 2. 303R = 0. 559/(3. 2710-4) Ea = 1709. 48 x 2. 303R Ea = 1709. 48 x 2. 303 x 8. 314 Ea = 32731. 65 J/mol Discussion Precautions Among approximately of the precautions taken were to wear gloves , safety gawk and lab coats to vitiate any accidental injury in case of exposure to chemicals.Secondly, thither were separate cadence cylinders prepared for each solution as to not commix 2 solutions in a measuring cylinder to avoid any reactions. The persulphate was poured in rapidly as this is an extremely fast step and has to be poured all at once. Finally,when diluting the persulphate solution, it was done as accurately as possible in order to avoid a wrong concentration instead of the one intended. Conclusion Based on the experiment done as surface as the analysis of the results and a fter doing get on results, we have learned that the activation energy of the reaction is 32. 73 kJ.Furthermore, we have gained an incursion into the kinetics of a reaction, its rate, the rate constants as well as the rate of reaction. References Martin S. Silberberg, interpersonal chemistry the Molecular Nature of Matter and Change, one-fifth Edition, McGraw Hill, 2005. F. Albert Cotton, Geoffrey Wilkinson, Carlos A. Murillo, and Manfred Bochmann, Advanced Inorganic chemical science, Sixth edition, arse Wiley& Son. 1999. F. Albert Cotton, Geoffrey Wilkinson, Paul L. Gaus, Basic Inorganic Chemistry, tierce Edition, John Wiley& Son. 1995. John C. Kotz, Paul M. Treichel, and Gabriela C. Weaver, Chemistry and Chemical Reactivity, Sixth Edition, Thomson 2006.