Lab : Iodine-starch Clock Reaction Pre-lab: Before the lab was conducted‚ the concentration of the Iodate ions to be in the mixture made by dissolving specific volumes of solution A with a constant concentration and water was calculated using the dissolution formula: C1V1 = C2V2 Sample Calculation 1: Concentration of the Iodate ions: For mixture 1: C2 = C1V1/ V2 = (0.020mol/L) x (0.003L)/(0.01L) = 0.006mol/L The same calculations were used in the calculating of the
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Due to the lack of literature value for the effects of temperature on the rate of the Iodine Clock Reaction‚ there was no final percentage error. However‚ Looking at Graph 1.6‚ the line of best fits clearly shows the low precision throughout this experiment resulting in an increase of Random error. This could be
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Experiment A1: Kinetics of the Reaction between Acetone and Iodine The key aim of this experiment was to determine the rate equation for the acid-catalysed iodination of acetone and to hence consider the insinuations of the mechanism of the rate equation obtained. The stoichiometric equation for the reaction between iodine and acetone is below‚ followed by the rate equation (where x‚y‚z and k are the values to be obtained): I2 + CH3COCH3 CH3COCH2I + HI -d[I2]/dt = k [I2]x [CH3COCH3]y [H+]z
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TITLE OF EXPERIMENT: An investigation of the iodine/propanone reaction. DATA COLLECTION AND PROCESSING : Chemical Equation: CH3COCH3 (aq) + I2 (aq) ( CH3COCH2I + H+ (aq) + I- (aq) Rate of reaction: R = V T Concentration of reactant after dilution : Volume of reactant x concentration of reactant Total volume of mixture Uncertainty for rate of reaction: R =( V + t ) x R V t Eg
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Purpose: To determine the general rate law for the reaction of S2O82- + I- through a series of experiments and calculations. Materials: -Temperature probe -3 large test tubes -3 rubber stoppers -Pipets -0.20 M KI soln -0.20 M NaCl soln -0.010 M Na2S2O3 soln -2% starch soln -0.20 M K2SO4 -0.20 M K2S2O8 -0.2 M CuSO4 -Timer or stopwatch -Small beaker -Hot water Procedure: Refer to Lab #12‚ No changes Data: Table #1: Quantitative/Qualitative Observations Room Temp: 25.4°C
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in the presence of small quantities of starch and sodium thiosulfate solutions. As the iodine molecules are produced they immediately react with the thiosulfate ions and are converted back to iodide ions: I2(aq) + 2S2O32⁻(aq) → 2I⁻(aq) + S4O62⁻(aq) During this period the reaction mixture remains colourless. But once the thiosulfate ions have been used up‚ a blue/black colour suddenly appears because the iodine molecules now get the chance to react with the starch. A series of experiments will be
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Experiment 16: Kinetics: The Iodine Clock Jane Smith Purpose: The objective of this experiment was for students to apply their knowledge of kinetics and rate laws in order to determine the rate of a chemical reactions‚ activation energy‚ and frequency factors of those reactions. Specifically‚ this experiment was performed using a series of solutions with varying concentrations of KI‚ Na2S2O3‚ and (NH4)2S2O3 . Students recorded time elapsed to observe physical evidence of a reaction taking place
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EXPERIMENT 3-CHEMICAL KINETICS: THE IODINE-CLOCK REACTION J.CHAN1 and C.CABANLIG2 1NATIONAL INSTITUTE OF MOLECULAR BIOLOGY AND BIOTECHNOLOGY‚ COLLEGE OF SCIENCE 2NATIONAL INSTITUTE OF MOLECULAR BIOLOGY AND BIOTECHNOLOGY‚ COLLEGE OF SCIENCE UNIVERSITY OF THE PHILIPPINES‚ DILIMAN‚ QUEZON CITY 1101‚ PHILIPPINES DATE SUBMITTED: JANUARY 8‚ 2013 DATE PERFORMED: DECEMBER 5‚ 2012 ------------------------------------------------- ABSTRACT The kinetics of the reaction between persulfate (S2O82-)
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Introduction The purpose of this experiment is to determine the rate equation for the “Iodine Clock Reaction” experiment. The experiment will consider the equations 〖2I〗^-+S_2 O_8→2〖〖SO〗_4〗^(2-)+I_2 and I_2+2〖S_2 O_3〗^(2-)→2I^-+S_4 O_6 in order to determine the rate law of Rate=k[〖〖S_2 O_8〗^(2-)]〗^a 〖[I^-]〗^b by using the experimental data to calculate the values of exponents a and b as well as the rate constant k. Experimental Supplies Needed: 250 mL Erlenmeyer flask‚ 100 mL beaker‚ graduated
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It was originally hypothesised that the reaction time would decrease with higher concentrations of the reactants‚ potassium iodate and sodium bisulfite as collision theory stated that more molecules present in a given volume meant a greater chance they would collide. Furthermore‚ the time was expected to decrease with higher temperatures as it influenced the reactant particles by raising their kinetic energy. However‚ the data collected from this experiment only partially supported this hypothesis
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