CHM1022 Lab Report 1 Rate Law of an Iodine Clock Reaction Name: Sashini Naomi Wijesekera Student ID: 23877847 Lab Partner: Zahiya Imam Lab Session: Monday 9.00am Aim The aim of the experiment is to determine the factors that affect the rate of a reaction‚ by performing the iodine clock reaction and repeating it changing different initial conditions in order to measure and compare the rate of reaction for each experiment and experimentally
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Using the Iodine clock method to find the order of a reaction Introduction When peroxodisulfate (VI) ions and iodide ions react together in solution they form sulfate (VI) ions and iodide. This reaction is shown below: S2O82-aq+ 2I-aq SO42-aq+ I2(aq) The reactants and the sulfate (VI) ions are colourless however the Iodine is a yellow/brown colour. This allows you to measure the progress of the reaction through the colour change when the iodine is produced. In order to determine the order of
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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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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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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 in a solution
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Lab #3: Method of Initial Rates: Iodine Clock Introduction The detailed system of steps in a reaction is called the reaction mechanism‚ and it is one of the principal aims of chemical kinetics to obtain information to aid in the elucidation of these mechanisms in order to better understand chemical processes. Reactions usually occur in a stepwise manner with each step proceeding at a different speed. If the rate of reaction is slow enough to measure‚ this is indicative of a step much slower
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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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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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Kinetics‚ A Clock Reaction Abstract The purpose for the experiment Chemical Kinetics‚ a clock reaction is to figure out the reaction rate of a solution regarding its concentration‚ temperature‚ and also determine the effects of when a catalyst is present. The experiment resulted that the concentration‚ as well as its temperature can affect the rate constant inversely the outcome of the rate constant. By conducting the experiment‚ it is also discovered that the rate order of the reaction resulted
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the rate of reaction in an iodide clock reaction with potassium peroxydisulphate ions? Background When peroxydisulfate ions (S2O82-) react with iodide ions (I-) in the presence of a starch indicator‚ they produce a dark blue solution. Reaction (1) S2O82- + 3I- I3- + 2 SO42- (peroxydisulfate ion) (iodide ion) (iodine ion) (sulfate ion) To determine the rate law for this reaction a series of changes in the concentration of peroxydisulfate‚ [S2O82-]‚ and
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