EFFECT OF CONCENTRATION ON REACTION RATE The aim of this experiment is to find the effect of varying the concentration of iodide ions on the rate of reaction between hydrogen peroxide and an acidified solution of potassium iodide: H2O2(aq) + 2H+(aq) + 2I⁻ → 2H2O(l) + I2(aq) The course of this reaction can be followed by carrying it out in the presence of small quantities of starch and sodium thiosulfate solutions. As the iodine molecules are produced they immediately react with the thiosulfate
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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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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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solution of KMnO4 and H2SO4‚ the solution will turn colourless and it will take a specific time for the reaction to complete. By increasing the temperature‚ the time it takes (the rate) for the solution to completely change to colourless will be increased. Thus it can be said‚ that it is being hypothesized that an increase in temperature will cause an equal increase in the rate of the reaction. Method:1). Using a measuring cylinder‚ place 50 cm3 of sulphuric acid into a 250 cm3 beaker‚ add 50 cm3
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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-) and iodide
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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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Determining the Stoichiometry of Chemical Reactions Mrs. Farrales Nikita Pandya October 23‚ 2012 December 3‚ 2012 INRODUCTION In the method of continuous variations the total number of moles of reactants is kept constant for the series of measurements. Each measurement is made with a different mole ratio of reactants. A mole ratio
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Kinetics of a Reaction I. List of reagents & products 1. 1.0 M Copper(II) nitrate (Cu(NO3)2‚ 0.10 M Hydrochloric Acid (HCl)‚ 0.010 M Potassium Iodide (KI)‚ 0.040 M Potassium Bromate (KBrO3)‚ 0.0010 M Sodium Thiosulfate (N2S2O3)‚ 2% Starch solution‚ Water (H2O) II. Summary of Procedure. Part 1: Find the Volume of One Drop of Solution 2. Fill pipet with 3ml of distilled water 3. Mass a beaker and record 4. Put 5 drops of water into beaker and record
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to the first test tubes‚ Sn granules to the second and Cu filings to the third and compared the rates of evolution of hydrogen gas in each test tube. 2.1.2. We mixed 3mL of 0.02 M KMnO4 and 2mL of 3 M H2SO4 in a test tube and stirred using a glass rod. Next‚ we divided the solution into two. We added 2mL of 0.03 M Na2C2O4 solution to the first half and 2 ml of H2O2 to the second and compared the rates at which the violet color of KMnO4 in the two test tubes disappeared. 2.2. Concentration 2
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Introduction – Lab Report What is a Chemical Reaction? A chemical reaction is a change in matter that produces one or more new substances. A chemical change or reaction occurs when bonds are broken and new ones are formed. The formation and dissolution of these bonds are dependent upon environment changes. Even without the usage of microscopes‚ chemical reactions are usually apparent to the naked eye. The two main kinds of changes that one can observe are the formation of new substances and changes
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