"Kinetics of the reaction between acetone and iodine" Essays and Research Papers

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    Iodine

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    Iodine Isotopes are the atoms that have in their nucleus an atomic number corresponding to the chemical behavior of that element. Since isotopes have the same number of protons‚ they all have identical chemical behavior. But‚ however‚ since their neutron numbers are different the isotopes of the same element may have different radioactivity. An isotope that is radioactive is called a radioisotope like iodine‚ which is important in our health. In radioactivity‚ the nucleus of an unstable isotope

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    Chemistry 12: Reaction Kinetics Review 1. Looking at the expressions for reaction rate‚ write expressions with which you could express rates for the following reactions. (Hint: look at what happens to reactants and products.) Recall that solid or liquids can lose or gain mass‚ gases can lose or gain volume and aqueous solutions can increase or decrease in concentration. ("a" is done as an example.) a) Mg(s) + 2HCl(aq) H2(g) + MgCl2(aq) reaction rate = mass of Mg consumed unit time b) c) or

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    PLAN Introduction: After having built up knowledge about the kinetics of reactions I decided to do an investigation in this area. I was initially introduced to this particular reaction1 in EP6.4 and then in AA2.1. I was interested in using this reaction as a means of potentially supporting and quantifying some of the theories that I have studied along with also perhaps extending on them. Aim: Using a clock reaction I shall: • Investigate the effect of concentration for each reactant and

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    Kinetics

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    A KINETIC STUDY OF AN IODINE CLOCK REACTION PURPOSE To investigate the kinetics of the reaction that occurs between iodide and persulfate ion. You will: (1) determine the rate law‚ (2) determine the numerical value of the rate constant at room temperature‚ (3) explore the effect of temperature on the reaction and determine the activation energy (Ea)‚ and (4) investigate catalytic activity of selected metal ions on the reaction. INTRODUCTION Reaction times vary from picoseconds (10-12 seconds)

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    The purpose of this experiment was to determine the speed at which a reaction took place between an iodine and hydrogen peroxide solution. In addition to a change in concentration‚ a change in temperature and a catalyst variable was also introduced to conclude whether or not their presence affected the overall speed of the reaction. In order to determine the effects of these variables‚ several iodine and hydrogen peroxide reactions were prepared‚ (all at varying temperatures‚ volumes‚ and concentrations)

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    Production of Acetone

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    5.1 MANUFACTURING PROCESSES: Acetone is produced directly or indirectly by propylene. Early processes for the manufacture of acetone were based on the thermal decomposition of calcium acetate or the carbohydrate fermentation of corn starch or molasses. The ready availability of propylene in the 1960s led to routes based on the dehydrogenation of isopropyl alcohol or cumene peroxidation. (1) By Cumene Oxidation (Hock Process). Propene is added to benzene [71-43-2] to form cumene [98-82-8]‚ which

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    This experiment was a Landolt Iodine clock reaction - Oxidation of Bisulphite by Iodate. It involved conducting three measured experiments. The first variable tested was concencentration. This was tested by conducting two experiments‚ each varying the concentration of either the NaHSO3 or KIO3. The varying of NaHSO3 involved using 0.1 Molar of KIO3 against decreasing concentrations of NaHSO3 (0.25 M‚ 0.125 M‚ 0.0625 M and 0.03125 M). When decreasing the concentration of KIO3‚ 0.25 M of NaHSO3 was

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    Iodine Clock

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    perform an experiment known as the "iodine-clock" reaction‚ in which hydrogen peroxide reacts with iodide to form iodine‚ and the iodine subsequently reacts with thiosulfate ion until the thiosulfate has been consumed. At that point‚ the reaction solutions turn blue in the presence of starch. The experiment helps students understand the fundamentals of chemical kinetics --- the speeds at which reactions take place. 1. Activation Energy * Chemical reactions are thermodynamically "favorable"

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    There are three reactions in the iodine clock reaction. The first reaction is IO3-(aq) + 3 HSO3-3 SO4-(aq) + I-(aq)+ 3 H+(aq)‚ where the iodate ions become iodide ions1. The second reaction is 6 H+(aq) +IO3-(aq) + 5 I-(aq) 3 I2(aq) + 3 H2O(l) where the iodate ions become molecular iodine2. The third reaction involves molecular iodine becoming a dark blue starch;I2(aq) + starch blue-black complex3. These three reactions react in a sequence. In any reaction the concentration is exponentially related

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    Substance Hazard images Exposure Symptoms Prevention First aid Spillage/Disposal Storage PREVENT GENERATION OF MISTS! AVOID ALL CONTACT! IN ALL CASES CONSULT A DOCTOR! Hydrogen peroxide Hydrogen dioxide Dihydrogen dioxide H2O2 Molecular mass: 34.0 20% Vol and lower   Corrosive to metals‚ category 1 Skin corrosion‚ categories 1A‚ 1B‚ 1C Serious eye damage‚ category 1 Oxidizing gases‚ category 1  Oxidizing liquids‚ categories 1‚2‚3 Inhalation Sore throat. Cough. Dizziness

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