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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PLANNING Investigating the Kinetics of the reaction between Iodide ions and Peroxodisulphate (VI) ions By the use of an Iodine clock reaction I hope to obtain the length of time taken for Iodine ions (in potassium iodide) to react fully with Peroxodisulphate ions (in potassium Peroxodisulphate). I will do three sets of experiments changing first the concentration of iodide ions‚ then the concentration of Peroxodisulphate ions and finally the temperature of the solution in which the reaction
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D-block ions and the kinetics of reactions iodine clock reaction: By Stephen Parsons 6K2 Centre number: 61813 Candidate number: 8270 Table of Contents My aim and my reaction: 3 Rate of reaction: 4 Activation enthalpy: 5 Collision theory: 6 The effect of temperature on reaction rate: 7 The effect of concentration on reaction rate: 7 The effect of a catalyst on reaction rate: 8 D-block elements: 9 The effect of extra kinetic energy (from stirring etc.): 10 Where do we use D-block ion catalysts
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Aims The aims of this investigation are: 1. To find the rate equation of the reaction of hydrogen peroxide and iodide ions. This will be achieved by using an iodine clock method and colorimetric analysis. 2. Draw a graph of rate against concentration for each reactant (Hydrogen peroxide‚ potassium iodide and H+ ions). 3. Finding the order for each reactant 4. Finding the rate-determining step. 5. Proposing a mechanism for the reaction. 6. Using Arrhenius’ equation to find the activation
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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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CHEM 1112 Kinetics of the Persulfate – iodide Clock Reaction The purpose of this experiment is to determine the rate law and the activation energy for the reaction between persulfate ion‚ S2O82-‚ and iodide ion‚ I-: S2O82-(aq) + 2 I-(aq) 2 SO42-(aq) + I2(aq) The rate law can be written as Reaction rate = (1) Where m and n are the orders with respect to S2O82- and I-‚ respectively‚ and k is the rate constant. Determining the rate law involves determining the values
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How does a catalyst in the form of a metal ion affect 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
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Research for Kinetics Coursework http://www.google.co.uk/#sclient=psy-ab&hl=en&rlz=1R2ADRA_enGB386&source=hp&q=An+investigation+into+the+kinetics+of+the+reaction+between+potassium+peroxodisulphate+and+potassium+Iodide&pbx=1&oq=An+investigation+into+the+kinetics+of+the+reaction+between+potassium+peroxodisulphate+and+potassium+Iodide&aq=f&aqi=&aql=1&gs_sm=e&gs_upl=4649l5023l3l5663l2l0l0l0l0l0l0l0ll0l0&rlz=1R2ADRA_enGB386&bav=on.2‚or.r_gc.r_pw.&fp=4cbda8eccdfde5e1&biw=1280&bih=600 http://www.chemistry-react
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Peroxodisulphate and Iodide practical – exemplar Skill A – Chemical Ideas Reaction between Peroxodisulphate and Iodide The reaction between peroxodisulphate and iodide ions is given by the following equation: S2O¬82- (aq) + 2 I- (aq) 2 SO42- (aq) + I2 (aq) The structure of the peroxodisulphate ion‚ with oxidation states‚ is shown below: (Structure) The changes in oxidation state within the reaction are as follows: Element Oxidation state in reactant Oxidation state in product Oxidised or
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We learning about how ions dissolve in water and also how dissolved ions of different compounds react with each other and finally examine the final product for the presence for ions. Materials- Sheet of Paper Lead (II) Nitrate Potassium Iodide Deionized Water Filter Paper Charcoal Matches Equipment- Clean dry spatula Small Beakers Glass stirring rod Ring stand Funnel Tweezers Bunsen Burner Small Test Tubes Safety- During this lab we are dealing with some dangerous chemical including Lead Nitrate
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