Determine the Activation Energy of the Reaction between Br— and BrO3— in Acid Solution S.6 ( ) Name: [ ] ( ) Time allowed: 55 minutes Introduction: The reaction can be represented by 5Br—(aq) + BrO3—(aq) + 6H+(aq) → 3Br2(aq) + 3H2O(l) The progress of the reaction may be followed by adding a fixed amount of phenol together with some methyl red indicator. The bromine produced during the reaction reacts very rapidly with phenol. Once
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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 use the results to find the rate equation for this particular
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LANNING Aim: Our aim is to detect which factors affect the rate of the decomposition of hydrogen peroxide with a fixed mass of catalyst. A catalyst is a substance‚ which alters the speed‚ or rate of a chemical reaction but is chemically unchanged at the end of the reaction. The two factors that we can change are the temperature and the concentration. We chose to vary the concentration of hydrogen peroxide. The catalyst to speed up the reaction without affecting the result will be manganese oxide. Prediction:
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PHYSICS LAB REACTION TIMES Mr. Brown Name: Jisoo Lee Partner: Seongwook Youn Date: 5/9/17 Purpose: To measure human body’s reaction time to respond and act on unexpected events. Apparatus: The following materials are required for this lab: US dollar bill (new) A meter stick Diagram: Procedure: Part A To be done in groups of two. One of the two will hold a US dollar bill vertically. The partner will lay their arm on a table and stick their hand out of the edge of a table. The
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Temperature on the Rate Constant Joel Costa‚ Alex Fuentes‚ Michael Chea‚ Rex Nwerem Dr. Morgan Ferguson July 9‚ 2013 ABSTRACT | It is often important to determine the rate at which a chemical reaction takes place‚ i.e.‚ how fast it yields the desired products. Temperature is one of the factors that influence the rate of reactions and it does so by providing energy to reactant particles so that a larger fraction of them reach the activation energy necessary to start the reaction. The purpose
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Coursework Rates of Reaction Research The rate of reaction tells us how quickly a chemical reaction takes place. It is important for people in industry to know how fast a reaction goes. They have to know exactly how much of their product they can make each hour‚ day or week. In a shampoo factory‚ the rate might be 100 bottles per minute. We can’t work out the rate of a reaction from its chemical equation. Equations can only tells us how much product we can get. They don’t say how quickly
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Catalyst in Heterogeneous Liquid-Liquid Reaction System S a t o r u Asai‚’ Hidemi Nakamura‚ Mitsunori Tanabe‚ and Kenji Sakamoto Department of Chemical Engineering‚ University of Osaka Prefecture‚ Sakai‚ Osaka 593‚Japan The synthetic reactions of triphenyl phosphate from diphenylphosphoryl chloride and sodium phenoxide and of benzyl benzoate from benzyl chloride and sodium benzoate with phase-transfer catalyst were studied in a heterogeneous liquid-liquid reaction system using an agitated vessel with
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successfully with a rate equation based on autocatalysis by total products. The values of rate constants and activation energy were determined. Recognising the fact that the industrial route to cyclohexene from benzene hydrogenation yields a mixture of cyclohexene and cyclohexane which are di$cult to separate‚ some experiments on oxidation of the mixture of cyclohexene and cyclohexane were also conducted. The values of rate constants remain unchanged in the presence of cyclohexane. The reaction was also studied
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the use of isotopes (as “tracer” elements) has become a valuable tool for the study of reaction kinetics (in slow reactions). 3. CONCENTRATION DEPENDENCE OF REACTION RATES Normally experimental data of kinetic investigations are records of concentrations of reactants and/or products as a function of time for constant temperatures (taken at various temperatures). Theoretical expressions for reaction rates (involving concentration changes) are differential equations of the general form: 1‚cndc
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Determining activation energy (Ea) of a reaction © KCl http://hk.geocities.com/fatherofchemistry Objective To determine the activation energy for the reduction of peroxodisulphate(VI) ions. S2O82-‚ by iodide ions I-‚ using a ’clock’ reaction. Principle The equation for reduction of S2O82- by I- is: S2O82- + 2I- → 2SO42- + I2 The formation of iodine is ’monitored’ by small & known amount of thiosulphate ions‚ S2O32-:
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