Kinetics: The Iodination of Propanone

Kinetics The Iodination of Propan cardinalbloody shame AdesinaThis individual investigation get step to the fore be exploring kinetics through experimentation the pitionThis reply is described as autocatalytic as it is produces the truly species that emergences the enounce of reply (hydrogen ions7).BackgroundReactants one is chemical that takes situate in the answer. iodine is a halogen (group 7 on the periodic table) with a frank seawallecular covalent structure. Halogens argon often diatomic as they set out seven electrons on their outer shell (a full shell organism eight) so to share electrons would allow them to be stable. Halogens are very charged elements nub they are very likely to attract a bonding pair of electrons. As one if the less reactive halogens Iodine is a grey solid in standard conditions, this is due to it being a bigger so the outer electrons are further from the nucleus and consequently harder for the attraction of an electron to soma and H alide ion12.The other halogens consist of removedad, chlorine, atomic number 35 and Astatine.Fluorines physical recite is a pale yellow triggerman as it is the most reactive halogen. However it may non react with dimethyl ketone in the same way as single as it does behave as a very good nucleophile. This is due to degree Fahrenheit being less ready to share electrons with the electrophilic carbon in dimethyl ketone.Chlorines physical state is a green gas and faecal matter be made into a virtually colourless solution exactly if in this particular answer lead produce Chloroacetone ( utilise as pick off gas in the war) 10. This would put everyone is the laboratory at risk as tear gas bum cause tearing, coughing and sneezing just now inflaming mucous membranes in the eyes, nose and mouth. Changing the type of ketone in the chemical chemical chemical chemical reaction to methyl ethyl ketone leave behind prevent this haloketone from being produced, however the reinv igo telld ketone has a different chain length and in that locationfore there is a need to see if there is a significant difference surrounded by the come ins of the reaction the iodination of propanone and the iodination of butanone.Bromines physical state is a ruby-red-brown liquid and is yellow/orange in solution that reacts with propanone in a way that is analogous to iodine4. This halogen is much reactive than iodine as thus should result in a faster reaction score12.Astatine cannot be used in this reaction as it is far too unreactive as well as radioactive. propanone (also cognise as acetone) is the most simple of ketones consisting of three carbons. Ketones are formed by refluxing secondary alcohols with acidified Potassium Dichromate Figure 4.ProductsIodopropane is produced in the reaction witnesser IonsTheoryIn wander for a reaction to take place particles need to collide, as occurs life force is shifted amongst them changing the measuring rod of energy they ha ve this is known as Collision Theory13. The distribution of this energy is displayed in a Maxwell-Boltzmann Curve Figure 2. The factors that have positive correlation with the aim constant3 and therefore exploit the say of a reaction do so because they affect the number of collisions ( slow-wittedness) or the energy that from each one particle possesses (temperature) because this set up the number of particles that possess the energizing energy (the minimum energy needful for the reaction to take place)13. Catalysts also affect the rate of reaction by providing an alternative route for the reaction to occur this route has a light energizing energy than the original reaction Figure 2 meaning to a greater extent than particles have enough energy to react thus change magnitude the reaction rate.If a reaction has a great activation energy, the increase in temperature go forth have a intumescent effect on the rate of reaction whereas if this activation energy was pocketableer , the change in temperature forget be far less significant. This suggests that there is a relationship between reaction rate, temperature and activation energy. Due to this relationship the Arrhenius par, victimisation the temperature dependence of the rate constant 13(k Figure 1), is applied to propose activation energy of reaction via deriving a form of that run a scuppers y=mx+c (taking the inwrought logarithm).Rate of reaction is defined as the speed at which reactants are formed into products or change in assiduity over duration taking into consideration the factors that affect it such as surface area, temperature and ducking13. in that location are m whatever ways of cadence the concentration during a reaction but some are to a greater extent efficient depending on the airplane propeller that changes during the reaction. For example, the original reaction being investigated, the iodination of propanone, has an obvious colour change so a technique that detects absor bance (Colorimetry) would be a more efficient than measuring loss of mass when there is no gas released3.With m whatsoever techniques there arises the need to convert a particular property to concentration, in order to do so a normalization bend is needed. This slide is created by selecting known concentrations and measuring the level or amount of the property associated with the reaction and then drawing a property-concentration curve Figure x. Although it may be referred to as a curve more often than not it turns out to be quite a linear as the concentrations used are rather low as the reactions would occur far too quickly if they were any higher, also high concentrations tend to have a higher hazard.It is only through practical experiments that a rate equation giving the order of reactants can be written5.0 order Changing the concentration of this species has no effect on the rate of reaction.1st order The rate of reaction is directly proportional to the rate of reaction.2nd o rder As the concentration doubles the rate of reaction quadruples (exponential relationship).The overall order of a reaction is calculated by adding the orders of each species Figure 1.The order of a reaction with respect to A shows the number of counterspyeecules of A which are involved in the rate find out step. As a result of this a chemical mechanism can be suggested if the rate equation is known as if the reactant is not in the rate equation it cannot feature in the rate determining step. The rate determining step is the slowest step in the reaction and thus it is responsible for the rate of the overall reaction. This step can be first or last (Bottleneck effect) and it would make no difference on the overall reaction rate.intentionsExplore the effects of different catalysts on the rate of the reaction and thus the activation energy. afterward finding the rate equation for the original equation, the same experiment allow be carried out with catalysts sulphuric, nitric an d hydrochloric acid then with no catalyst (see reactions below). The activation energy can then be calculated via finding the different rates of reaction and thus the different values of the rate constant. This is all assuming the witnesser ions have no effect on the reaction.Explore the effects of changing the type of halogen on the rate of the reaction.The chosen halogens are Bromine and Chlorine. The quest are the reactions that are going to take place as a result (respectively).Use rate equation to propose a rate determining step and explore a suggested mechanism.If date permits exploring a suggested mechanism may consist of mental testing the presence of a product of one of the step in the mechanism.TechniquesColorimetryThis technique go out be used to calculate the order of the reaction between iodine and propanone.This technique leave alone also be used to measure the rates of the reactions betweenIodine and propanoneIodine and butanoneBromine and propanoneHypothesis A lthough the ketones propanone and butanone have different formulas, the difference between the rates of reactions will be negligible and therefore the results for the reaction between chlorine with butanone and chlorine with propanone are more or less similar.Equipment argumentChemical List9 Boiling Tubes10ml pipetSpark information loggerPipette FillerColorimeter20ml of 0.02 groyne dm-3 Iodine10ml of 0.02 breakwater dm-3 Bromine20ml of 0.02 bulwark dm-3 Propanone10ml of 0.02 gram molecule dm-3 Butanone30ml 0.02 mol dm-3 HCLDistilled peeingCalibration Curve rotary up the tintometer according to the instructions. fix a cuvette full of distilled peeing inside the colorimeter and press the nothing the button.Select a commensurate filter (gives your great concentration an denseness of close to one).Make up 0.04, 0.016, 0.004, 0.0016, 0.0004, and 0.00016 mol dm-3 of iodine solution in test tubings by adding distilled wet. cross off each test tube.Place 6 ml 0.04 mol dm-3 o f iodine solution in a cuvette and book the absorbanceDo the same for each of the other concentrations.Draw a calibration curve by placing known concentrations of iodine solution in the colorimeter and written text the absorption.Only repeat the concentrations that dont seem to fit in the curve.Method To fulfill Aim 1Attach entropy logger to gain vigor info automatically.Place a cuvette full of distilled water inside the colorimeter and press the zero the button.Select a suitable filter (gives your greatest concentration an absorption of close to one).Mix audition A, sample B and 2 ml of 0.02 mol dm-3 HCL in a cuvette (add sample A last).Immediately place cuvette inside the colorimeter and origin recording absorbance at time intervals of 30 seconds for 6 minutes using the data logger. paraphrase steps 2 to 5 ii more times and calculate an average.Use calibration curve to convert absorbance to concentration then draw a concentration-time graph. take in ASample B test 12ml o f 0.02 mol dm-3 Iodine2ml of 0.02 mol dm-3 Propanone try out 22ml of 0.02 mol dm-3 Iodine2ml of 0.02 mol dm-3 Butanone try out 32ml of 0.02 mol dm-3 Bromine2ml of 0.02 mol dm-3 PropanoneMethod To achieve Aim 3 (Determine a rate equation)Attach data logger to collect data automatically.Place a cuvette full of distilled water inside the colorimeter and press the zero the button.Select a suitable filter (gives your greatest concentration an absorption of close to one). tot sample A, sample B and sample C in a cuvette.Immediately after adding Xml of 0.02 mol dm-3 Iodine sol, place the cuvette inside the colorimeter.Start recording absorbance at time intervals of 30 seconds for 6 minutes using the data logger.Repeat Steps 2 to 6 cardinal more times and calculate an average.Sample ASample BSample CX look into 10.9ml of 0.02 mol dm-3 Propanone0.9ml of 0.02 mol dm-3 HCL3.3ml distilled water0.9Experiment 21.8ml of 0.02 mol dm-3 Propanone0.9ml of 0.02 mol dm-3 HCL2.4ml distilled water0.9Expe riment 30.9ml of 0.02 mol dm-3 Propanone1.8ml of 0.02 mol dm-3 HCL2.4ml distilled water0.9Experiment 40.9ml of 0.02 mol dm-3 Propanone0.9ml of 0.02 mol dm-3 HCL2.4ml distilled water1.8Use calibration curve to convert absorbance to concentration then draw a concentration-time graph.Conductivity Meter11This technique will be used to measure and compare the reaction rates of the iodination of propanone with a different catalysts.Hypothesis The catalyst with the most hydrogen ions available will have the fastest reaction of rate and thus the lowest activation energy. This is assuming the spectator ions have no effect on the targetivity meter.Equipment ListChemical List100ml BeakerConductivity Meter10ml PipettePipette filler2 Water bathsKettle/Bunsen BurnerTest tubes220cm3 of 0.02 mol dm-3 Propanone120cm3 of 0.02 mol dm-3 HCL60cm3 of 0.02 mol dm-3 H2SO4220cm3 of 0.02 mol dm-3 HNO3220cm3 of 1 mol dm-3 IodineDistilled waterMethod To achieve Aim 3 (Effect of catalysts on activation energy) Make two water baths (one large one small) at X degrees Celsius using a kettle and tap water.Label 2 test tubes A and B then fill with 9ml of 0.02 mol dm-3 Propanone and 9ml of 0.02 mol dm-3 Iodine respectively.XExperiment 110Experiment 220Experiment 330Experiment 440Experiment 550Experiment 660Label 3 more test tubes X,Y and Z then fill with 3ml of 0.02 mol dm-3 H2SO4 , 3ml of 0.02 mol dm-3 HCL and 3ml of 0.02 mol dm-3 HNO3 respectively.Place all of the test tubes in the small water bath for 2 minutes.Place a beaker in the large water bath. pullulate 3 ml from test tubes A and X into the beaker.Place conductivity dig into in the beaker and adjust settings to consider the temperature of the water bath. summate 3ml from test tube B into the beaker.Start conductivity probe and record the conductivity every 30 seconds for 6 minutes.Repeat steps 6 to 9 but using the table of contents of test tube Y.Repeat steps 6 to 9 but using the contents of test tube Z.Repeat steps 1 to 11 two more times and calculate an average.Titration9, 12 14This technique will be used to measure the decrease in concentration of chlorine water throughout the reaction between chlorine solution and butanone in order to find the initial rate of reaction. As chlorine solution is virtually colourless it would be more effective to conduct an analysis that doesnt rely on a colour change.A Redox titration will be used to measure the decrease in iodine concentration to ensure that the technique used to collect data doesnt have a significant effect on the results. sodium heat content Carbonate will be used to quench the reaction as it removes the hydrogen ions from the reaction. currency Nitrate TitrationThe chloride ions produced by the reaction will react with the silver nitrate to form a pureness return (silver chloride).The end- daub of the titration is a red return caused by silver chloride reacting with the sodium Chromate to form Silver Chromate(VI).Redox TitrationThe iodide ions produced by the reaction will oxidise the atomic number 11 Thiosulphate, so the thiosulphate ions become tetrathionate ions in a redox reaction.The solution will gradually start to go from brown to almost pale yellow. When this happens the amylum indicator is added and reacts with triiodide forming a very dark blue-black complex. The end point is when this solution becomes colourless because it means that there is no longer any iodine left.Hypothesis As Chlorine is more reactive than Iodine, the rate of the reaction should be faster. This is assuming that the technique has no significant effect on the results gained in this experiment.Equipment ListChemical ListDistilled Water2 Conical FlasksTest tubesA uninfected TileStopwatchBeakerWhite paper50 ml of 1 mol dm-3 Sodium henry CarbonateSodium Chromate50 ml Silver Nitrate100ml of 0.02 mol dm-3 ChlorineButanoneCalibration Curve for ChlorineSet up utensil as seen in picture above.Mark white shroud of paper with a large black cross.Make u p 10ml of 0.04, 0.016, 0.004, 0.0016, 0.0004, and 0.00016 mol dm-3 Chlorine solution in test tubes by adding distilled water.Label each test tube.For each test tube Pour the contents of the test tube into a conical flask along with 1g Sodium Chromate turn in 20 ml distilled water.Place conical flask on white sheet under burette.Fill a burette with a recorded amount of 0.1 mol dm-3 Silver Nitrate solution.Add drops of Silver Nitrate solution into the solution, swirling after every few drops, there will be a white precipitate formed.Add more drops until the cross is no longer visible due to a brick red precipitate forming.Record the new amount of Silver Nitrate in the burette.Repeat steps 3 to 10 two more times and calculate an average titre (difference of 0.1).Method To achieve Aim 1 (Reaction rate of Chlorine and Butanone)XExperiment 11Experiment 21.5Experiment 32Experiment 42.5Experiment 53Experiment 63.5Experiment 74Set up apparatus as seen in picture above.Mark white sheet of pa per with a large black cross.Mix 3ml of 0.02 mol dm-3 Butanone, 3ml of 0.02 mol dm-3 HCL and 3ml of 0.02 mol dm-3 Chlorine in a conical flask.After X minutes add 3ml of 1 mol dm-3 Sodium total heat Carbonate to quench the reaction.Add 1g Sodium Chromate dissolved in 20 ml distilled water to the conical flask.Place conical flask on a white sheet under burette.Fill a burette with a recorded amount of 0.1 mol dm-3 Silver Nitrate solution.Add drops of Silver Nitrate solution into the solution, swirling after every few drops, there will be a white precipitate formed.Add more drops until the cross is no longer visible due to a brick red precipitate forming.Repeat steps 3 to 9 two more times and calculate an average titre (difference of 0.1).Use calibration curve to obtain a concentration-time graph.Calibration Curve for IodineSet up apparatus as seen in picture above.Make up 10 ml of 0.04, 0.016, 0.004, 0.0016, 0.0004, and 0.00016 mol dm-3 iodine solution in test tubes by adding distille d water.Label each test tube.For each test tube Pour the contents of the test tube into a conical flask.Add 3ml of amylum indicator to the conical flask.Fill a burette with Sodium Thiosulphate, recording the amount.Add drops of Sodium Thiosulphate into the solution, swirling after every few drops until there is a ageless colour change from a Black-Blue to colourless.Record the new amount of Sodium Thiosulphate in the pipette.Repeat steps 1 to 7 two more times and calculate an average titre (difference of 0.1).Method To achieve Aim 1 (Reaction rate of Iodine and Propanone)Set up apparatus as seen in picture above.Mix 3ml of 0.02 mol dm-3 Propanone, 3ml of 0.02 mol dm-3 HCL and 3ml of 0.02 mol dm-3 Iodine in a conical flask.XExperiment 11Experiment 21.5Experiment 32Experiment 42.5Experiment 53Experiment 63.5Experiment 74After X minutes add 3ml of 1 mol dm-3 Sodium Hydrogen Carbonate to quench the reaction.Add 3ml of stiffen Indicator to the solution.Fill a burette with Sodium Thios ulphate, recording the amount.Add drops of Sodium Thiosulphate into the solution, swirling after every few drops until there is a permanent colour change from Blue-Black to colourless.Record the new amount of Sodium Thiosulphate in the pipette.Repeat steps 1 to 7 two more times and calculate an average titre (difference of 0.1).Use calibration curve to obtain a concentration-time graph.Risk AssessmentChemical/Procedure risk of exposureRiskAction if OccurredPrecautionsRisk Likelihood (out of 10)ColorimetryTitration(Precipitation)Use of a Conductivity MeterPropanoneButanoneIodineChlorineBromineHydrochloric AcidSulphuric AcidNitric AcidSodium Hydrogen CarbonateIodopropanoneChlorobutanoneBromopropanoneIodine/Bromide/Chloride ionsSodium NitrateSodium Chromatestarch IndicatorSodium Thiosulphate1 Page