Computerized Data Acquisition of a Second Order Reaction Essay Example for Free

Computerized Data Acquisition of a Second Order Reaction EssayThe pass judgment at which reactions occur depend on the composition and the temperature of the reaction mixture. Usually the value of reaction is found to be proportional to the concentrations of the reactants raise to a power.1 in that location are many reactions that have a tempo virtue in the form of (1) v = kAaBbAccording to reference1 the power to which the concentration of a species (product or reactant) is raised in a rate law of this nature is the ordain of the reaction with respect to that species. In equation (1) first order with respect to A and first order with respect to B however, the overall reaction is the sum of the individual orders. Thus we have a second order reaction. In this experiment a hexacyanoferrate(III) ion (Fe(CN)63-) oxidizes ascorbic acid (C6H8O6) by the following reaction (2) 2Fe(CN)63- + C6H8O6 = 2Fe(CN)64- + C6H6O6 + 2H+The reaction above is of a first order reaction at room t emperature with respect to individual reactants therefore the reaction stoichiometry and rate law at time t are (3) aA + bBproducts and (4) -dA = kA Bwhere A represents the concentration of ascorbic acid and B represents the concentrations of Fe(CN)63- at time t. For this experiment we will use an integrated rate law in the form of (5) ln A = b A0 a B0 kt + ln A0where A0 and B0 are the initial concentrations of C6H8O6 and Fe(CN)63- and a=1 and b=2. From equation (5), it is possible to calculate the second-order rate constant k by plotting ln A/B against time (find slope of line where b=2 and a=1). EDTA in this experiment is used as a masking agent to insure metal ions that would normally interfere with the analysis in this reaction. Thus the absorbance of Fe(CN)63- at time t is given by (6) Absorbance = 1012 Fe(CN)63-The oxidation of C6H8O6 by Fe(CN)63- involves a weapon that consists of 3 steps.2 In the first step, the ascorbate ion (AH-) is rapidly formed by ionization of the a scorbic acid. (7) AH2 AH + H+Following the ionization is the slow rate-determining step, the oxidation of the ascorbate ion to an ascorbate free radical (AH) (8) Fe(CN)63- + AH-Fe(CN)64- + AH During the final examination step, an electron is rapidly transferred from the ascorbate free radical to the hexacyanoferrate(III) anion, producing dehydroascorbic acid (A) (9) Fe(CN)63- + AH- Fe(CN)64- + A + H+The slow rate-determining step is an ionic reaction between Fe(CN)63- and AH-. According to reference3, the specific rate constant of an ionic reaction in aqueous solution depends on two factors the ionic strength I of the solution and on the charges ZA and ZB of the ionic species reacting to for the emotional complex. (10) log k = log k0 + 1.02ZAZB I1/2ExperimentalAll reagents in this experiment were of reagent grade. Mass measurements were taken on a Shimadzu Libror AEG-120 analytical scale with an distrust of 0.0001. Manual data acquisition was taken with a Barnstead/Turner SP-830 spectrophotometer and a stopwatch. The computerized data acquisition was completed by a Cary 50 Bio. The experiment began by preparing four solutions of 1 x 10-3 M of K3Fe(CN)6 with varied concentrations of NaNO3 0.025 M, 0.05 M, 0.1 M and 0.2 M.This was completed by dissolving 0.0329245 (0.001) g of K3Fe(CN)6 with the specified concentrations of NaNO3 and deionized water in a vitamin C mL volumetric flask. A 25 mL aliquot of each solution was transferred into a 250 mL Erlenmeyer flask and the temperature of the aliquot was recorded. Next, a 500 mL 2.5 x 10-4 M solution of ascorbic acid was prepared by using a standardized 0.01 M HNO3 solution dissolved in 0.005 g of EDTA and deionized water. A 25 mL aliquot was transferred into each of the four 100 mL beakers by using a 25 mL pipet.The spectrophotometer was set to 418 nm and the absorbance class period was zeroed by using deionized water as a standard. The ascorbic acid in the beaker was poured into the K3Fe(CN)6 solution and th e timer was immediately started. The Erlenmeyer flask was swirled for 2-3 seconds before pouring the reacting mixture into a 1-cm cuvette. The cuvette was conditioned with the reacting solution 4 times before being placed into the sample holder of the spectrophotometer. An absorbance reading was taken at 30 seconds and every 30 seconds thereafter for a total of 6 minutes. The same process was implemented with the Cary 50 Bio except that each sample was analyzed by the computer for 7 minutes and 53 seconds. Data/Results