REPORTPre-Lab Work\(individual ¨C CHECK VOH FOR UPDATED GUIDELINEIntroductionIn-Lab WorkPost-Lab Notebook Report (CHECK VOH FOR UPDATED GUIDELINES)Mastery ChartTHE REACTION OF RED FOOD COLOR WITH BLEACH TECHNICAL AND THEORETICAL SKILLS In this assignment you will monitor the rate of a chemical reaction prepare a volumetric solution determine the extinction coefficient of a compound use a spreadsheet to analyze data calculate the order and rate constant of a reaction SAFETY FD&C Red #3, or Erythrocin B sodium, the food coloring dye that you will use in this experiment is intensely colored. Always wear safety glasses or goggles and a protective lab coat or apron. Handle the dye carefully avoiding spilling on the balance or bench top. Sodium hypochlorite, household bleach, is a bronchial irritant. Keep solutions covered or in the hood; avoid breathing the vapors. Immediately, wipe any spills of either reagent and wash any residues with large quantities of water. INTRODUCTION In this assignment, you will study rate of the reaction of FD&C Red #3 (Red #3) with sodium hypochlorite. Since this reaction is very visible, you will use a spectrophotometer to quantitatively follow the rate of disappearance of the colored reagent. Your rate data will allow you to determine the rate law and to propose a possible mechanism for the reaction. COINaOICOONaIOI FD&C #3 Because of the extended conjugation within the molecule, the π−π* absorption occurs in the visible region of the spectrum at 500 nm. When the dye reacts with hypochlorite, the color disappears. A possible explanation of this reaction is that the bleach oxidizes the central methylene carbon to an alcohol. The resulting triphenylmethanol derivative, with the sp3 methane carbon, would no longer have the extended conjugation system and the π−π* absorption of the less conjugated product would occurs at a lower wavelength outside of the visible region of the spectrum. Schematically we can represent this reaction as shown on the next page: This stoichiometry, however, does not indicate how the reaction occurs or the mechanism of the reaction. A study of how the concentrations of the reactants affect the rate of the reaction gives insight into the mechanism and whether this simple explanation is correct. Spring 2005 1COINaOICOONaIOIOINaOICOONaIO-IHO+OCl- Red Colorless Extended Conjugation Isolated Areas of Conjugation The Rate Law The rate of a reaction can be represented either by the disappearance of reactants for the appearance of products. Since Red #3 is the only colored species in the reaction, we can monitor the rate of the reaction shown above by recording the decrease in the color of the solution with time. That is, Rate = − d[Red #3]dt = k[Red #3]a[OCl-]b (1) where the exponents a and b indicate the molecularity or order of the reaction with respect to each reagent, and k is the overall rate constant for the reaction at room temperature. The objective of this experiment is to determine the values of the exponents a and b and the value of k at room temperature. If the concentration of the bleach is held constant throughout a reaction by having a large excess present, then the rate law simplifies to Rate = − d 3[Red # ]dt = κ' [Red #3]a (2) where [OCl-]b has been absorbed in the pseudo-rate constant κ'. Rearranging this rate expression to − d[Red #3][Red # 3]a = κ' dt (3) gives a form that can be integrated depending on the value of a. If a = 1, the integrated expression becomes -ln[Red #3] = κ' t (4) and a plot of ln[Red #3] vs time will give a straight line with a slope of κ'. Spring 2005 2If, however, a = 2, the integrated expression becomes 1[Red # 3] = κ't (5) and a straight line occurs with a plot of 1/[Red #3] vs time. Thus, if one can experimentally determine the concentration of the dye at various times during a reaction, the relationship of that concentration with time that gives a linear fit allows an experimenter to establish the molecularity of the reaction with respect to the dye, that is a value for a. A second set of rate data, collected for reactions where the concentration of the dye is held constant and the initial excess concentration of the bleach is changed in a simple ratio between trials, can then allow a determination of a value for b. For example, since the pseudo rate constant κ' = k [OCl-]b , if [OCl-] is doubled between trials and the κ' also doubles, then b must = 1. On the other hand, if [OCl-] is doubled and the observed rate increases by a factor of 4 then b = 2. However, if [OCl-] is doubled between trials and there is no change in the observed rate of the reaction, then b = 0 and it can be concluded that the bleach is not involved in the rate determining steps of the mechanism. PROCEDURE The TA will assign you into a group with 2 other students. For each rate reaction trial, one person will be the timer, one person will be the data recorder and one person will read out the absorbances as indicated by the timer. You should rotate roles between rate runs. Before you begin work, agree upon who will be responsible for each part of the work and the report. Record this in your notebooks. Sign each of the notebooks indicating the agreement. You will turn in one report with all the group member names on it, and the allocation of responsibility. Solution Preparation: You will need to prepare several solutions to carry out the necessary rate runs. It is most efficient to have all the solutions ready before you start any of the runs. Solution 1. Weigh about 0.35g of food coloring dye to the nearest tenth of a milligram using weighing paper. Record the weight and quantitatively transfer the dye to a 100-mL volumetric flask. Re-weigh the weighing paper to determine the actual weight of dye that you transferred to the volumetric flask and make up the volumetric solution to the mark following standard procedures for the preparation of a volumetric solution. Transfer the solution to a clean, dry container. Label this container as “Solution 1.” Solution 2. Thoroughly rinse and clean the inner walls of the volumetric flask three to four times with distilled water. Using a 5-mL volumetric pipet, transfer 5 mL of Solution 1 to the 100-mL volumetric flask. Again use standard procedures to complete the preparation of this volumetric solutions. Transfer this solution to a clean, dry flask and
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