Kinetics of the Reaction of Crystal Violet with Sodium Hydroxide This experiment
ID: 862437 • Letter: K
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Kinetics of the Reaction of Crystal Violet with Sodium Hydroxide This experiment was developed and written by L. R Hunsberger and J. W. Moore and reivsed by J. March; based on KinetiesLab: The Crystal Violet Sodium Hydroxide Reaction, by John F. Cannon, Steven Gammon, and Lymn R. Hunsburger, Journalefaemical Education: Sylware 1994, volume TB, Numbor Copyright (a 1994 by Division ofChemical Education, Inc., American Chemical Society. Used with permission. B INSTRUCTIONS he Textbook Use the index of your textbook to identify background reading material relating to: multi-step mechanisms; temperature and reaction rate; rate laws, integrated; effect of concentration on rate; and chemical kinetics. ur Notebook outline a procedure in your own words that will allow you to collect the required data for each of the exercises below. Anticipate the type of data you will collect and prepare space in your notebook to record the data (data tables or space for observations). Review prior exercises that established the relationship between absorbance and concentration (Beer-Lambert Law). In the first exercise you will need to determine this relationship for a crystal violet solution. Before arriving at the laboratory you should have the answers to the following questions in your notebook. 1. What is the concentration of the solution prepared by placing 3.54 mL of 1.00x 10 s M crystal violet in a 25-mL volumetric flask and diluting to the mark? 2. Sketch the graph including the required axes that will establish the relationship between absorbance and concentration. 3. The concentration of sodium hydroxide is 1.0 Mand the concentration of crystal violet is 1.00 x 103 M. Identify the limiting reagent and calculate how much of the excess reagent remains after the reaction runs to completion. 4. sketch the graphs expected for a zero-, first-, and second-order reactions. Your Safety You must wear your goggles whenever you are in the laboratory. The solutions encountered in this experiment must be handled with care. small volumes of these solutions come in contact with your skin, you should wash the affected area with lots of water. a large spill occurs you should also notify your instructor. Avoid waste: do obtain more reagent than you really need. All solutions and reaction mixtures can be disposed of in the sink. Crystal Violet is an organic dye and will stain most clothing. Gloves must be worn when cleaning up any spill that occurs during this laboratory period. After this lahoratory experience you should be able to:Explanation / Answer
Hello,
1. Use the molarity and mL to determine amount of moles of Crystal Violet .00354 L x 1 x 10-4 mol/1L = 3.54 x 10-7 mol crystal violet. Then divide that by .025 L to get mol/L or Molarity. 3.54 x 10-7 / .025 L = 1.416 x 10-5 M.
I believe the rest can be found on this link. http://course1.winona.edu/jfranz/Lab/chem%20213%20lab/Exp2_CV_Kinetic_Study.pdf
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