which is in an Erlenmeyer flask in the hood. Pour the mixture immediately into the round bottom flask. Add 0.75 mL of 1-butanol to the round bottom flask‚ attach the condenser‚ start the water circulating and the stir bar spinning. Turn on the heating mantle and heat the mixture at gentle reflux (look for the reflux ring in the condenser) for about one hour. After the heating period‚ lift the round-bottom flask from the heat and allow it to cool. Do not remove the condenser until the flask is cool. You
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A KINETIC STUDY OF AN IODINE CLOCK REACTION PURPOSE To investigate the kinetics of the reaction that occurs between iodide and persulfate ion. You will: (1) determine the rate law‚ (2) determine the numerical value of the rate constant at room temperature‚ (3) explore the effect of temperature on the reaction and determine the activation energy (Ea)‚ and (4) investigate catalytic activity of selected metal ions on the reaction. INTRODUCTION Reaction times vary from picoseconds (10-12 seconds)
Free Chemical kinetics Chemical reaction Reaction rate
PRINCIPLES OF CHEMISTRY LAB I Experiment 2 Separation Of Mixtures INTRODUCTION A mixture can simply be defined as a substance that is made up or consists of two or more elements and/or compounds that are physically combined but that have not reacted chemically to form new substances. A mixture may be a solid‚ liquid‚ gas‚ or some combination of those states. Mixtures can be found almost every wher in our everyday lifes and some common examples are * sand and water * salt and water
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tarring a plastic weigh boat on a scale‚ and then adding the salicylic acid powder-like solid. This amount was then poured into a 125mL Erlenmeyer flask. Next‚ 5mL of acetic anhydride was measured using a 10mL graduated cylinder‚ which was then added to the same Erlenmeyer flask. Lastly‚ 5 drops of the concentrated sulfuric acid catalyst were added to the Erlenmeyer flask‚ and this was mixed for 5 seconds using a swirling
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Abstract The objective of this experiment was to observe multi-step purification of benzoic acid after performing the extraction from a mixture containing benzoic acid‚ cellulose‚ and methyl orange. Recrystallization was done to remove impurities from the sample. The amount of BA recovered during recrystallization is much less than the extracted amount of BA. The difference between the pure and impure samples was observed by comparison of melting points. It was found that impure samples will have
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Using a cotton ball a small amount of distilled water was dabbed on each of 6 mealworms. The mealworms were then placed into an Erlenmeyer flask using the forceps. Using the ring stand and clamp to keep the flask in place the CO2 sensor and datalogger were inserted into the flask and initial and final CO2 readings were recorded.(Use pages 105-108 in General Biology‚ Bio 101 Laboratory manual 2010-2011 for correct usage and setup of datalogger) This procedure
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Recrystallization and Melting Point Determination W. H. Bunnelle‚ L. A. Meyer‚ R. E. Glaser (Version 3) Introduction Consider what happens when a solid material is placed in a solvent in which it has a low solubility. Not much! A small fraction of the solid will dissolve‚ but the rest will just sit there. (Actually‚ it doesn’t just ’sit there’ since an equilibrium is in effect‚ with solid molecules going into solution‚ and an equivalent number of dissolved molecules reforming solid‚ but we
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involves the attack of the aryl group at the electrophilic trimethylcarbocation. The resulting product will be recrystallized using methanol and characterized using TLC and melting point analysis. Materials: 400-mL beaker‚ ice for ice bath‚ 25 mL Erlenmeyer flask‚ several volumetric and Pasteur pipets‚ 1.0-mL 10 x 100 mm reaction tube‚ glass stirring rod‚ rubber bulb‚ TLC plate Table 1. Chemicals used in Friedel Crafts synthesis of 1‚4-di-t-butyl-2‚5-dimethoxybenzene Substance Molecular Weight (g/mol)
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Dehydration of Alcohols Abstract The dehydration of cyclohexanol to cyclohexene can be done through fractional distillation. Once the fraction has been collected it must then be dried. The dried distillate is finally tested to determine whether or not it has been dehydrated. The three tests used were infrared spectroscopy‚ Bromine chemical test and Bayer’s chemical test. The infrared spectroscopy showed a large narrow peak at 3062.12(cm-1) and 3020.71(cm-1) which indicates that there is a double
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In this experiment‚ the production of a Grignard reagent (phenylmagnesium bromide) was performed from a bromobenzene reactant combined with magnesium and ether. Phenylmagnesium bromide was then transformed into a tertiary alcohol called triphenylmethanol‚ through addition of another compound called benzophenone‚ as well as additional ether. The end product of triphenylmethanol was analyzed via NMR and IR. Figure 1: Preparation of the Grignard agent by combining bromobenzene with magnesium and ether
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