Dr. Jefferson Andrews Chemical Principalities - CHEM 1101 1 October 2008 Copper, the Funnest Lab Ever. Abstract: This experiment served as a test of our individual laboratory skills in carrying out several Abstract: chemical transformations involving copper. The experiment was successful in that the Abstract: percent yield was reasonable, and we were able to recover our copper sample with Abstract: maximum efficiency ( we were able to recover all of the copper with which we began ). Introduction: This experiment involved the separation and purification of our desired product ( copper ) from any unwanted side products. This was accomplished using several different methods including filtration, sedimentation, decantation, extraction, and sublimation.
Gently stir the pellets until the acid is dissolved by shaking the the apparatus. Lift the calorimeter lid and wash out its contents and the thermometer. Repeat this experiment using 50.0 mL of 1.0M acetic acid. Repeat experiment using 25.0 mL of each 2.0M sodium hydroxide and 2.0M acetic acid. Data Table(s): Reaction equation Mass of solid NaOH Initial Temp.
So, qwater = qmetal Using the formula qmetal = m × c × ΔT, calculate the specific heat of the metal. Use the data from your experiment for the metal in your calculation. Part II: Calculate the energy change (q) of the surroundings (water) using the enthalpy equation qwater = m × c × ΔT. We can assume that the specific heat capacity of water is 4.18 J / (g × °C) and the density of water is 1.00 g/mL. Show ALL your work.
I then poured the mixture on to a solid white piece of paper. I then used a magnet wrapped in clear plastic bag to separate the iron from the mixture. I weighed the iron and calculated and recorded the mass in table 1. I put the remaining mixture in a beaker with 50 mL of distilled water and heated to a boil and removed, then poured the liquid from the beaker into a paper cup. I then added 15 mL of distilled water and heated to a boil and removed, then poured the liquid from the beaker into the same paper cup that held the previous liquid.
MATERIALS * One Bunsen burner * 1 gram of Sodium Chloride * 1 gram of Potassium Chloride * 1 gram of Lithium Chloride * 1 gram of Barium Chloride * Nichrome wire (wire with a loop) * 0.4 grams of water * Protective eyewear * Lab gloves Barium is a toxic metal, be sure to wear gloves and goggles when handling this material, also if using a Bunsen burner be sure to turn of the gas. METHOD Part One: Be sure to clean and dry the Nichrome wire, looped wire, to ensure no residue is present on the wire that could produce different results. Once the wire is clean and dry, place 0.1 grams of water on the end of the wire with the loop. When the water has been placed on the loop, carefully place the 1 gram sample of Sodium Chloride on the loop where the water was previously placed. This can be done by placing the sample on the table top and dabbing the end of the metal wire with the loop filled with water on the sample.
Extraction and Drying: Using a separatory funnel, the cooled filtrate was extracted with 10ml of methylene chloride. After shaking our mixture, we broke and dried our emulsion by slowing passing the lower layer through a cotton ball layered with anhydrous magnesium sulfate. The extraction process was repeated 2 more times for maximum collection of the organic layer. Distillation: The extracts were poured into a 50ml round bottle flask and connected to a simple distillation apparatus. To obtain the caffeine, the methylene chloride was removed from the extract, leaving us with our solid caffeine residue.
Second, methyl benzoate is added to form a new carbon-carbon sigma bond. The intermediate magnesium alkoxide will then be hydrolyzed to form tertiary alcohol product. Experimental Procedure: Part A: Preparing the Grignard reagent • I placed 1.98 grams of magnesium turnings into a cleaned 250mL round-bottom flask and then attached the calcium chloride drying tube into the round-bottom flask • Then, I placed this flask onto a heating mantel and adjust the controller to setting ‘6’. This flask is heated until it was too hot to touch. • After the flask was heated, I removed it from the heating mantel and allowed it to cool to room temperature.
Each test (for Iodine (I2), for Iodide (I-), and for Triiodide (I3-)) match the standard for each reactant (I2, I-, I3-). For example, when testing for I2 we mixed 1/3 of our home-made tincture and added the reagent mineral oil. Mineral oil, unlike water, is nonpolar and when mixed with nonpolar iodine, like dissolves like. Iodine mixes with mineral oil and a purple color is observed. Therefore our standard results matched our home-made results.
Gas Volume Determination Lab Objective: Use stoichiometry and ideal gas law to predict gas production. Successfully collect gas being produced. Introduction: Write an introduction. Materials: Small flask 100 mL graduated cylinder 5 mL graduated cylinder Rubber stopper Tubing Tubing/Stopper connector Water basin 6M HCl Zinc metal Ring Stand if needed Clamp if needed Copper wire Metal cutters Procedure: 1. Obtain between 0.1 to 0.2g of zinc metal.
(˚C) | Final Temp. (˚C) | Final Water Temp. in Calorimeter (˚C) | Initial Water Temp. in Calorimeter (˚C) | Metal Temp. Change with Metal (˚C) | Iron Shot | 20 | 100 | 28 | 20 | 8 | Aluminum Shot | 20 | 100 | 34 | 20 | 14 | Copper Shot | 20 | 100 | 27 | 20 | 7 | Results The results from this experiment were interesting.