Boil at least 10 minutes. 7. While the metal is still in the boiling water bath, measure the temperature of the boiling water carefully with a thermometer and record to tenths, one decimal place, in Data Table 2 8. After the metal has been heating 10 minutes, remove the metal from the boiling water bath using the string. Immediately transfer the metal into the calorimeter cup so that the water covers the metal.
The mixture was decanted again in to the same beaker. Next, we added boiling chips to the liquid and evaporated the solvent over the hot plates under the hood. After the solvent was evaporated and the flask was cooled, we used a spatula to remove a small amount of the crude product and took its melting point. We determined the melting point range of the sample to be 43.0-46.0 degrees Celcius.The crude product was yellow colored when it was warm and orange in color when cooled and sticky. We then recrystallized our sample using 5 ml of warm acetone that was heated on a hot plate under a hood.
Hydrochloric acid was then added to the solution until the bubbles stopped in order to completely get rid of all of the zinc. Next, we used vacuum filtration to filter the copper out of the solution. We drizzled alcohol and acetone over the copper to help it dry faster. Once it appeared dry, we weighed the copper and filter paper. When we subtracted the mass of the filter paper, the mass came out to 1.312g.
8. Placed the remaining mixture, containing sand, benzoic acid and table salt into beaker and added 50mL of distilled water. 9. Set up the beaker stand and burner fuel and heated the beaker of solids and water to near boiling. Stirred the mixture to make sure all soluble material dissolves.
The release button on the lighter is pressed and held until approximately 90 ml of water is displaced from the cylinder; the level of the water in the cylinder should be level with the water in the trough. The temperature of the water is taken and the lighter is reweighed. All data is recorded and then this experiment is repeated three times, using all the same material. Data and Observations: As the water is displaced from the cylinder, bubbles continuously floated to the end of the cylinder as the water level went down. See Table 1 for all the recorded results.
Atomic Mass = 26.4/ specific heat. Equipment/Materials: samples of metals large test tube 400 mL beaker hot plate balance foam coffee cups thermometer Safety: • An apron and goggles must be worn in the laboratory. • Avoid contact with the hot plate. Procedure: 1. Place about 200 mL of tap water in a 400 mL beaker and place it on the hot plate.
Record the initial temperature of the liquid in the calorimeter. Watch the thermometer until maximum temperature is achieved. Weigh out 2.0g of NaOH pellets. Record the temperature of the distilled water in the calorimeter until the temperature is constant then add all of the pellets at once. Gently stir the pellets until the acid is dissolved by shaking the the apparatus.
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.
• After the flask was heated, I removed it from the heating mantel and allowed it to cool to room temperature. • Next, I poured 15mL of absolute ether and 9mL of bromobenzene into the 250mL flask and waited 5 minutes for any reaction. • There were no signs of reaction after 5 minutes; therefore the lab assistant used a glass stirring rod to crush the magnesium in order to get the reaction started. When this was done, the liquid became cloudy, rapidly bubbling, and the color turned rusty red. • Next, I added 25mL of absolute ether and attached a reflux condenser to the flask.
After 5-10 minutes with the heat we started to observe a color change, after the CuSO4 (copper sulfate) cooled it had turned a grayish/ blue color. Using the electronic balance we weighed the CuSO4 with the crucible, which weighed 19.972 and subtracted the original weight of the crucible (19.972-19.071), which came to about .901, the weight of the leftover CuSO4. Heating to a constant mass is the only way to insure that the reaction is complete. It means checking the mass to ensure it is near each other at the end of a reaction. The color change in the copper sulfate when we heated it indicated that all of the water has evaporated, to be sure, we heated and weighed the crucible and CuSO4 again, and it came out to be .901g again.