Chem Lab 1 - density of an unknown sample I also learned...

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Determination of Density Thursday, April 15, 2010 Chem 1031-015 Procedure: Pick one larger and one smaller sample from the same unknown sample bin. Remember the
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number of the bin and write it down on the data sheet. Weigh a clean 50-mL beaker on the analytical balance and record it. Then weigh each sample, one at a time, while inside the beaker. Record the values on the data sheet. Then obtain the volume of each same by putting one into an already water- filled graduated cylinder and record the mL, and then put the other sample in and record the mL. Do the same previous procedures for two new different samples, again getting on large and one small each time. The last two times you generate the mass of each sample, you use a semi-analytical balance and a triple beam balance. Conclusions and Reflections: During the Determination of Density Lab, I learned how to calculate the mass, volume, and
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Unformatted text preview: density of an unknown sample. I also learned how to use those numbers to find the average density, percent error, and molar volume of the sample. The only problem that I encountered was the lack of triple-beam balances. I liked how the lab taught me to be precise while taking measurements and to double check my answers. Questions: 5) I believe that my unknown sample was Aluminum (Al). I think this because my average density of 2.79 g/mL was closest to Aluminum's average density of 2.70 g/cm^3. 8) Density of solid carbon dioxide = 1.560 g/mL-D = m/v-V = m/d-V = 6.9 g/ 1.560 g/mL-V = 4.4 mL-mass = 6.9 g-volume = ?-6.9 grams of dry ice would occupy a volume of 4.4 mL. 9) Specific gravity of mercury = 13.60-volume = 4.55 mL-mass = ?-D = m/v-M = dv-M = 13.60(4.55 mL)-M = 61.88 g-When a sample of mercury occupies a volume of 4.55 mL, the mass is 61.88 g....
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