The lab “Aluminum Atoms” was designed to determine whether heavy-duty or house hold aluminum foil was the thicker than the other and to show the different atomic calculations of each type of foil. It was learned that heavy-duty foil is thicker than the household aluminum foil. An atom is the basic unit of a chemical element. Avogardo’s number, 6.02 x 1023, is the number of particles found in one mole of a substance. The molar mass is the weight of one mole (or 6.02 x 1023 molecules) of any chemical compounds. All three of these components can complement each other when solving molar conversions, which are the steps taken to determine how many moles, atoms, grams, or molecules are in a substance. Aluminum has a density of 2.7 g/cm3, an atomic volume of 10.00 cm3, a melting point of 660.32 °C, and a boiling point of 2519 °C. The molar mass of aluminum is 26.98 g/mol. Aluminum has 13 protons, 13 electrons, and 14 neutrons. The objective of this lab was for students to determine the thickness of household and heavy-duty aluminum foil and how many atoms are in each type of foil. There were 4.2 x 1023 atoms in the household aluminum foil that was tested and it had a thickness of 0.0018 cm3. There were 5.1 x 1022 atoms in the heavy-duty aluminum that was tested and it had a thickness of 0.0027 cm3. Understanding the purpose of this lab provides further help with molar conversions of atoms and help with understanding the thickness between the two types of foil.
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