The ruby shown below haas a mass of 12.15 carats (1 carat = 200.0 mg). Rubies are made of a crystalline form of Al2O3. 1.) What percentage of the mass of the ruby is aluminum? 2.) How many atoms of aluminum are in this ruby? 3.) The density of rubies is 4.02 g/cm3. What is the volume of the ruby?
Updated 121 days ago|8/3/2023 1:23:21 PM
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User: The ruby shown below haas a mass of 12.15 carats (1 carat = 200.0 mg). Rubies are made of a crystalline form of Al2O3. 1.) What percentage of the mass of the ruby is aluminum? 2.) How many atoms of aluminum are in this ruby? 3.) The density of rubies is 4.02 g/cm3. What is the volume of the ruby?

Weegy:

Updated 121 days ago|8/3/2023 1:23:21 PM
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1.) The percentage of aluminum in Al2O3 is: 52.93%.
The formula for aluminum oxide is Al2O3, which means that there are two aluminum atoms for every three oxygen atoms. The atomic mass of aluminum is 26.98 g/mol and the atomic mass of oxygen is 16.00 g/mol. Therefore, the molar mass of Al2O3 is (2 x 26.98 g/mol) + (3 x 16.00 g/mol) = 101.96 g/mol x 100% = 52.93%.

2.) The number of atoms of aluminum in the ruby is 2.87 x 10^22 atoms.
The mass of the ruby is 12.15 carats x (200 mg / carat) = 2430 mg = 2.43 g. The number of moles of Al2O3 in the ruby is 2.43 g / (101.96 g/mol) = 0.0238 mol. Since there are two aluminum atoms per formula unit of Al2O3, the number of moles of aluminum in the ruby is 0.0238 mol x 2 = 0.0476 mol. 0.0476 mol x (6.022 x 10^23 atoms/mol) = 2.87 x 10^22 atoms.

3.) 0.604 cm^3 - is the volume of the ruby.
The volume of the ruby can be calculated using its mass and density: volume = mass / density = (2.43 g) / (4.02 g/cm^3) = 0.604 cm^3.

Added 121 days ago|8/3/2023 1:23:21 PM

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