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28. Aluminum is a metal with a high strength-to-mass ratio and a high corrosion resistance; thus, it is often used forrnstructural purposes. Calculate both the number of moles of atoms and the number of atoms in a 10.0-g sample ofrnaluminum.
Accepted Answer
Here's how to calculate the moles and atoms in a 10.0 g sample of aluminum:
1. Moles:
- Find the molar mass of aluminum (Al) from the periodic table: 26.98 g/mol.
- Divide the mass of the sample by the molar mass:
moles of Al = (10.0 g) / (26.98 g/mol) = 0.371 mol
2. Atoms:
- Use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles to atoms:
atoms of Al = (0.371 mol)
(6.022 x 10^23 atoms/mol) = 2.23 x 10^23 atoms
Therefore, a 10.0 g sample of aluminum contains 0.371 moles of aluminum atoms and 2.23 x 10^23 aluminum atoms.
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