A single aluminum drink can weighs 0.0328 pounds. How many Al atoms are in this drink can?
3.33 x 1023 atoms Al
1.61 x 1018 atoms Al
1.61 x 1024 atoms Al
0.553 atoms Al
Answers
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Given:
- The mass of the aluminium drink (w) = 0.0328 pounds
- One pound = 453 g
- Molar mass of Aluminium (Mm) = 27 g/mol
- Avogadro's number (NA) = 6.023*10²³
To find:
The number of aluminium atoms in the drink.
Solution:
- The mass of the aluminium in grams (w) = 0.0328*453 = 14.85 g
- The number of moles of aluminium (n) = w/Mm = 14.85/27 = 0.55
- One mole of any substance contains Avogadro's number of particles. So, the number of aluminium atoms in the drink = 0.55*NA = 3.33*10²³
Answer:
The number of aluminium atoms in the drink is equal to 3.33*10²³
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The number of Al atoms are in this drink can is 3.31 × 10³³ atoms
Explanation:
The mass of the Al atoms = 0.0328 pounds = w = 0.0328 × 453 = 14.87 g
The molar mass of aluminum = 27 g/mol
The number of moles in aluminium = n = w/M
On substituting the values, we get,
n = 14.87/27 = 0.55 moles
The number of Al atoms is given as:
Number of atoms = n × Avagrado number
Number of atoms = 0.55 × 6.023 × 10²³
∴ Number of atoms = 3.31 × 10²³ atoms
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