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Approximately how many atoms of silicon and oxygen would be in a cube of silicon dioxide 0.5 mm on a side? (a grain of sand)

Question #146770. Asked by Walneto.
Last updated Apr 25 2019.
Originally posted Apr 25 2019 3:49 PM.

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brm50diboll star
Answer has 15 votes
Currently Best Answer
brm50diboll star
12 year member
37 replies avatar

Answer has 15 votes.

Currently voted the best answer.
This isn't so much an internet research question as a mathematical Chemistry question. Sand is essentially silica (SiO2), which (in my one internet search) has a density of 2.65 g/cc. 0.5 mm is 0.05 cm. A cube with a side of 0.5 mm would therefore have a volume of (0.05 cm)^3 = 0.000125 cc. The mass of this grain would be m=dV or m= 0.000125 × 2.65 = 0.00033125 g. The number of moles is the number of grams divided by the molar mass of SiO2, (which is 60.0835 g/mol), so mol = 0.00033125/60.0835 = 5.51316 × 10^(-6) mol. The number of formula units is Avogadro's number times the number of moles, or (6.022 × 10^23) × (5.51316 × 10^(-6)) = 3.320 × 10^18 formula units. There is one silicon atom per formula unit, and two oxygen atoms per formula unit in SiO2, so:

Number of silicon atoms = 3.320 × 10^18
Number of oxygen atoms = 6.640 × 10^18

link https://www.quora.com/What-is-the-density-of-silica-sand

Response last updated by brm50diboll on Apr 25 2019.
Apr 25 2019, 4:54 PM
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