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cluponka
10 days ago
5

Molybdenum (Mo) has a BCC crystal structure, an atomic radius of 0.1363 nm, and an atomic weight of 95.94 g/mol. Compute and com

pare its theoretical density with the experimental value found inside the front cover of the book.
Physics
2 answers:
Ostrovityanka [2.1K]10 days ago
8 0

Answer:

The book is titled Solid State or Condensed Matter

Explanation:

Yuliya22 [2.4K]10 days ago
8 0

Answer

The experimental value is 10.78 g/cm³

Explanation:

The density formula yields \frac{mass}{volume}

In a BCC structure for Mo, there are 9 atoms, and the cell edge length (a) is twice the atomic radius (

r).

a = 9, r = 0.1363 nm = 1.363 A

Therefore, a = 2 × 9 r = 18r

The total volume of atoms = a^{3} = (18r)^{3} = 5832(1.363)^{3}= 14, 767.434 cm^{3}

The molar mass of Mo is 95.95 g/mol

Thus, the density can be calculated as \frac{95.95 g/mol}{14, 767.4355 cm^{3} } × \frac{1 mol}{6.022*10^{23} atoms Mo }

= 1.0788 ×

= 10.79E1810^{20}

resulting in a density of 10.79 g/cm³ (experimental density).

The theoretical density is noted as 10.22 g/cm³.

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Refer to the diagram below.

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