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Question: A metal crystallizes in a bcc lattice. Its unit cell edge length is about 300 pm and its molar mass ...

A metal crystallizes in a bcc lattice. Its unit cell edge length is about 300 pm and its molar mass is about 50gmol−1.mol^{- 1}. What would be density of the metal?

A

6.2gcm−36.2gcm^{- 3}

B

3.1gcm−33.1gcm^{- 3}

C

9.3gcm−39.3gcm^{- 3}

D

12.4gcm−312.4gcm^{- 3}

Answer

6.2gcm−36.2gcm^{- 3}

Explanation

Solution

For bcc, Z = 2

d=Z×Ma3×NAd = \frac{Z \times M}{a^{3} \times N_{A}}

d=2×50(300×10−10)3×6.023×1023=6.2gcm−3d = \frac{2 \times 50}{(300 \times 10^{- 10})^{3} \times 6.023 \times 10^{23}} = 6.2gcm^{- 3}